At 20°C a gas has a volume of 16.00 L. What will the volume be at 175.0 °C?

Answer:

physical change, because a new substance is not formed

Explanation:

Answer:

4) physical change, because a new substance is not formed

a physical change is where you can change the look and feel of whatever and get it back to what it was before but a chemical change. is a change where you can not get back to what it was originally

Explanation:

please give me brainliest

The correct statement is: the most probable molecular speed decreases as the molar mass of the gas increases. The relationship observed between the most probable molecular speed and the molar mass of the gas is that the most probable molecular speed decreases as the molar mass of the gas increases. This is because heavier molecules have more inertia and therefore move more slowly than lighter molecules. So, the larger the molar mass, the slower the molecular speed.

This relationship can be explained by the equation for the most probable molecular speed (V_p), which is derived from the Maxwell-Boltzmann distribution:

V_p = √(2 * R * T / M)

where:
- V_p is the most probable molecular speed
- R is the ideal gas constant
- T is the temperature in Kelvin
- M is the molar mass of the gas

As you can see from the equation, the most probable molecular speed (V_p) is inversely proportional to the square root of the molar mass (M). This means that when the molar mass increases, the most probable molecular speed decreases, and vice versa.

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The relationship observed between the most probable molecular speed and the molar mass of the gas is the most probable molecular speed decreases as the molar mass of the gas increases.

This relationship can be explained by the following steps:
1. Molecular speed refers to the velocity of individual molecules in a gas sample.
2. Molar mass is the mass of one mole of a substance, usually expressed in grams per mole (g/mol).
3. The most probable molecular speed can be estimated using the Maxwell-Boltzmann distribution, which describes the distribution of molecular speeds in a gas.
4. According to this distribution, lighter molecules (with lower molar mass) tend to have higher molecular speeds than heavier molecules (with higher molar mass) at the same temperature.
5. Therefore, as the molar mass of a gas increases, the most probable molecular speed decreases.

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The total number of joules of heat energy needed to raise the temperature of 10 grams of water from 20°C to 30°C is 418.4 J. The specific heat capacity of water is 4.184 J/g·°C.

To find the total heat energy needed, we can use the formula:

Q = m·c·ΔT

where:

Q = heat energy (in Joules)

m = mass of the water (in grams)

c = specific heat capacity of water (4.184 J/g·°C)

ΔT = change in temperature (in °C)

Substituting the values given, we get:

Q = 10 g × 4.184 J/g·°C × (30°C - 20°C)

Q = 418.4 J

Therefore, the total number of joules of heat energy needed to raise the temperature of 10 grams of water from 20°C to 30°C is 418.4 J.

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The concentrations of major species in a mixture of weak and strong acids and bases are determined by their dissociation behavior and interaction in a solution, influencing the overall pH and buffering capacity.

The relationship among the concentrations of major species in a mixture of weak and strong acids and bases can be understood through their dissociation and interaction in a solution.

Strong acids, such as HCl, fully dissociate in water, releasing a high concentration of H+ ions. Similarly, strong bases, like NaOH, dissociate completely, releasing a high concentration of OH- ions.

Weak acids, such as acetic acid (CH3COOH), only partially dissociate in water, releasing a smaller concentration of H+ ions. Likewise, weak bases, like ammonia (NH3), partially dissociate, releasing a smaller concentration of OH- ions.

When a mixture of weak and strong acids and bases is present, the strong species will react first due to their higher concentrations of H+ or OH- ions. This reaction will affect the pH of the solution, as well as the concentrations of the weak species, as they will be buffered by the strong species.

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When solid mercury(I) chloride (Hg₂Cl₂) reacts with ammonia (NH₃), two precipitates form: white mercurous ammonium chloride (HgNHCl) and black mercuric nitride (Hg₃N₂).

The chemical equation for the reaction is:

Hg₂Cl₂(s) + 2NH₃(aq) → HgNH₂Cl(s) + Hg₃N₂(s) + 2HCl(aq)

The first precipitate, mercurous ammonium chloride, is a white solid that forms because of the reaction between Hg₂Cl₂ and NH₃. It is also known as white precipitate and has a molecular formula of HgNH₂Cl.

The second precipitate, mercuric nitride, is a black solid that forms because of the reaction between the excess ammonia and the Hg²⁺ ions produced by the Hg₂Cl₂. The molecular formula of mercuric nitride is Hg₃N₂.

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The molar mass of the unknown gas is 27.0 g/mol.

