If the volume of a gas at -40.0°C is doubled to 80.0 L, calculate the final temperature in degrees Celsius.

Answer:

M=0.06998 mol/L

Explanation:

The independent and dependent variables are compounds and elements, respectively.

Elements and compounds make up everything in our surroundings. Knowing how things operate can aid in our ability to comprehend our surroundings.

Water is one of the chemicals listed in the table (H2O). This molecule has 3 atoms, which can be broken down into 2 hydrogen (H) atoms and 1 oxygen atom (O).

Several compounds can be created by mixing the same two elements' atoms in different ratios.

Because these elements mix in various ways and in various quantities to create unique compounds, we have a huge variety of compounds in this universe.

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To calculate the cell potential, Ecell, for the given reaction at 298K, we need to use the Nernst equation. The Nernst equation relates the cell potential to the standard cell potential, temperature, and the concentrations of the reactants and products. The Nernst equation is given as follows:

Ecell = E°cell - (RT/nF) ln(Q)

where,

Ecell = cell potential

E°cell = standard cell potential

R = gas constant (8.314 J/K.mol)

T = temperature (298 K)

n = number of electrons transferred in the balanced redox reaction

F = Faraday constant (96,485 C/mol)

Q = reaction quotient

The given reaction is a redox reaction, which involves the transfer of two electrons from Co to Ag+. The balanced half-reactions are as follows:

Co(s) → Co2+(aq) + 2 e-

Ag+(aq) + e- → Ag(s)

The standard reduction potentials for these half-reactions are:

Co2+(aq) + 2 e- → Co(s) E°red = -0.28 V

Ag+(aq) + e- → Ag(s) E°red = +0.80 V

The overall standard cell potential can be calculated by subtracting the standard reduction potential of the anode from that of the cathode:

E°cell = E°red,cathode - E°red,anode

= +0.80 V - (-0.28 V)

= +1.08 V

Now we need to calculate the reaction quotient Q using the concentrations of the reactants and products. According to the given information, [Ag+] = 0.010 M and [Co2+] = 0.015 M.

Q = ([Co2+][Ag+]^2)/([Ag+]^2)

= ([0.015][0.010]^2)/([0.010]^2)

= 0.015 M

Substituting the values in the Nernst equation, we get:

Ecell = E°cell - (RT/nF) ln(Q)

= 1.08 - (8.314 x 298 / (2 x 96485)) ln(0.015)

= 0.829 V

Therefore, the cell potential, Ecell, for the given reaction at 298K is 0.829 V.

Answer:

colloid

Explanation:

there's no explanation

[tex]CaCO_{3}[/tex]and HCl reaction chemical equation with physical states balanced [tex]CaCl_{2}[/tex] (q) + Carbon 2 (g) + H atoms Of oxygen = [tex]CaCO_{3}[/tex](s) - 2HCl (aq) (l) Water cannot dissolve calcium carbonate.

How should a chemical equation be written?

Chemical expressions and other characters are used to denote the initial substances, or reactants, which are customarily represented upon that left column of the equation and the final substances, or products, that are traditionally written on the right. From the source to the products, an arrow leads.

How is a chemical equation balanced?

"Inspection," often known as trial and error, is the quickest and most widely applicable technique for balancing chemical equations. This method can be used to effectively balance a chemical equation, as shown below.

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Taking into account definition of percent yield, the correct answer is option c): the percent yield for the reaction is 0.947.

In first place, the balanced reaction is:

CH₄ + 2 O₂ → CO₂ + 2 H₂O

By reaction stoichiometry, the following amounts of moles of each compound participate in the reaction:

The molar mass of the compounds is:

By reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

The following rule of three can be applied: if by reaction stoichiometry 16.05 grams of CH₄ form 44.01 grams of CO₂, 136 grams of CH₄ form how much mass of CO₂?

mass of CO₂= (136 grams of CH₄× 44.01 grams of CO₂)÷16.05 grams of CH₄

mass of CO₂= 372.92 grams

Then, 372.92 grams of CO₂ can be produced from 136 grams of CH₄.

