Answer
Molarity (C) = 0.455 mol/L
Explanation
Given:
Mass of H2SO4 = 78 g
Molar mass of H2SO4 = 98.0 g/mol
Volume of the solution = 1.75 L
Required: The molarity of the solution
Solution
Step 1: Calculate the number of moles of moles of H2SO4
n = m/M where n is the moles, m is the mass and M is the molar mass
n = 78 g/98.0 g/mol
n = 0.796 mol
Step 2: Calculate the molarity of the solution
C = n/V where C is the molarity/concentration, and V is the volume of the solution
C = 0.796 mol/1.75 L
C = 0.455 mol/L
3.0 grams of dry ice (solid CO 2 ) is converted to a gas at STP. How many liters of gas is present?
answer and explanation
3.0 grams is converted to gas.
we first find the number of mols
n = m/M
n - mols
m - mass
M - molar mass
n = 3.0/ 28.01
= 0.12 mols
we know that at STP every gas has a volume of 22.4 L
therefor 0.12 mols will have a volume of:
0.12 x 22.4 = 2.69 L
How many electrons would be too many for a nitrogen atom
Determine from the balanced chemical reaction ifthe derived mole ratio is correct or incorrect.4Zn + 10HNO3 + 4Zn(NO3)2 + N20 + 5H204 moles Zn10 moles HNO3correctincorrect
Answer
Correct
Explanation
[tex]4Zn+10HNO_3\rightarrow4Zn(NO_3)_2+N_2O+5H_2O[/tex]From the balanced chemical reaction, 4 moles of Zn reacted with 10 moles of HNO3 to produced 4 moles, 1 mole, and 5 moles of Zn(NO3)2, N2O, and H2O respectively.
Therefore, comparing the mole of Zn to HNO3, then the derived ratio is correct.
How many moles of methane(CH4)are in 7.31x1025 molecules?Let's begin by setting up our equation.What belongs in the green box?7.31x1025 molecules CHA?A. 1 mole CH4B. 6.02 x 1023 molecules CHAEnter
Answer
B. 6.02 x 10²³ molecules CH₄
Explanation
Avogardro's constant says 1 mole of a substance has 6.02 x 10²³ molecules.
⇒ 1 mole = 6.02 x 10²³ molecules/atoms
Therefore, the mole of methane in the given molecules can be calculatedas follows
[tex]Mole\text{ of methane }=\frac{7.31\times10^{25}_{}}{6.02\times10^{23}\text{ }molecules\text{ }CH_4}=121.43\text{ mole}[/tex]Hence, what belongs to the green box is 6.02 x 10²³ molecules CH₄
Conservation of Mass Activity WorksheetInstructions: Observe and analyze the interactions between the substances pictured in the slide show. Compare the properties of substances before and after each interaction. You will submit your completed worksheet for grading.Data TableOn the table below, record your observations before and after the interactions and explain how mass was conserved. Describe the changes in properties that prove a chemical reaction occurred. The first row is an example. Observations Before InteractionObservations After InteractionHow was mass conserved?Proof of a Chemical ReactionExample: Sugar + HeatThe sugar is in tiny white particles in a pile. Heat is not seen but is implied by the heat source. The pile of sugar in the pot has a mass of 100 grams.There is a solid, light brown mass at the bottom of the pot. It has a mass of 100 grams.The mass of the sugar is the same in melted form as it is in solid crystal form.There was not a chemical reaction. Sugar did not change composition. It only melted. Melting point is a physical property, and this is a physical change.Steel Wool + Oxygen (Fire) Egg + Heat Water + Heat Zinc + Hydrogen Chloride Sodium Hydroxide + Copper Sulfate
Steel wool and Oxygen (Fire)
Steel wool is mostly iron (Fe) and oxygen cannot be seen but it is used during heating or burning of substances. When iron is burned, it reacts with oxygen in the air to form iron oxide (FeO2). This reaction releases heat. When the steel wool is heated, a new substance is created. The mass of steel wool (product) is increased. This is a chemical change/reaction because the steel wool changes to iron oxide, and mass is not conserved.
Egg and heat
An egg is a liquid substance which consists of colorless substance and yellow yolk. Heat is not seen but produced by the heat source. When the egg is heated, it becomes a solid. The mass of the egg is not changed, it remains the same, the only difference is that it changes from being a liquid to solid. Only a physical change occurred.
