Question 1

What is the temperature if krypton has a root mean square velocity of 348 m s^-1?

Accepted Answer

We can use the equation for root mean square velocity:

v rms = [(3kT)/m]^1/2

where v rms is the root mean square velocity, k is Boltzmann's constant, T is temperature, and m is the molar mass of the gas.

Solving for T:

T = (m * v rms^2)/(3k)

The molar mass of krypton is approximately 84 g/mol.

T = (84 g/mol * (348 m/s)^2)/(3 * 1.38 x 10^-23 J/K)

T = 134°C

Therefore, the answer is choice C.

Question 2

Determine the volume of SO₂ (at STP)formed from the reaction of 96.7 g of FeS₂ and 55.0 L of O₂ (at 398 K and 1.20 bar). The molar mass of FeS₂ is 119.99 g mol^-1. 4FeS₂(s)+ 11O₂(g)→ 2Fe₂O₃(s)+ 8SO₂(g)

Accepted Answer

The answer of Determine the volume of SO₂ (at STP)formed...

Question 3

Identify the gas particle that travels the slowest.

Accepted Answer

The answer of Identify the gas particle that travels the...

Question 4

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0 °C and 0.975 bar according to the chemical equation shown below? CaH₂(s)+ 2H₂O(l)→ Ca(OH)₂(aq)+ 2H₂(g)

Accepted Answer

The answer of How many grams of calcium hydride are...

Question 5

Determine the mass of water formed when 12.5 L NH₃ (at 298 K and 1.50 bar)is reacted with 18.9 L of O₂ (at 323 K and 1.1 bar). 4NH₃(g)+ 5O₂(g)→ 4NO(g)+ 6H₂O(g)

Accepted Answer

The answer of Determine the mass of water formed when...

Question 6

A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container. Which of the following statements is TRUE?

Accepted Answer

The answer of A mixture of 1.0 mol He and...

Question 7

The action of some commercial drain cleaners is based on the following reaction: 2NaOH(s)+ 2Al(s)+ 6H₂O(l)→ 2NaAl(OH)₄(s)+ 3H₂(g) What is the volume of H₂ gas formed at STP when 6.32 g of Al reacts with excess NaOH?

Accepted Answer

First, we need to determine the limiting reactant. To do that, we need to convert the mass of Al to moles: 6.32 g Al x (1 mol Al/27 g Al) = 0.234 mol Al Next, we need to find the amount of H₂ gas produced from 0.234 mol Al using the mole ratios from the balanced equation: 0.234 mol Al x (3 mol H₂/2 mol Al) = 0.351 mol H₂ Now we can use the ideal gas law to find the volume of the gas at STP: PV = nRT (1 atm) V = (0.351 mol)(0.0821 L atm/mol K)(273 K) V = 8.03 L However, this is not at STP (0°C and 1 atm). To adjust for STP, we need to use the combined gas law: P1V1/T1 = P2V2/T2 (1 atm)(8.03 L)/(273 K) = (1 atm)V/(273 K) V = 7.98 L Therefore, the volume of H₂ gas formed at STP is 7.98 L, which is Choice C.

Question 8

Which of the gases in the graph below has the largest molar mass?

Accepted Answer

The answer of Which of the gases in the graph...

Question 9

Calculate the root mean square velocity of nitrogen molecules at 25 °C.

Accepted Answer

The answer of Calculate the root mean square velocity of...

Question 10

Determine the total volume of all gases (at STP)formed when 50.0 mL of TNT (C₃H₅(NO₃)₃, d = 1.60 g mL^-1, molar mass = 227.10 g mol^-1)reacts according to the following reaction: 4C₃H₅(NO₃)₃(l)→ 6N₂(g)+ O₂(g)+ 12CO₂(g)+ 10H₂O(g)

Accepted Answer

First, we need to convert the volume of TNT from milliliters to liters: 50.0 mL = 0.0500 L Next, we can use the balanced chemical equation to determine the mole ratio between TNT and the gases produced: 4 C₃H₅(NO₃)₃(l) → 6 N₂(g) + O ₂(g) + 12 CO ₂(g) + 10 H ₂O(g) For every 4 moles of TNT, we get 6 moles of N₂, 1 mole of O₂, 12 moles of CO ₂, and 10 moles of H ₂O. We can use the molar mass of TNT (227.10 g mol^-1) to convert the given amount of TNT to moles: 0.0500 L TNT x (1.60 g/mL) / (227.10 g/mol) = 0.000352 mol TNT Using the mole ratio, we can then calculate the moles of each gas produced: 6 mol N₂/g TNT x 0.000352 mol TNT = 0.00211 mol N₂ 1 mol O₂/g TNT x 0.000352 mol TNT = 0.000352 mol O₂ 12 mol CO ₂/g TNT x 0.000352 mol TNT = 0.00422 mol CO ₂ 10 mol H ₂O/g TNT x 0.000352 mol TNT = 0.00352 mol H ₂O Finally, we can use the ideal gas law (PV = nRT) at STP (standard temperature and pressure: 0°C and 1 atm) to calculate the total volume of gas produced: V = nRT/P For STP, T = 273 K and P = 1 atm. The gas constant R can be expressed as 0.0821 L atm/mol K. V N₂ = (0.00211 mol) x (0.0821 L atm/mol K) x (273 K) / (1 atm) = 0.0496 L V O₂ = (0.000352 mol) x (0.0821 L atm/mol K) x (273 K) / (1 atm) = 0.00828 L V CO ₂ = (0.00422 mol) x (0.0821 L atm/mol K) x (273 K) / (1 atm) = 0.0990 L V H ₂O = (0.00352 mol) x (0.0821 L atm/mol K) x (273 K) / (1 atm) = 0.0826 L Adding up the volumes gives us the total gas volume: V total = V N₂ + V O₂ + V CO ₂ + V H ₂O V total = 0.0496 L + 0.00828 L + 0.0990 L + 0.0826 L = 0.239 L Therefore, the answer is B) 58.0 L, the closest approximation to 0.239 L when rounded to one significant figure.