The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage and this is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:

percent yield= (actual yield÷ theoretical yield)× 100%

where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product.

In this case, you know:

Replacing in the definition of percent yield:

percent yield= (353 grams÷ 372.92 grams)× 100%

Solving:

percent yield= 94.7%= 0.947

Finally, the percent yield for the reaction is 0.947.

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3.21 grams of Aluminum Sulfate are got when 4 g of Aluminum Nitrate reacts chemcially with 3 g of Sodium Sulfate.

The equation given is not balanced. Thus,  when balanced the equation becomes:

2 Al(NO₃)₃ + 3 Na₂SO₄ → Al₂(SO₄)₃ + 6 NaNO₃

The molar mass of Al(NO₃)₃ is:

Al(NO₃)₃ = 1(Al) + 3(N) + 9(O) = 213 g/mol

The molar mass of Na₂SO₄ is:

Na₂SO₄ = 2(Na) + 1(S) + 4(O) = 142 g/mol

From the balanced equation, we can see that 2 moles of Al(NO₃)₃ react with 3 moles of Na2SO4 to produce 1 mole of Al₂(SO₄)₃. Therefore, we can calculate the number of moles of Al(NO₃)₃ and Na₂SO₄ that react:

Number of moles of Al(NO₃)₃ = 4 g / 213 g/mol = 0.0188 mol

Number of moles of Na₂SO₄ = 3 g / 142 g/mol = 0.0211 mol

From the balanced equation, we can see that 2 moles of Al(NO₃)₃ produce 1 mole of Al₂(SO₄)₃. Therefore, the number of moles of Al₂(SO₄)₃ produced is:

Number of moles of Al₂(SO₄)₃ = 0.0188 mol / 2 * 1 = 0.0094 mol

The molar mass of Aluminum Sulfate (Al₂(SO₄)₃) is:

Al₂(SO₄)₃ = 2(Al) + 3(S) + 12(O) = 342 g/mol

Therefore, the mass of Aluminum Sulfate produced is:

Mass of Al₂(SO₄)₃ = Number of moles of Al₂(SO₄)₃ * Molar mass of Al₂(SO₄)₃

= 0.0094 mol * 342 g/mol

= 3.21 g

Hence, 3.21 grams of Aluminum Sulfate are liberated when 4 g of Aluminum Nitrate change state with 3 g of Sodium Sulfate.

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Answer:

Neutrons and Protons

Explanation:

Different elements can have subatomic particles of varying sizes. The size of an atom is defined by the size of its electron cloud, which is composed of electrons, and the size of its nucleus, which is composed of protons and neutrons. The atomic number and subsequently the identity of an element are determined by the number of protons in the nucleus. The quantity of protons and neutrons in the nucleus determines its size. The quantity of electrons in the electron cloud and the energy levels they are located at define its size. The size of atoms can differ depending on the element due to differences in the amount of protons, neutrons, and electrons.

252,212 Joules of energy are required to heat 100g of water from 35°C to 115°C water vapor.

To calculate the amount of energy required to heat water from 35°C to 100°C, we use the specific heat capacity of water, which is 4.18 J/(g°C). This means that it takes 4.18 Joules of energy to heat one gram of water by one degree Celsius.

So, the energy required to heat 100 g of water from 35°C to 100°C can be calculated as follows:

Q1 = m × c × ΔT

Q1 = 100 g × 4.18 J/(g°C) × (100°C - 35°C)

Q1 = 26,212 Joules

Next, we need to calculate the amount of energy required to vaporize the water at 100°C. This is done using the heat of vaporization of water, which is 2260 J/g.

So, the energy required to vaporize 100 g of water at 100°C is:

Q2 = m × Lv

Q2 = 100 g × 2260 J/g

Q2 = 226,000 Joules

Therefore, the total energy required to heat 100 g of water from 35°C to 115°C water vapor is:

Q = Q1 + Q2

Q = 26,212 Joules + 226,000 Joules

Q = 252,212 Joules

Thus, 252,212 Joules of energy are required to heat 100g of water from 35°C to 115°C water vapor.