Water and heat
Water (I will assume it is in its liquid state) is liquid and heat is the source of energy, it cannot be seen but is implied by the heat source which can be a stove in this case. When liquid water is heated, its state is changed to vapor or gas. The mass of the water remains the same, thus mass is conserved because this is a physical reaction or change.
Zinc and hydrogen Chloride
Zinc is a brittle metal at room temperature and has a silver-greyish appearance. Hydrogen Chloride is a colourless gas at room temperature. When zinc reacts with hydrochloric acid (hydrogen chloride), the metal displaces the hydrogen to form zinc chloride. This is a chemical reaction since zinc increases in mass, thus mass is not conserved.
Sodium hydroxide and Copper sulfate
Sodium hydroxide is a white solid and copper sulfate is a blue solid. When sodium hydroxide reacts with copper sulfate a blue precipitate of copper hydroxide is formed. This is a chemical reaction, thus the mass of one of the reactants will be larger in products. However, mass is conserved if all products are observed/calculated.
Drag each conversion factor to the arrow that indicates where it should be used
Explanation:
mass ----> moles ---> representative particles:
To go from mass to moles we usually use the molar mass of the substance or compound that we are working with. Molar mass is expressed in g/mol, so we divide by the molar mass.
mass --> moles: g * 1 mol/(number of g) = mol
To go from moles to representative particles we use Avogadro's number. There are 6.02 *10^23 particles in 1 mol of particles.
moles ---> particles: moles * 6.02 * 10^23 particles /(1 mol) = particles
Then to go from particles to moles we do something similar.
particles---->moles: particles * 1 mol/(6.02 * 10^23 particles) = moles
And to go from moles to grams, instead of dividing by the molar mass we multiply by it.
moles --> mass: moles * number of g/(1 mol) = g
Answer:
mass ----> 1 mol/(number of g) ---> moles ---> 6.02 * 10^23 particles /(1 mol) ----->particles
mass <---number of g/(1 mol) <----- moles <----1 mol/(6.02 * 10^23 particles)<----- particles
What is the value of the rate constant for this reaction?
Let's start by stating the important given data:
time ln[A]
0
20
To answer this question, we have to use the following formula corresponding to the first-order reaction rate constant:
[tex]\ln[A]=-kt+\ln[A]_0[/tex]Using
state the preparation and properties of carboxylic acids.
thankyou!
An organic compound with a carboxyl functional group is known as a carboxylic acid. They can be found in abundance in nature and are also synthesized by humans. Carboxylic acids deprotonate to produce a carboxylate anion with the general formula R-COO-, which can be used to make several useful salts including soap.
preparation ---
using Alcohol -(see image)
With the addition of oxidizing agents, primary alcohol is oxidized to produce carboxylic acid. As a result, the oxidation of primary alcohols yields aldehydes, which are then oxidized again to yield carboxylic acids.
using Grignard reagents-(see image)
The Grignard reagents reaction allows for the formation of carboxylic acid. Grignard reagents form carboxylic acid salts when they react with crushed dry ice or solid carbon dioxide.
properties ---
1)Carboxylic acid molecules are polar due to the presence of two electronegative oxygen atoms
2)They also participate in hydrogen bonding due to the interaction of the carbonyl group (C=O) and the hydroxyl group.
To know more about organic chemistry click below
https://brainly.com/question/26088065
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Consider the reaction between calicium oxide and carbon dioxide. CaO(s) + CO2 arrow CaCO3(s)A chemist allows 14.4 g of CaO and 13.8 g of CO2 to react. When the reaction is finished the chemist collects 19.4 g of CACO3. Determine the limiting reactant, theoretical yield and the percent yield for the reaction.
They give us the equation of the reaction already balanced:
CaO(s) + CO2 ----> CaCO3(s)
So we can proceed to do the calculations.
We will initially determine which is the limiting reactant and we will make the theoretical yield calculations based on this reactant. Finally we will find the percent yield by dividing the amount obtained by the chemist by the theoretical amount.
We will follow the following steps:
1. We calculate the moles of the reactants by dividing the given weight by the molar mass.
Molar mass CaO= 56.0774g/mol
Molar mass CO2= 44.01g/mol
2. We calculate the limiting reactant by determining which reactant has fewer moles. This is because the CaO to CO2 ratio is 1 to 1, meaning that the same moles of each reactant are needed to react.