According to the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. At STP, the pressure is 1 atm, the volume is 2.5 L, and the temperature is 273.15 K.

To find the number of moles of gas present, we can rearrange the ideal gas law equation to solve for n:

n = PV/RT

Substituting the values at STP, we get:

n = (1 atm) x (2.5 L) / [(0.08206 L atm/mol K) x (273.15 K)]

n = 0.1018 moles

The difference in weight between the gas-filled vessel and the evacuated vessel is 2.75 g, which is the weight of 0.1018 moles of the unknown gas.

So the molar mass of the gas can be calculated as:

molar mass = mass / moles

molar mass = 2.75 g / 0.1018 mole

molar mass = 27.0 g/mol

Therefore, the molar mass of the unknown gas is 27.0 g/mol.

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The molar mass of the unknown gas is 27.0 g/mol.

According to the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. At STP, the pressure is 1 atm, the volume is 2.5 L, and the temperature is 273.15 K.

To find the number of moles of gas present, we can rearrange the ideal gas law equation to solve for n:

n = PV/RT

Substituting the values at STP, we get:

n = (1 atm) x (2.5 L) / [(0.08206 L atm/mol K) x (273.15 K)]

n = 0.1018 moles

The difference in weight between the gas-filled vessel and the evacuated vessel is 2.75 g, which is the weight of 0.1018 moles of the unknown gas.

So the molar mass of the gas can be calculated as:

molar mass = mass / moles

molar mass = 2.75 g / 0.1018 mole

molar mass = 27.0 g/mol

Therefore, the molar mass of the unknown gas is 27.0 g/mol.

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The lambda max (λmax) of an azo color is the wavelength at which the color retains light most unequivocally.

It is decided by the electronic structure of the color atom, which in turn depends on the nature and position of the chromophores and auxochromes within the atom.

A chromophore could be a gathering of iotas in an atom that retains light due to the nearness of delocalized π electrons.

An autochrome may be a gathering of molecules in an atom that changes the electronic properties of the chromophore and impacts the absorption spectrum of the particle.

In azo dyes, the chromophore is the azo gather (-N=N-), which incorporates a tall molar termination coefficient and assimilates emphatically within the unmistakable locale of the electromagnetic range.

The auxochromes are ordinarily fragrant rings, amino bunches, or carboxylic corrosive bunches, which can give or pull back electrons from the chromophore and move the λmax of the color.

When a coupling reagent is included in an azo color response, it responds with a diazonium salt to make an unused azo color. The structure of the coupling reagent can influence the λmax of the coming about color by modifying the electronic properties of the chromophore.

For case, a coupling reagent with an electron-donating gather can increment the electron thickness on the chromophore and move the λmax to a longer wavelength, while a coupling reagent with an electron-withdrawing bunch can diminish the electron thickness on the chromophore and move the λmax to a shorter wavelength.

The number of fragrant rings within the nucleophile can moreover influence the λmax of the azo dye. Fragrant rings are electron-rich and can give electrons to the chromophore, expanding its electron thickness and moving the λmax to a longer wavelength.

Hence, a nucleophile with different fragrant rings will have a more prominent impact on the λmax of the color than a nucleophile with only one fragrant ring.

In rundown, both the conjugation of the coupling reagent and the number of fragrant rings within the nucleophile can impact the electronic structure of the azo color and move its λmax.

Be that as it may, the impact of the nucleophile is ordinarily more critical since it specifically influences the electron thickness of the chromophore. 

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As the compression is carried out quasi-statically, the gas's temperature will not change during the process. The temperature of the gas is T= 60.65 K.

The temperature of the gas will remain constant during the compression process since it is being done quasi-statically.

This means that the temperature of the gas will remain constant throughout the compression process.

Since the amount of work (500 J) is given, the temperature of the gas can be determined using the equation U = (3/2)nRT, where U is the work, n is the number of moles, R is the ideal gas constant, and T is the temperature.

Solving for T, we find that the temperature of the gas is T = (2/3)(500 J)/(0.50 mol)(8.31 J/mol K) = 60.65 K.

Complete Question:

It takes 500 J of work to compress 0.50 mol of an ideal gas quasi-statically to one-fifth its original volume. What is the temperature of the gas, assuming it remains constant during the compression?

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The volume of 4.50 moles of nitrogen gas at STP is approximately 101 L. So, the correct answer is 101 L.