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1. Record the current volume of NaOH in the burette.2. Add a few drops of phenolphthalein to the vinegar solution.

A solution is a method or process of resolving a problem or difficulty. It is typically a result of problem-solving, which is the process of working through details of a problem to reach a solution. Solutions are found through various methods including trial and error, research, and reasoning. When a solution is found, it is often a combination of various ideas, techniques, and strategies.

3. Titrate the solution until the endpoint is reached .4. Record the final volume of NaOH in the burette.5. Calculate the amount of NaOH consumed in the titration by subtracting the initial volume from the final volume.

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It requires 10.15 kilojoules of energy.

The term "vaporisation" (or "evaporation") often refers to the transformation of a liquid's condition into a vapour phase below its boiling point. The phrase, however, can also refer to the process of removing a solvent, independent of the temperature used.

When a body moves to exert force, it is said to be exerting work. Energy is the capacity to accomplish work. Energy is something we always need, and it can take many different forms.

If the gold is present in the liquid state, you only have to determine the latent heat of vaporization, or lvap. The empirical data for gold is 330 kJ/mol.

Q = mlvap

Q = (2 kg)(1 kmol/197 kg)(1,000 mol/1 kmol)

Q = 10.15 kJ

It needs an energy of 10.15 kilojoules

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Answer:

-191 kJ

Explanation:

The given reaction is:

N₂(g) + 3H₂(g) → 2NH₃(g) ΔH = -76.4 kJ/mol

From the balanced equation, we can see that the stoichiometric ratio between hydrogen (H₂) and ammonia (NH₃) is 3:2. This means that 3 moles of hydrogen react to produce 2 moles of ammonia.

To determine the heat energy when 5.0 g of hydrogen (H₂) burns, we need to follow these steps:

Step 1: Calculate the moles of hydrogen (H₂)

Using the molar mass of hydrogen (H₂), which is 2 g/mol, we can calculate the moles of hydrogen (H₂) in 5.0 g of hydrogen:

Moles of H₂ = Mass of H₂ / Molar mass of H₂

Moles of H₂ = 5.0 g / 2 g/mol

Moles of H₂ = 2.5 mol

Step 2: Use the stoichiometry of the reaction

Based on the stoichiometry of the reaction, we know that 3 moles of hydrogen (H₂) react to produce 2 moles of ammonia (NH₃), and the enthalpy change (ΔH) is -76.4 kJ/mol.

Step 3: Calculate the heat energy

The heat energy for 2.5 moles of hydrogen (H₂) can be calculated using the given enthalpy change (ΔH) and the stoichiometry of the reaction:

Heat energy = Moles of H₂ x ΔH

Heat energy = 2.5 mol x -76.4 kJ/mol

Heat energy = -191 kJ (rounded to three significant figures)

So, the heat energy when 5.0 g of hydrogen (H₂) burns is -191 kJ (rounded to three significant figures), and the negative sign indicates that the reaction is exothermic, releasing heat.

Light takes 20,100 seconds or 5.583 hours to travel 6.03 billion km.

To calculate the time it takes for light to travel 6.03 billion km, we can use the formula:

time = distance / speed of light

where distance is 6.03 x 10^9 km and the speed of light is approximately 299,792,458 meters per second (m/s).

First, we need to convert the distance from kilometers to meters:

distance = 6.03 x 10^9 km x 10^3 m/km = 6.03 x 10^12 m

Now we can calculate the time:

time = distance / speed of light

= 6.03 x 10^12 m / 299,792,458 m/s

= 20,107.394 seconds

To 3 significant figures, the answer is 20,100 seconds or 5.583 hours (since there are 3600 seconds in an hour).

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We can plug them into the equation above and plot the temperature of the sensor and the actual temperature against time on a graph to visualize how they change over time during the ascent of the balloon.