3. We find the moles of CaCO3 by the stoichiometry of the reaction.
4. We find the grams of CaCO3 by multiplying the moles found by the molar mass, this will be the theoretical yield. Molar mass CaCO3=100.0869g/mol
5. We calculate the percent yield by dividing the amount found above by the current yield=19.4g CaCO3.
Let's proceed with the calculations.
1. Moles of reactants
Mol of CaO
[tex]molCaO=14.4gCaO\times\frac{1molCaO}{56.0774gCaO}=0.257molCaO[/tex]Mol of CO2
[tex]molCO_2=13.8gCO_2\times\frac{1molCO_2}{44.01gCO_2}=0.314molCO_2[/tex]2. Limiting reactant
We have fewer moles of CaO, since the ratio is 1 to 1 this will be the limiting reactant, so the following calculations we will do with 0.257mol of CaO
Limiting reactant: CaO
3. Moles of CaCO3
The ratio CaCO3 to CaO is 1/1 so we have the same number of moles of CaO.
Moles of CaCO3 = 0.257mol
4. Grams of CaCO3 (Theoretical yield)
[tex]gCaCO_3=0.257molCaCO_3\times\frac{100.0869gCaCO_3}{1molCaCO_3}=25.7gCaCO_3[/tex]The theoretical yield of CaCO3 is 25.7g
5. Percent yield
[tex]\begin{gathered} PercentYield=\frac{ActualYield}{TheoreticalYield}\times100\% \\ PercentYield=\frac{19.4gCaCO_3}{25.7gCaCO_3}\times100\% \\ PercentYield=75.5\% \end{gathered}[/tex]The percent yield of CaCO3 is 75.5%
When ammonia burns in pure oxygen, the reaction is: 4 NH3(g) + 3 O2(g) 2 N2(g) + 6 H2O(g)What mass of water could be produced from 45.0 g of ammonia and excess Oxygen?
This is a stoichiometry problem, where we have an initial amount of reactant and we need to find out how much of the product will we end up with, in order to do that we need to:
1. Set up the properly balanced equation, which the question already provided us
4 NH3 + 3 O2 -> 2 N2 + 6 H2O
2. See how many moles of reactant there are in the given amount of grams, we will do that by using its molar mass
NH3 molar mass = 17g/mol, and we have 45 grams of it
17g = 1 mol
45g = x moles
x = 2.65 moles of NH3
3. Check the molar ratio between the two compounds, this we can see from the balanced equation, the molar ratio between NH3 and H2O is 4:6, this means that for every 4 moles of NH3 in the reaction, we will have 6 moles of water as product, but we have 2.65 moles of NH3
4 NH3 = 6 H2O
2.65 NH3 = x H2O
x = 3.97 moles of H2O, or we can go ahead and round up to 4 moles of H2O
4. Calculate how many grams will be equal to the number of moles that we found out, using the molar mass of H2O
H2O molar mass = 18g/mol
18 g = 1 mol
x grams = 4 moles of H2O
x = 72 grams of H2O
Look at the equation.6CO2 + 6H2O → C6H12O6 + 6O2 What process does the chemical equation represent?PhotosynthesisRespirationOsmosisDigestion
H₂O and CO₂ are the substances needed to carry out photosynthesis. Chlorophyll molecules absorb sunlight and break down molecules of H₂O, releasing O₂ and hydrogen. Then, hydrogen binds to CO₂ and forms glucose (C₆H₁₂O₆).
6 CO₂ + 6 H₂O → C₆H₁₂O₆ + 6 O₂
So this chemical reaction equation represents Photosynthesis.
What is the wavelength of 101-WCHEM its broadcasting frequency is 101.9 megahertz?
What is the wavelength of 101-WCHEM its broadcasting frequency is 101.9 megahertz?
The relationship between the frequency of an electromagnetic wave and its wavelength is given by this formula:
c = λ * f
where, c stands for the speed of light, λ is the wavelength and f is the frequency.
According to our problem:
f = 101.9 megahertz
λ = ??
And we can search for the value of the speed of light:
c = 2.99 * 10⁸ m/s
To solve the problem we have to convert MHz into cycles/sec
1 MHz = 1 000 000 Hz = 1 * 10⁶ Hz
1 Hz = 1 cycle/sec
f = 101.9 MHz * (1 * 10⁶ Hz) / (1 MHz) = 1.019 * 10⁸ Hz = 1.019 * 10⁸ cycles/sec
Our unknown is the wavelength. Let's solve our formula for λ:
λ = c / f
Replacing:
λ = (2.99 * 10⁸ m/s) / ( 1.019 * 10⁸ cycles/s)
λ = 2.93 m
The wavelength of 101-WCHEM is 2.93 m.