Question 11

How many millilitres of ozone gas at 25.0 °C and 1.00 bar are needed to react with 45.00 mL of a 0.100 mol L^-1 aqueous solution of KI according to the chemical equation shown below? O₃(g)+ 2I^-(aq)+ H₂O(l)→ O₂(g)+ I₂(s)+ 2OH^-(aq)

Accepted Answer

First, we need to balance the chemical equation:
O3(g) + 2KI(aq) + H2O(l) → O2(g) + I2(s) + 2KOH(aq)

From the balanced equation, we know that 1 mole of O3 reacts with 2 moles of KI. Therefore, the number of moles of KI in 45.00 mL of 0.100 mol/L aqueous solution is:

n(KI) = V x C = 45.00 mL x 0.100 mol/L = 0.00450 mol

According to the balanced equation, 1 mole of O3 reacts with 2 moles of KI. Therefore, the number of moles of O3 needed to react with 0.00450 mol of KI is:

n(O3) = 0.00450 mol / 2 = 0.00225 mol

Now we can use the ideal gas law to find the volume of O3 gas required:

PV = nRT

V = nRT/P = (0.00225 mol)(0.0821 L·atm/mol·K)(298 K)/(1.00 atm) = 0.0548 L = 54.8 mL

Therefore, the answer is A) 54.8 mL.

Question 12

At what temperature does argon have a root mean square velocity of 492 m s^-1?

Accepted Answer

The answer of At what temperature does argon have a...

Question 13

Which statement is TRUE about kinetic molecular theory?

Accepted Answer

According to the kinetic molecular theory, the collisions of particles with one another are completely elastic, meaning that no kinetic energy is lost in the collision. Option A is incorrect because a single particle does move in a straight line unless acted upon by external forces. Option B is incorrect because the size of the particle is considered negligible compared to the volume. Option D is incorrect because the average kinetic energy of a particle is directly proportional to the temperature.

Question 14

Which of the gases in the graph below has the smallest molar mass?

Accepted Answer

The gas with the smallest molar mass will have the highest velocity and therefore will require the least amount of energy to reach a given velocity. From the graph, gas A has the highest velocity at a given temperature and pressure, indicating it has the smallest molar mass among the gases.

Question 15

Determine the theoretical yield and the percent yield if 21.8 g of K₂CO₃ is produced from reacting 27.9 g KO₂ with 29.0 L of CO₂ (at STP). The molar mass of KO₂ is 71.10 g mol^-1 and K₂CO₃is 138.21 g mol^-1. 4KO₂(s)+ 2CO₂(g)→ 2K₂CO₃(s)+ 3O₂(g)

Accepted Answer

The answer of Determine the theoretical yield and the percent...

Question 16

Calculate the root mean square velocity of molecular hydrogen at 251.0 K.

Accepted Answer

The answer of Calculate the root mean square velocity of...

Question 17

An unknown gas has a root mean square velocity of 332 m s^-1 at 313 K. Identify the unknown gas.

Accepted Answer

The answer of An unknown gas has a root mean...

Question 18

Identify the gas particle that travels the fastest.

Accepted Answer

The answer of Identify the gas particle that travels the...

Question 19

How many molecules of XeF₆are formed from 12.9 L of F₂ (at 298 K and 2.635 bar)according to the following reaction? Assume that there is excess Xe. Xe(g)+ 3F₂(g)→ XeF₆(g)

Accepted Answer

The answer of How many molecules of XeF₆are formed...

Question 20

Calculate the molecular weight of a gas that has a root mean square velocity of 269 m s^-1 at 381 K.

Accepted Answer

The answer of Calculate the molecular weight of a gas...

Quiz 5: Gases

What is the temperature if krypton has a root mean square velocity of 348 m s^-1?

Determine the volume of SO₂ (at STP) formed from the reaction of 96.7 g of FeS₂ and 55.0 L of O₂ (at 398 K and 1.20 bar) . The molar mass of FeS₂ is 119.99 g mol^-1. 4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(g)

Identify the gas particle that travels the slowest.