At STP (standard temperature and pressure), the volume of one mole of any gas is 22.4 liters. Therefore, to find the volume of 4.50 moles of nitrogen gas at STP, we can simply multiply the number of moles by the molar volume:

At STP (Standard Temperature and Pressure), the volume of 4.50 moles of nitrogen gas (N2) can be calculated using the ideal gas law:

PV = nRT

Where P is the pressure (which is 1 atm at STP), V is the volume, n is the number of moles, R is the gas constant, and T is the temperature (which is 273.15 K at STP).

Rearranging this equation to solve for V, we get:

V = (nRT)/P

Substituting the values for n, R, P, and T, we get:

V = (4.50 mol x 0.08206 L atm K^-1 mol^-1 x 273.15 K)/1 atm

V = 101.3 L

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Answer:

a.) Instead of configuring all up before some down, all of the configurations were placed as up and down, leaving two spots empty in the 2p sublevel.

b.) There is a missing s sublevel for row 3.

c.) There are two up arrows in one of the lines.

d.) When you get to the "d" section you must subtract the number you're using by 1. So, it's supposed to be 2d to the power of 10.

CH4 has only sigma bonds between the carbon and hydrogen atoms, and no pi bonds.

The answer is (E) CH4.

Pi bonding refers to the sharing of electrons between two atoms that occurs when two atomic orbitals with parallel electron spins overlap. Pi bonds are formed by the sideways overlap of two p orbitals.

In the given options, all except CH4 have pi bonds:

(A) CO2 has two pi bonds between the carbon atom and the oxygen atoms.
(B) C2H4 has a double bond between the two carbon atoms, which consists of one sigma bond and one pi bond.
(C) CN− has a triple bond between the carbon and nitrogen atoms, consisting of one sigma bond and two pi bonds.
(D) C6H6 has six pi bonds due to the delocalized pi electron system in the benzene ring.

In contrast, CH4 has only sigma bonds between the carbon and hydrogen atoms, and no pi bonds.

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The volume of a solution, prepared by diluting a 1.0 L solution of 0.40 M KOH to 0.13 M is approximately 3.08 liters.

To calculate the volume of a solution, in liters, prepared by diluting a 1.0 L solution of 0.40 M KOH to 0.13 M, you can use the dilution formula:

M1V1 = M2V2

where M1 is the initial molarity of the solution (0.40 M), V1 is the initial volume of the solution (1.0 L), M2 is the final molarity of the solution (0.13 M), and V2 is the final volume of the solution (in liters) that we need to find.

Rearrange the formula to solve for V2:

V2 = (M1V1) / M2

Now, plug in the given values:

V2 = (0.40 M * 1.0 L) / 0.13 M

V2 = 0.40 L / 0.13

V2 ≈ 3.08 L

So, the volume of the diluted solution is approximately 3.08 liters.

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The volume of the solution after dilution is approximately 3.08 liters.

To calculate the volume of the solution, we can use the formula:

V1C1 = V2C2

where V1 is the initial volume, C1 is the initial concentration, V2 is the final volume, and C2 is the final concentration.

Plugging in the values given in the question, we get:

(1.0 L)(0.40 M) = V2(0.13 M)

Solving for V2, we get:

V2 = (1.0 L)(0.40 M) / (0.13 M) = 3.08 L

Therefore, the volume of the solution, in liters, prepared by diluting a 1.0 L solution of 0.40 M KOH to 0.13 M is 3.08 L.
Hi! I'd be happy to help you calculate the volume of the solution. To do this, we'll use the dilution formula:

C1V1 = C2V2

where C1 and V1 represent the initial concentration and volume, and C2 and V2 represent the final concentration and volume.

1. Plug in the given values:
C1 = 0.40 M (initial concentration of KOH)
V1 = 1.0 L (initial volume of the solution)
C2 = 0.13 M (final concentration of KOH)

2. Rearrange the formula to solve for V2:
V2 = (C1V1) / C2

3. Substitute the values into the formula:
V2 = (0.40 M × 1.0 L) / 0.13 M

4. Calculate V2:
V2 ≈ 3.08 L

So, the volume of the solution after dilution is approximately 3.08 liters.

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The number of moles of acid and base that react depends on the stoichiometry of the chemical reaction and the amounts of reactants used

Without additional information about the chemical reaction or system being referred to, we cannot determine the number of moles of acid and base that reacted.

If we assume that the orange spheres represent sulfate ions in a specific reaction, then we would need to know the stoichiometry of the reaction to determine the number of moles of acid and base that reacted.