If we want to convert it to cm:
100 cm = 1 m
λ = 2.93 m * 100 cm/(1 m) = 293 cm
The wavelength of 101-WCHEM is 293 cm.
Nitrogen gas is cooled from 300k to 50k. If it’s original volume was 40L,what is the final volume?
In this question, we have a gas going through a change in temperature and the law that shows the relationship between temperature and volume is Charles's gas Law, which can be presented with the following formula:
V1/T1 = V2/T2
We have:
V1 = 40 L
T1 = 300 K
V2 = ?
T2 = 50 K
Now we just need to add these values into the formula:
40/300 = V2/50
0.1333 = V2/50
V2 = 6.7 Liters will be the new volume
___Na+__H2O➡️__NaOH+__H2In a experiment, 2.35g of Na react with 7.25 g of H2O1) write the formula for the reactant that is the limiting reactant
Answer:
Explanations:
Given the unbalanced chemical reaction expressed as:
[tex]aNa+bH_2O\rightarrow cNaOH+dH_2[/tex]The balanced chemical reaction will be expressed as:
[tex]2Na+2H_2O\rightarrow2NaOH+H_2[/tex]Given the following
Mass of Na = 2.35g
Mass of H2O = 7.25g
Determine the moles of the elements
Moles of Na = Mass/Molar mass
Moles of Na = 2.35/.35
How many moles of h2o are there in 180g of water (molar mass is 18.001g/mole)
First, remember that:
1 mol of any compound is the same thing as the molecular mass of the compound.
So, we could say that 1 mol of H2O is equal to the molecular mass of H2O, which is 18.001g/mole.
Given that we have 180g of water, we could write:
[tex]180gH_2O\cdot\frac{1molH_2O}{18.001gH_2O}=10molesH_2O[/tex]Therefore, there are 10 moles of water in 180g of water.
To convert grams to moles, we just divide the amount in grams we have by the molecular mass.
[tex]\text{moles}=\frac{\text{mass given}}{molecular\text{ mass}}[/tex]how do i write out the equation please include states and the balancing with the work
Answer
[tex]C_8H_7O_2COOH(aq)+NaOH(aq)\rightarrow NaC_8H_7O_2COO(aq)+H_2O(l)[/tex]Explanation
ASA from the question implies Acetysalicylic Acid (C₈H₇O₂COOH)
Therefore, a balanced neutralization equation for the neutralization of ASA and NaOH is:
[tex]C_8H_7O_2COOH(aq)+NaOH(aq)\rightarrow NaC_8H_7O_2COO(aq)+H_2O(l)[/tex]Calculate the number of C, H, O adams in 9.74 grams of glucose. Be sure your answer has the correct number of significant figures.
Given that :
• Mass of C6H12O6 = 9.74g
,• Molecular mass C6H12O6 =180.156g/mol
,• Moles of C6H12O6 = mass/M.Mass
=9.74g/180.156g/mol
=0.054moles.
2. Calculate mole ratio of C, H, O , since we have 0.054moles of C6H12O6(2.1) Carbon → 1 mole C6H12O6 : 6mol C
so, 0.054moles : x mol C
Therefore x mol C = 0.054 * 6 = 0.324moles of Carbon
• Number of atoms for C
No of C atoms = mole* Avogadro number
=0.324 * 6.022*10^23
=1.95x10^23 atoms
(2.2) Hydrogen → 1 mole of C6H12O6 : 12 mol of H
So; 0.054moles : x mol H
Therefore xmol H = 0.054*12 = 0.648 moles of Hydrogen
• Number of atoms for H
No of H atoms = 0.648 * 6.022*10^23
=3.90x10^23 atoms .