What is Temperature?

Temperature is a measure of the average kinetic energy of the particles in a substance, such as a solid, liquid, or gas. It is a scalar quantity that reflects the hotness or coldness of a substance. In other words, temperature indicates how much thermal energy is present in a substance.

This equation describes an exponential decay of the temperature with time. As time goes on, the temperature of the sensor decreases exponentially towards zero.

To sketch the sensor temperature and the actual temperature versus time, we would need additional information, such as the initial temperature T0, the time constant tc, and the rate of ascent V of the balloon.

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The pH of the solution can be calculated using the following steps:

Write the chemical equation for the dissociation of ethanoic acid:

CH3COOH + H2O ⇌ CH3COO- + H3O+

Write the equilibrium expression for the dissociation of ethanoic acid:

Ka = [CH3COO-][H3O+] / [CH3COOH]

Since the solution is equimolar in CH3COOH and CH3COO-, we can assume that the initial concentrations of CH3COOH and CH3COO- are equal. Let's use the variable x to represent the concentration of CH3COO- and CH3COOH in mol/L.

[CH3COOH] = x mol/L [CH3COO-] = x mol/L

Since CH3COOH is a weak acid, we can assume that only a small fraction of it dissociates in water. Let's use the variable y to represent the concentration of H3O+ ions in mol/L that are produced from the dissociation of CH3COOH. From the dissociation of ethanoic acid, we know that [CH3COO-] = [H3O+].

[CH3COO-] = y mol/L [H3O+] = y mol/L

Use the equilibrium expression to solve for the concentration of H3O+ ions:

Ka = [CH3COO-][H3O+] / [CH3COOH] 1.79 x 10^-5 = y^2 / x

Solving for y in terms of x, we get:

y = sqrt(Ka * x)

Calculate the pH of the solution using the equation:

pH = -log[H3O+]

pH = -log(y)

Substituting in the value of y from Step 5, we get:

pH = -log(sqrt(Ka * x))

Simplifying, we get:

pH = -0.5 * log(Ka * x)

Substituting in the value of Ka, we get:

pH = -0.5 * log(1.79 x 10^-5 * x)

Now we can calculate the pH for the solution by substituting the value of x as it is equimolar.

pH = -0.5 * log(1.79 x 10^-5 * x)

pH = -0.5 * log(1.79 x 10^-5 * 1)

pH = -0.5 * log(1.79 x 10^-5)

pH = 4.74

Therefore, the pH of an equimolar solution of ethanoic acid and Na+CH3COO- is 4.74.

Answer: C)Deposition (gas to solid)

Explanation: According to the phase diagram, at room temperature (25°C) and 1 atm, the sample is in the gas phase.  As the temperature decreases to 80 K, it falls below the sublimation curve. T he sublimation curve represents the conditions at which a substance can change directly from a solid to a gas or from a gas to a solid without passing through the liquid phase.

Since the sample is in the gas phase at room temperature, cooling it to 80 K would cause it to go through the process of deposition, where the gas particles directly transform into a solid without first becoming a liquid.  This is indicated by the section of the phase diagram below the sublimation curve.

K and Br since an halogen and a metal make a salt

0.02314 moles of  NO₂ can be formed from the decomposition of 1.25 g of dinitrogen pentoxide.

The balanced equation for the decomposition of dinitrogen pentoxide is:

2 N₂O₅ → 4 NO₂ + O₂

The molar mass of N₂O₅  is 108.01 g/mol.

To determine the number of moles of N₂O₅  present in 1.25 g, we use the following calculation:

moles N₂O₅  = mass / molar mass

moles N₂O₅ = 1.25 g / 108.01 g/mol

moles N₂O₅ = 0.01157 mol

From the balanced equation, we can see that 2 moles of N₂O₅  decompose to form 4 moles of NO2. Therefore, the number of moles of NO2 produced can be calculated as:

moles  NO₂ = (0.01157 mol N2O5) × (4 mol NO2 / 2 mol N2O5)

moles  NO₂ = 0.02314 mol

Therefore, 0.02314 moles of  NO₂ can be formed from the decomposition of 1.25 g of dinitrogen pentoxide.