For example, if the reaction involved sulfuric acid ([tex]H_2SO_4[/tex]) and sodium hydroxide (NaOH) and the orange spheres represent sulfate ions ([tex](SO_4)^{2-[/tex]), then the balanced chemical equation would be:

[tex]H_2SO_4 + 2NaOH - > Na_2SO_4 + 2H_2O[/tex]

In this case, we would need to know the amount of sodium hydroxide used to determine the number of moles of acid and base that reacted. If we know the number of orange spheres representing sulfate ions and the amount of sodium hydroxide used, we can determine the moles of acid and base that reacted.

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The heat capacity of 28.4 g of water is 118.8976 J/°C. The closest option to this answer is option b) 119 J/°C.

To calculate the heat capacity of 28.4 g of water, we need to use the formula:

Heat capacity = mass x specific heat

where mass is given as 28.4 g and specific heat of water is given as 4.184 J/g.°C.

So, substituting the values in the formula, we get:

Heat capacity = 28.4 g x 4.184 J/g.°C
Heat capacity = 118.8976 J/°C


To calculate the heat capacity of 28.4 g of water, you need to multiply the mass of water (m) by its specific heat (c). The formula for heat capacity (Q) is:

Q = m × c

Given:
m = 28.4 g
c = 4.184 J/g.°C

Substitute the values and perform the calculation:

Q = 28.4 g × 4.184 J/g.°C = 118.8 J/°C

The closest answer among the given options is:

b) 119 J/°C

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The average repeat unit molecular weight for average molecular weight of 229,500 g/mol and a number degree of polymerization of 4,000 is equals to the 57.4 g/mol. So, option(c) is right one.

Polymers are large molecules made up of repeating structural units linked together. The degree of polymerization (DP) is the number of repeating units in the polymer molecule. The average molecular weight is the degree of polymerization (MP) multiplied by the molecular weight of the repeat unit (m) is written as [tex] \bar M_n = (DP)(m)[/tex]

We have a random copolymer produced by polymerization of vinyl chloride and propylene.

Average molecular weight= 229500 g/mol

Number degree of polymerization = 4000

Using the above formula, the average repeat unit molecular weight = 229500 g/mol/ 4000

= 57.37 ~ 57.4 g/mol

Hence, required value is 57.4 g/mol.

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Answer:

combustion

respiration by humans

Explanation:

burning of wood leaves release carbon dioxide which is a green house gas and detrimental to the climate

, the molar concentration of the solution is 2.202 M. molar concentration of a solution that contains 45.0 g of nacl dissolved in 350.0 ml of water

To calculate the molar concentration of a solution, we need to first determine the number of moles of the solute present in the solution, and then divide that by the volume of the solution in liters.

The molar mass of NaCl is 58.44 g/mol. Therefore, the number of moles of NaCl in 45.0 g can be calculated as:

mole= mass / molar mass = 45.0 g / 58.44 g/mol = 0.7709 mol

Next, we need to convert the volume of the solution from milliliters to liters:

volume = 350.0 ml = 0.3500

Finally, we can calculate the molar concentration (M) of the solution as:

M = moles / volume = 0.7709 mol / 0.3500 L = 2.202 M

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Answer:

Answer (Detailed Solution Below)

Explanation:

Option 3 : Substance in solid phase has the least entropy.

The pair of elements that are nonmetals and gases at room temperature and normal atmospheric pressure are:

Oxygen (O₂) - Oxygen is a nonmetal that exists as a diatomic gas at room temperature and normal atmospheric pressure. It is colorless, odorless, and tasteless.

Nitrogen (N₂) - Nitrogen is another nonmetal that exists as a diatomic gas at room temperature and normal atmospheric pressure. It is also colorless, odorless, and tasteless.

Both oxygen and nitrogen are essential components of the Earth's atmosphere, with nitrogen making up about 78% of the air we breathe and oxygen making up about 21%.

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It depends on what you meant by saying not visible. Of it is not visible by using accurate measuring equipment then I think so, but if you mean that all transparent water is drinkable, then no. Think about this. When you put salt in water, you can't see it but it is still there: if you taste the water you can tell that there's salt in there. Let's say that instead of salt there are some bacteria, or some other type of salt which is not appropriate to drink at high levels, such as nitrates. I personally wouldn't recommend drinking from any type.of water unless you are not sure about its purity

we need to use the atomic weight of lead to convert the given weight in grams to moles. The atomic weight of lead is 207.2 g/mol.