(2.3) Oxygen → 1 mole of C6H12O6 : 6 mol of O
So, 0.054 moles : xmol O
Therefore x mol O = 0.054 * 6 =0.324 moles
• Number of atoms for Oxygen =0.324 * 6.022*10^23
=1.95x10^23 atoms
Finally, number of C atoms =1.95x10^23 atoms. number of H atoms =3.90x10^23 atoms . number of O atoms =1.95x10^23 atoms
Balance the following redox reaction in base solution:SO32- (aq) + MnO4 (aq) → SO42- (aq) + MnO₂ (s)(ВH₂O + 3SO32 + 2MnO4 →3SO42- + 2MnO₂ + 2OH™H₂O + 3SO32- + 2 MnO4 →3SO42- + 2MnO₂35032 +2MnO4-3SO2 + 2 MnO₂ + 2OH™3502 +2MnO4-3SO2 + 2MnO₂
Answer:
Explanation:
Here, we want to balance the given redox reaction in a basic medium
We start by breaking the reaction into half-reactions:
[tex]\begin{gathered} SO_3^{2-}\text{ }\rightarrow\text{ SO}_4^{2-} \\ MnO_4^-\text{ }\rightarrow\text{ MnO}_2 \end{gathered}[/tex]The next step here is to balance the other elements aside from oxygen and hydrogen. We can see, however, that the other elements are balanced. Then we proceed to the next step
We balance the oxygen atoms by adding water molecules:
[tex]\begin{gathered} SO_3^{2-}\text{ + H}_2O\text{ }\rightarrow\text{ SO}_4^{2-} \\ MnO_4^-\text{ }\rightarrow\text{ MnO}_2\text{ + 2H}_2O \end{gathered}[/tex]Now, the next step is to balance the hydrogen by adding hydrogen ions
We have that as:
[tex]\begin{gathered} SO_{\text{ }3}^{2-}\text{ + H}_2O\text{ }\rightarrow\text{ SO}_4^{2-}\text{ + 2H}^+ \\ MnO_4^-\text{ + 4H}^+\rightarrow\text{ MnO}_2\text{ + 2H}_2O \end{gathered}[/tex]Now, we balance the charges by adding electrons:
[tex]\begin{gathered} SO_3^{2-}\text{ + H}_2O\text{ }\rightarrow\text{ SO}_4^{2-}\text{ + 2H}^+\text{ + 2e}^- \\ MnO_4^-\text{ + 4H}^+\text{ + 3e}^-\rightarrow\text{ MnO}_2\text{ + 2H}_2O \end{gathered}[/tex]Now, we seek to strike out the electrons. We multiply equations 1 by 3 and 2 by 2:
[tex]\begin{gathered} 3SO_3^{2-}\text{ + 3H}_2O\text{ }\rightarrow\text{ 3SO}_4^{2-}\text{ + 6H}^+\text{ + 6e}^- \\ 2MnO_4^-\text{ + 8H}^+\text{ + 6e}^-\text{ }\rightarrow\text{ 2MnO}_2\text{ + 4H}_2O \end{gathered}[/tex]Balancing this, we have:
[tex][/tex]A sample containing 4.20 g of O2 gas has an initial volume of 20.5 L . What is the final volume, in liters, when each of the following occurs and pressure and temperature do not change?A sample of 2.25 g of O2 is removed.
Answer
V2 = 10.95 L
Explanation
Given:
mass 1 = 4.20 g
mass 2 = 2.25 g
volume 1 = 20.5 L
Required: volume 2
Solution
Step 1: Find the number of moles of mass 1 and 2.
For mass 1:
n = m/M where n is the moles, m is the mass and M is the molar mass
n = 4.20g/31.998g/mol
n = 0.131 mol
For mass 2:
n = 2.25g/31.998g/mol
n = 0.070 mol
Step 2: For this problem, we will use the ideal gas law equation
PV = nRT
However, P, V and R are constant
Therefore
[tex]\frac{n_1}{V_1}\text{ = }\frac{n_2}{V_2}[/tex]V2 = (V1n2)/n1
V2 = (20.5L x 0.070 mol)/0.131 mol
V2 = 10.95 L
How are scientific laws different from scientific theories?OA. Scientific theories are based on mathematical equations, whilescientific laws are based on observations.OB. Scientific theories are used to explain phenomena, while scientificlaws describe the natural world.C. Scientific theories are used to guide investigations, while scientificlaws govern the procedures used by scientists.D. Scientific theories are reviewed by other scientists, while scientificlaws are not.
In the scientific world, we have different names to describe each step of the scientific method, two definitions which are very close to one another are Scientific Law and Scientific Theory.