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Answer: 239/94Pu → 239/95Am + 0/-1e

Explanation: The present chemical transformation involves the conversion of a neutron residing in the nucleus of the element Plutonium-239 to a proton, accompanied by the release of an electron by beta decay. The subatomic particle known as the proton remains confined within the atomic nucleus, thereby triggering a metamorphosis of the constituent element, resulting in the creation of Am-239. Meanwhile, the emission of a beta particle occurs from the nucleus.

a)  The conjugate base of aspirin (acetylsalicylic acid) is formed when the acidic proton (H+) is removed from the carboxylic acid group (-COOH) in the molecule.

b)  More aspirin will be available for absorption in the duodenum (97%) compared to the stomach (12%).

a. The conjugate base of aspirin (acetylsalicylic acid) is formed when the acidic proton (H+) is removed from the carboxylic acid group (-COOH) in the molecule.

b. The percentage of aspirin available for absorption depends on the degree of ionization of the molecule, which is related to the pH of the surrounding medium. At pH values below the pKa (2.97), most of the molecules exist in the protonated form (HA), while at pH values above the pKa, most of the molecules exist in the deprotonated form (A-).

Using the Henderson-Hasselbalch equation:

pH = pKa + log([A-]/[HA])

We can calculate the ratio of deprotonated (A-) to protonated (HA) forms at different pH values. At pH 2.0, the ratio is:

2.0 = 2.97 + log([A-]/[HA])

log([A-]/[HA]) = -0.97

[A-]/[HA] = 0.12

So, at pH 2.0, only 12% of the aspirin molecules are in the deprotonated form and available for absorption.

At pH 4.5, the ratio is:

4.5 = 2.97 + log([A-]/[HA])

log([A-]/[HA]) = 1.53

[A-]/[HA] = 31.6

So, at pH 4.5, 97% of the aspirin molecules are in the deprotonated form and available for absorption.

Therefore, more aspirin will be available for absorption in the duodenum (97%) compared to the stomach (12%).

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The addition of concentrated HCl to the equilibrium mixture will result in the precipitation of more NH₄Cl(s) as the equilibrium shifts towards the left. This can be observed as cloudiness or precipitation forming in the solution.

When concentrated hydrochloric acid (HCl) solution is added to the equilibrium mixture of NH₄Cl(s) + heat <=> NH₄+(aq) + Cl-(aq), the equilibrium will shift towards the left, meaning more solid NH₄Cl will be formed.

This is because HCl is a strong acid that will react with NH₄+ ion to form NH₄Cl(s) and H+ ion:

NH₄+(aq) + Cl-(aq) + HCl(aq) → NH₄Cl(s) + H₂O(l)

The increase in H+ ion concentration due to the addition of HCl will result in the shift of the equilibrium to the left to reduce the excess H+ ion concentration. This will favor the formation of more solid NH₄Cl.

Therefore, the addition of concentrated HCl to the equilibrium mixture will result in the precipitation of more NH₄Cl(s) as the equilibrium shifts towards the left. This can be observed as cloudiness or precipitation forming in the solution.

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1.8 moles of water are formed when 1.20 moles of ammonia reacts

How is ammonia used?

Ammonia produced by industry is used as fertilizer in agriculture to the tune of 80%. In addition to these uses, ammonia is used to make polymers, explosives, textiles, insecticides, dyes, and other compounds. It is also used to purify water sources.

Ammonia is a colorless, intensely unpleasant gas with a pungent, choke-inducing smell. It readily dissolves in water to produce an ammonium hydroxide solution that can irritate the skin and burn. Ammonia gas is easily compressed and, when put under pressure, turns into a clear, colorless liquid.