First, let's convert the given weight in pounds to grams: 1.00 lb = 454 g
Next, let's calculate the number of moles of lead atoms in 454 g of lead: moles of lead atoms = (454 g) / (207.2 g/mol) = 2.19 mol.

Therefore, there are 2.19 moles of lead atoms in 1.00 lb (454g) of lead. To calculate the number of moles of atoms in 1.00 lb (454g) of lead, you need to use the formula: moles = mass (g) / molar mass (g/mol)

The molar mass of lead (Pb) is 207.2 g/mol. Using the given mass of 454g, the calculation is as follows:
moles = 454g / 207.2 g/mol = 2.19 moles
So, there are 2.19 moles of atoms in 1.00 lb (454g) of lead.

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To determine how many moles of atoms are there in 1.00 lb (454g) of lead, you'll need to follow these steps:

Step 1: Convert weight to grams.
1.00 lb of lead is already given as 454g.

Step 2: Find the molar mass of lead.
Lead (Pb) has a molar mass of approximately 207.2 g/mol.

Step 3: Calculate the number of moles.
To find the moles, divide the mass of lead (454g) by its molar mass (207.2 g/mol).

Moles = 454g / 207.2 g/mol

Your answer: There are approximately 2.19 moles of atoms in 1.00 lb (454g) of lead.

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The formation of ions is an essential process in chemistry and is involved in many chemical reactions and compounds.

Atoms are composed of protons, neutrons, and electrons. The number of protons in an atom determines its atomic number and the element it represents. The electrons in an atom occupy different energy levels or shells, and these electrons participate in chemical reactions. The outermost shell of electrons, called the valence shell, is particularly important in chemical reactions because it determines the chemical properties of the atom.

When an atom gains or loses electrons, it becomes charged and is called an ion. The process of gaining or losing electrons is called ionization. When an atom loses one or more electrons, it becomes a positively charged ion called a cation. Cations have a smaller number of electrons than protons and have a net positive charge. For example, when the element sodium (Na) loses one electron, it becomes a sodium ion (Na+).

On the other hand, when an atom gains one or more electrons, it becomes a negatively charged ion called an anion. Anions have a larger number of electrons than protons and have a net negative charge. For example, when the element chlorine (Cl) gains one electron, it becomes a chloride ion (Cl-).

The formation of ions is a fundamental process in many chemical reactions. Ions can combine with each other to form ionic compounds, which are compounds composed of ions held together by electrostatic forces. For example, sodium ions (Na+) and chloride ions (Cl-) can combine to form sodium chloride (NaCl), which is common table salt.

Overall, the formation of ions is an essential process in chemistry and is involved in many chemical reactions and compounds.

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(a) If one of the reaction products was the then unknown neutron, what was the other product is the C -12.

(b) The q-value of this reaction is the 5.9 × 10⁸ J.

The James Chadwick was discovered the neutron during the experiment involving the nuclear reaction in that the beryllium, bombarded with the alpha particles. The equation of the reaction is as :

⁴Be₉  +  ²He₄  ---->  ⁶C₁₂  +  ⁰n₁

(a) If one of the reaction products was the then unknown neutron, what was the other product is the C -12.

(b) The q-value of this reaction is as :

q = mc²

Where,

The m is the mass

The c is the speed of the light.

m = 4.002603 + 2.014102

m = 1.988501

q = 1.988501  × 3 × 10⁸

q = 5.9 × 10⁸ J

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The sample of pure carbon would contain approximately 2.135 x 10²⁴ carbon atoms.

The majority of carbon atoms—98.93%—have masses of 12 atomic mass units. A mass of 13.00 atomic mass units is present in 1.07% of the carbon atoms. 14.) Identify one distinction between the nuclei of carbon-12 and carbon-13 atoms in terms of the subatomic particles that can be discovered there.

First, using the atomic mass of carbon, we must determine how many moles of carbon are present in the sample:

1 mole of carbon atoms = 12.01 g of carbon atoms (atomic mass of carbon)

42.552 g of carbon atoms / 12.01 g/mol = 3.545 moles of carbon atoms

Using Avogadro's number, we can then determine how many carbon atoms are present in the sample:

Number of carbon atoms = 3.545 moles of carbon atoms x 6.022 x 10²³ atoms/mole

Number of carbon atoms = 2.135 x 10²⁴ atoms

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The equator of the sun rotates faster than the poles.