Usually Scientific laws are described using mathematical equations and formulas to describe what will happen in a given situation, for example the Gravity Law
Scientific theory will describe how a phenomenon happens, and it is usually done through observations and testing, like the Evolution theory
Therefore the best answer will be letter B
Calculate the heat released when 1200 g of steam changes phase to liquid water. Assume no temperature change and Hv = 2260J/g
According to the explanation given in the previous session, now we have a similar situation, but now we have steam changing to liquid water and a release of heat and not absorption. The formula will be the same:
Q = m * ΔHv
We have:
m = 1200 grams
ΔHv = 2260 J/g, but since we are releasing energy, this value has to be negative, -2260 J/g
Now we add these values into the formula:
Q = 1200 * -2260
Q = - 2712000 Joules or 2712 Kilojoules
How many moles of OO are in 1.9 molmol of Ca(NO3)2Ca(NO3)2?
1) First, let's find out how many moles of O are in 1 mol of Ca(NO₃)₂
It has:
1 mol of Ca
If the compound is enclosed in parentheses, you must multiply the value outside the parentheses by each atom of each element that is within the parentheses. In this case the value is 2, so it is necessary to multiply 2x1 (because inside the parentheses there is an atom of N) and multiply 2x3 to find the amount of oxygen (because inside the parentheses there are 3 atoms of O)
2 mol of N
6 mol of O
2) Now let's use the rule of 3 to find out how many moles of O are in 1.9 mol of Ca(NO₃)₂
1.9 mol of Ca(NO₃)₂ ------ x mol of O
1 mol of Ca(NO₃)₂ -------- 6 mol of O
x = 1.9 × 6
x = 11.4 moles of O
Answer: 11.4 mol O
Question 7 of 10What is latent heat?A. The heat required to increase the temperature of an object 1°CB. The heat absorbed or released during a phase changeC. The heat absorbed or released when bonds that hold a moleculetogether break or formD. The heat required for a chemical reaction to occurSUBMIT
A. The heat required to increase the temperature of an object 1°C
The latent heat is the energy absorbed or released by a body when its temperature changes
the energy absorbed or released during a phase change is the freezing enthalpy or vapor enthalpy depending on the phases
The energy involved when bonds are broken or formed is the formation enthalpy
the energy involved in a chemical reaction is the reaction enthalpy.
2 NaOH + H2SO4 - 2 H2O + Na2SO4How many moles of sodium hydroxide are needed to form 63 grams of sodium sulfate?
1) Write the chemical equation.
[tex]2NaOH+H_2SO_4\rightarrow2H_2O+Na_2SO_4[/tex]2) Convert the mass of Na2SO4 to moles of Na2SO4.
The molar mass of Na2SO4 is 142.0421 g/mol.
[tex]mol\text{ }Na_2SO_4=63\text{ }g\text{ }Na_2SO_4*\frac{1\text{ }mol\text{ }Na_2SO_4}{142.0421\text{ }g\text{ }Na_2SO_4}=0.4435\text{ }mol\text{ }Na_2SO_4[/tex]3) Moles of NaOH needed
The molar ratio between NaOH and Na2SO4 is 2 mol NaOH: 1 mol Na2SO4.
[tex]mol\text{ }NaOH=0.4435\text{ }mol\text{ }Na_2SO_4*\frac{2\text{ }mol\text{ }NaOH}{1\text{ }mol\text{ }Na_2SO_4}=0.8871\text{ }mol\text{ }NaOH[/tex]0.8871 mol NaOH is required to form 63 g Na2SO4.
Which of the following statements best describes photochemical smog in large cities in the United States?Photochemical smog is more prevalent during winter months.Answer A: Photochemical smog is more prevalent during winter months.APhotochemical smog causes negative human health impacts such as eye and lung irritation.Answer B: Photochemical smog causes negative human health impacts such as eye and lung irritation.BPhotochemical smog contains secondary pollutants that form when sulfur dioxide and nitrogen oxide interact in the atmosphere.Answer C: Photochemical smog contains secondary pollutants that form when sulfur dioxide and nitrogen oxide interact in the atmosphere.CPhotochemical smog is composed of primary and secondary pollutants that are not reactive.
Answer
C: Photochemical smog contains secondary pollutants that form when sulfur dioxide and nitrogen oxide interact in the atmosphere.