4 NH₃ + 5 O₂ → 4 NO + 6 H₂O

4 moles of ammonia gives 6 moles of water

Moles of H₂O = 1.2 moles of NH₃ x 6 moles of H₂O/4 moles of NH₃

Moles of H₂O = 1.8moles

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The concentrations of all species in a 0.510 M NaCH₃COO (sodium acetate) solution: [Na+]= 0.510 M , [OH-]= 1.8x10⁻⁵ M , [H₃O+]= 1.8x10⁻⁵ M , [CH₃COO-]= 0.510 M and [CH₃COOH]= 0.510 - (1.8x10⁻⁵) = 0.50982 M.

Concentration is the ability to focus your attention on a single task or thought for a prolonged period of time. It involves being able to ignore distractions and to be able to work through any difficulties or obstacles that may arise. Concentration is an important skill to master in order to achieve success in any endeavor, whether it be academic, professional, or personal. Good concentration can help you to stay focused, organized, and productive. When you are able to concentrate, you can take in the information needed to make better decisions and solve problems. Concentration is a skill that can be developed with practice, such as by setting goals, breaking down tasks into smaller, manageable pieces, and avoiding distractions.

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The reaction's G value at 805 K is -2625.7 kJ.

Sulfur dioxide gas is the byproduct of the interaction between sulphur and oxygen. Sulphurous acid is created when sulphur dioxide dissolves in water. Sulfuric acid causes blue litmus paper to turn red. Non-metal oxides typically have an acidic character.

ΔG = ΔH - TΔS

where ΔH is the enthalpy change, ΔS is the entropy change, T is the temperature in Kelvin, and ΔG is the change in Gibbs free energy.

Substituting the given values:

ΔG = -2374 kJ - (805 K)(312.2 J/K)

ΔG = -2374 kJ - 251717 J

ΔG = -2374 kJ - 251.7 kJ

ΔG = -2625.7 kJ

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Determine the amount of KOH present in the resulting solution. KOH was initially 0.00875 mol, then 0.00525 mol of it interacted with HCl. As a result, 0.00875 mole - 0.00525 mol (= 0.00350 mol of KOH is left. The resulting solution has a volume of 70.0 mL (35.0 mL plus 35.0 mL).

The titrant (NaOH), which is added gradually throughout the course of a titration, is added to the unknown substance. The equivalency point is the moment at which precisely the right quantity of titrant (NaOH) has indeed been added that react to the entire analyte (HCl).

What took place during titration: One mole of NaOH interacts with one mole of HCl inside the reaction between the two substances. NaOH with HCl equals NaCl plus H2O. (NaOH and HCl have a mole ratio of 1:1.) • The NaOH concentration is 0.1 M, or 0.1 molecules per litre.

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The new volume of the helium sample would be 2.4 L.

According to the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in kelvins.

At STP (standard temperature and pressure), which is defined as 0°C (273.15 K) and 101.325 kPa, the volume of 2.0 liters of helium gas contains one mole of helium atoms.

To find the new volume of the helium sample when the temperature is increased to 27°C (300.15 K) and the pressure is decreased to 80 kPa, we can use the following equation:

(P1V1)/T1 = (P2V2)/T2

where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature, respectively.

Plugging in the values, we get:

(101.325 kPa)(2.0 L)/(273.15 K) = (80 kPa)(V2)/(300.15 K)

Solving for V2, we get:

V2 = (101.325 kPa)(2.0 L)/(273.15 K) * (300.15 K)/(80 kPa) = 2.36 L

Therefore, the new volume of the helium sample is approximately 2.4 L (rounded to the nearest tenth).

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The percent yield of copper(I) sulfide in this experiment is 31.83%.

What is percent yield?

To calculate the percent yield, we need to compare the actual yield (the amount of product that was obtained in the experiment) with the theoretical yield (the amount of product that should have been obtained if the reaction had gone to completion).

The balanced chemical equation for the reaction between copper and sulfur to form copper(I) sulfide is:

Cu + S →  [tex]Cu_{2}S[/tex]

The molar mass of Cu is 63.55 g/mol, and the molar mass of S is 32.06 g/mol. The molar mass of  [tex]Cu_{2}S[/tex]  is 159.17 g/mol.