The equator of the sun rotates faster than its poles. This is known as differential rotation, and it is due to the fact that the sun is not a solid body, but is composed of gas and plasma. The equatorial regions of the sun rotate faster because they are farther from the center of the sun, where the gravitational pull is stronger, and thus experience less resistance to their motion.

The period of rotation of the equator of the sun is shorter than that of the poles. The equator rotates once every 25.4 days, while the poles rotate once every 36 days.

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A pure substance (such as H₂O or iron) can only exist in three phases (solid, liquid, and gas) - True.

A kind of matter with a predictable chemical composition and physical characteristics is referred to as a chemical substance. According to certain texts, a chemical compound cannot be physically divided into its component parts without rupturing chemical bonds. Chemical compounds, alloys, and simple substances (substances made up of a single chemical element) are all examples of chemical substances.

To distinguish them from mixes, chemical compounds are frequently referred to as 'pure'. Pure water is a popular illustration of a chemical substance; regardless of whether it is separated from a river or created in a lab, it has the same characteristics and hydrogen to oxygen ratio. Other chemicals that are frequently found in their purest forms are refined sugar (sucrose), gold, table salt (sodium chloride), and diamond (carbon). In reality, though, no material is completely pure, and chemical purity is determined by the chemical's intended application.

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The number of moles of H₂ that can be produced from x grams of Mg is (x / 24.31)

The balanced chemical equation for the reaction between Mg and HCl is,

Mg + 2HCl → MgCl₂ + H₂

This equation shows that 1 mole of Mg reacts with 2 moles of HCl to produce 1 mole of H₂. Therefore, the number of moles of H₂ that can be produced from x grams of Mg can be calculated as follows:

Calculate the number of moles of Mg in x grams:

Number of moles of Mg = mass of Mg / molar mass of Mg

Number of moles of Mg = x / 24.31

Use the mole ratio between Mg and H₂ to calculate the number of moles of H₂ produced:

Number of moles of H₂ = Number of moles of Mg × (1 mole of H₂ / 1 mole of Mg)

Number of moles of H₂ = (x / 24.31) × (1/1)

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Answer:

mass of NH₃ formed when 22g of H₂ react completely = 124.67 grams

Explanation:

3H₂ + N₂ → 2NH₃

The ratio of coefficients of reactants and products in the above reaction equation (3 : 1 : 2), is known as the stoichiometry of the reaction.

A stoichiometric amount of a reagent is the the optimum amount or ratio where, assuming that the reaction proceeds to completion, all of the reagent is consumed, there is no deficiency of the reagent, and there is no excess of the reagent. Thus if the stoichiometry of a reaction is known, as well as the mass of one of the substances, then it is possible to calculate the mass of any of the other substances.

The mole is a unit of amount of substance established by the International System of Units, to make expressing amounts of reactant or product in a reaction more convenient. As defined by Avogadro's Constant, a mole is 6.022×10²³ amounts of something. The mole is used in stoichiometric calculations, instead of the mass.

To convert from mass to moles, we need to divide the mass present in grams, by the molar mass of the substance (the sum of the molar masses of the individual elements comprising the compound), in g/mol, to get the moles. This can be represented by the formula: n = m/M, where n = number of moles, m = mass, M = molar mass.

So if we have 22 g of H₂ gas, which reacts completely, and therefore is a stoichiometric amount, then converting this to moles:

n(H₂) = m/M = 22/2 = 11 mol.

Using our stoichiometry, we can see that the ratio of H₂ to NH₃ = 3 : 2.

Therefore, for every 3 moles of H₂ used, we produce 2 moles of NH₃.

n(NH₃) = 2/3 × n(H₂) = 2/3 × 11 = 7.333 mol.

Finally, converting moles back to mass we get:

m(NH₃) = n×M = 7.333×17 = 124.67 grams

∴ mass of NH₃ formed when 22g of H₂ react completely = 124.67 grams

The amino acid that contains the R groups that are hydrophobic are the non - polar.

The Amino acids are the building blocks of the molecules of the  proteins. These contains the one hydrogen atom and the one amine group, the one carboxylic acid group and the one side chain that is the R group will be attached to the central carbon atom.

The side chains of the non polar amino acids includes the long carbon chains or the carbon rings, which makes them bulky. These are the hydrophobic, that means they repel the water. Therefore the non-polar amino acids are the hydrophobic.

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