Explanation
Photochemical smog is a mixture of pollutants that are formed when nitrogen oxides and volatile organic compounds react to sunlight, creating a brown haze above cities in the United States. It tends to occur more often in summer because that is when we have the most sunlight. Their low concentration causes irritation in the nose and throat and their high concentration causes headache, chest pain, cough, and difficulty in breathing.
There is a tire that has a volume of 35 L, 38 atm, and a temperature of240 K. How many moles of air is in the tire?
In this question, we have to calculate how many moles of air is in a tire with this following setup of data:
35 L
38 atm
240 K
In order to find the number of moles, we will be using the Ideal gas law formula, which is:
PV = nRT
Where:
P = pressure, 38 atm
V = volume, 35 L
n = number of moles
R = gas constant value, 0.082
T = temperature, 240 K
Now we add these values into the formula:
38 * 35 = n * 0.082 * 240
1330 = 19.68n
n = 1330/19.68
n = 67.6 moles of air are in this tire
Calculate the [H3O+] value of each aqueous solution.NaOH with [OH−]=1.0×10−2M Express your answer using two significant figures.
Answer
[H₃O⁺] = 1.0 x 10⁻¹² M
Explanation
Given that:
[OH⁻] = 1.0 x 10⁻² M
What to find:
To calculate the [H₃O⁺] of the NaOH solution.
Step-by-step solution:
The [H₃O⁺] of the NaOH solution can be calculated using the relation given below:
[H₃O⁺] x [OH⁻] = 1.0 x 10⁻¹⁴
Therefore, the [H₃O⁺] will be:
[tex].\left[H₃O⁺\right]=\frac{1.0\times10^{-14}}{[OH^-]}=\frac{1.0\times10^{-14}}{1.0\times10^{-2}}=1.0\times10^{-12}\text{ }M[/tex]Hence, the [H₃O⁺] value of the NaOH aqueous solution is 1.0 x 10⁻¹² M
A polar covalent bond is a bond betweenQuestion options:two atoms that share electrons unequally.two atoms that share electrons equally.two oppositely charged ions.two polar molecules.
In this question, we have to determine which option will fit best the polar covalent bond definition.
Covalent bonds are by definition a type of bonding in which we will have the share of electrons instead of donating, like ionic bonds. Polar covalent bonds still follow this definition but we will have an unequal sharing, one atom will end up pulling more of the electrons towards its own side, because this atom is more electronegative.
Therefore the best answer will be the 1st answer
Calculate the dH value for the following chemical reaction:C + 2H2O CO2 + 2H2First equation: C + O2 CO2 dH = -394 kJSecond Equation: 2H2 + O2 2H2O dH = -484 kJ
dH = +90kJ
Explanations:
Given the following chemical reactions with their individual enthalpy change expressed as:
[tex]\begin{gathered} C+O_2\rightarrow CO_2\text{ }\triangle H=-394kJ \\ 2H_2+O_2\rightarrow2H_2O\text{ }\triangle H=-484kJ \end{gathered}[/tex]We need the enthalpy change value for the reaction shown:
[tex]2H_2O\rightarrow CO_2+2H_2[/tex]To get the equivalent reaction from the 2chemical reactions above, we will interchange the product and reactant of the formation of water to have:
[tex]\begin{gathered} C+\cancel{O_2}\operatorname{\rightarrow}CO_2\operatorname{\triangle}H=-394kJ \\ 2H_2O\rightarrow2H_2+\cancel{O_2}\triangle H=+484kJ \\ _{--------------------------------------} \\ C+2H_2O\rightarrow CO_2+2H_2\text{ }\triangle H=-396kJ+484kJ=+90kJ \end{gathered}[/tex]Hence the dH value for the following chemical reaction C + 2H2O -> CO2 + 2H2 is +90kJ
How much water must be added to 500.0 mL of a 3.00 M HCl solution to obtain a solution that is 2.00 M
Water must be added to 500.0 mL of a 3.00 M HCl solution to obtain a solution that is 2.00 M is 750ml
A solution is a homogeneous mixture of one or more solutes dissolved in a solvent
Here given data is
M₁V₁ = M₂V₂
M₁ = 2.00 M
V₁ = ?
M₂ = 3.00 M
V₂ =500.0 mL
Si putting this value in equation
M₁V₁ = M₂V₂
2.00 M×V₁ = 3.00 M×500.0 mL
V₁ = 750ml
750ml water must be added to 500.0 mL of a 3.00 M HCl solution to obtain a solution that is 2.00 M
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