First, we need to calculate the theoretical yield of copper(I) sulfide using the amount of copper used in the experiment:

5 g Cu × (1 mol Cu / 63.55 g Cu) × (1 mol [tex]Cu_{2}S[/tex] / 1 mol Cu) × (159.17 g  [tex]Cu_{2}S[/tex] / 1 mol [tex]Cu_{2}S[/tex] ) = 12.57 g  [tex]Cu_{2}S[/tex]

So the theoretical yield of copper(I) sulfide is 12.57 g.

The actual yield obtained in the experiment is 4 g.

The percent yield is then:

percent yield = (actual yield / theoretical yield) × 100%

percent yield = (4 g / 12.57 g) × 100%

percent yield = 31.83%

Therefore, the percent yield of copper(I) sulfide in this experiment is 31.83%.

What is theoretical yield ?

The theoretical yield is the amount of product that would be obtained in a chemical reaction if it went to completion, meaning that all the limiting reactant was used up and no product was lost. It is calculated using stoichiometry, which involves balancing the chemical equation for the reaction and using the coefficients to determine the mole ratio between the reactants and products.

Theoretical yield is often used as a reference value to compare with the actual yield obtained in an experiment, which is the amount of product actually obtained from the reaction. The percent yield can then be calculated by dividing the actual yield by the theoretical yield and multiplying by 100%.

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0.1 mol of sodium hydroxide (NaOH) would react exactly with 7.5 g of the diprotic acid [tex]H_{2}[/tex]A.

What is Molar Mass?

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is calculated by adding up the atomic masses of all the atoms in a molecule or the formula mass of all the ions in an ionic compound.

The balanced chemical equation for the reaction between diprotic acid, [tex]H_{2}[/tex]A, and sodium hydroxide, NaOH, can be represented as follows:

2[tex]H_{2}[/tex]A + 2 NaOH -> [tex]Na_{2}[/tex]A + 2 [tex]H_{2}[/tex]O

From the balanced equation, we can see that 2 moles of [tex]H_{2}[/tex]A react with 2 moles of NaOH to produce 1 mole of [tex]Na_{2}[/tex]A and 2 moles of water ([tex]H_{2}[/tex]O).

First, we need to calculate the number of moles of [tex]H_{2}[/tex]A in 7.5g using the formula:

moles = mass / molar mass

moles of [tex]H_{2}[/tex]A = 7.5g / 150 g/mol = 0.05 mol

Since diprotic acid, [tex]H_{2}[/tex]A, reacts in a 1:2 ratio with NaOH, we need to multiply the moles of [tex]H_{2}[/tex]A by 2 to determine the moles of NaOH required for complete reaction:

Moles of NaOH = 2 * Moles of [tex]H_{2}[/tex]A

Moles of NaOH = 2 * 0.05 mol

Moles of NaOH = 0.1 mol

0.1 mol of sodium hydroxide (NaOH) would react exactly with 7.5 g of the diprotic acid [tex]H_{2}[/tex]A.

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Addition of a catalyst, at 15 °C, a certain reaction is able to produce 0.80 moles of product per minute at 25 °C it will produce at a rate of 0.40 moles per minute. The correct option to this question is C.

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Answer:

140.3 *C

Explanation:

(P1 * V1) / T1 = (P2 * V2) / T2

where P1 = 3.000 atm, V1 = 200.0 ml, T1 = 37.0°C + 273.15 = 310.15 K, P2 = 2.000 atm, V2 = 400.0 ml.

Substituting these values into the formula gives:

(3.000 atm * 200.0 ml) / 310.15 K = (2.000 atm * 400.0 ml) / T2

Solving for T2 gives:

T2 = (2.000 atm * 400.0 ml * 310.15 K) / (3.000 atm * 200.0 ml)

T2 ≈ 413 K or 140°C.