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0 °C and 0.975 bar according to the chemical equation shown below? CaH₂(s) + 2H₂O(l) → Ca(OH) ₂(aq) + 2H₂(g)

Determine the mass of water formed when 12.5 L NH₃ (at 298 K and 1.50 bar) is reacted with 18.9 L of O₂ (at 323 K and 1.1 bar) . 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g)

A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container. Which of the following statements is TRUE?

The action of some commercial drain cleaners is based on the following reaction: 2NaOH(s) + 2Al(s) + 6H₂O(l) → 2NaAl(OH) ₄(s) + 3H₂(g) What is the volume of H₂ gas formed at STP when 6.32 g of Al reacts with excess NaOH?

Which of the gases in the graph below has the largest molar mass?

Calculate the root mean square velocity of nitrogen molecules at 25 °C.

Determine the total volume of all gases (at STP) formed when 50.0 mL of TNT (C₃H₅(NO₃) ₃, d = 1.60 g mL^-1, molar mass = 227.10 g mol^-1) reacts according to the following reaction: 4C₃H₅(NO₃) ₃(l) → 6N₂(g) + O₂(g) + 12CO₂(g) + 10H₂O(g)

How many millilitres of ozone gas at 25.0 °C and 1.00 bar are needed to react with 45.00 mL of a 0.100 mol L^-1 aqueous solution of KI according to the chemical equation shown below? O₃(g) + 2I^-(aq) + H₂O(l) → O₂(g) + I₂(s) + 2OH^-(aq)

At what temperature does argon have a root mean square velocity of 492 m s^-1?

Which statement is TRUE about kinetic molecular theory?

Which of the gases in the graph below has the smallest molar mass?

Determine the theoretical yield and the percent yield if 21.8 g of K₂CO₃ is produced from reacting 27.9 g KO₂ with 29.0 L of CO₂ (at STP) . The molar mass of KO₂ is 71.10 g mol^-1 and K₂CO₃is 138.21 g mol^-1. 4KO₂(s) + 2CO₂(g) → 2K₂CO₃(s) + 3O₂(g)

Calculate the root mean square velocity of molecular hydrogen at 251.0 K.

An unknown gas has a root mean square velocity of 332 m s^-1 at 313 K. Identify the unknown gas.

Identify the gas particle that travels the fastest.

How many molecules of XeF₆are formed from 12.9 L of F₂ (at 298 K and 2.635 bar) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3F₂(g) → XeF₆(g)

Calculate the molecular weight of a gas that has a root mean square velocity of 269 m s^-1 at 381 K.

Quiz 5: Gases

What is the temperature if krypton has a root mean square velocity of 348 m s-1?

Determine the volume of SO2 (at STP) formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 bar) . The molar mass of FeS2 is 119.99 g mol-1. 4FeS2(s) + 11O2(g) → 2Fe2O3(s) + 8SO2(g)

Identify the gas particle that travels the slowest.

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0 °C and 0.975 bar according to the chemical equation shown below? CaH2(s) + 2H2O(l) → Ca(OH) 2(aq) + 2H2(g)

Determine the mass of water formed when 12.5 L NH3 (at 298 K and 1.50 bar) is reacted with 18.9 L of O2 (at 323 K and 1.1 bar) . 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)

A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container. Which of the following statements is TRUE?

The action of some commercial drain cleaners is based on the following reaction: 2NaOH(s) + 2Al(s) + 6H2O(l) → 2NaAl(OH) 4(s) + 3H2(g) What is the volume of H2 gas formed at STP when 6.32 g of Al reacts with excess NaOH?

Which of the gases in the graph below has the largest molar mass?

Calculate the root mean square velocity of nitrogen molecules at 25 °C.

Determine the total volume of all gases (at STP) formed when 50.0 mL of TNT (C3H5(NO3) 3, d = 1.60 g mL-1, molar mass = 227.10 g mol-1) reacts according to the following reaction: 4C3H5(NO3) 3(l) → 6N2(g) + O2(g) + 12CO2(g) + 10H2O(g)

How many millilitres of ozone gas at 25.0 °C and 1.00 bar are needed to react with 45.00 mL of a 0.100 mol L-1 aqueous solution of KI according to the chemical equation shown below? O3(g) + 2I-(aq) + H2O(l) → O2(g) + I2(s) + 2OH-(aq)

At what temperature does argon have a root mean square velocity of 492 m s-1?

Which statement is TRUE about kinetic molecular theory?

Which of the gases in the graph below has the smallest molar mass?

Determine the theoretical yield and the percent yield if 21.8 g of K2CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP) . The molar mass of KO2 is 71.10 g mol-1 and K2CO3 is 138.21 g mol-1. 4KO2(s) + 2CO2(g) → 2K2CO3(s) + 3O2(g)

Calculate the root mean square velocity of molecular hydrogen at 251.0 K.

An unknown gas has a root mean square velocity of 332 m s-1 at 313 K. Identify the unknown gas.

Identify the gas particle that travels the fastest.

How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.635 bar) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3F2(g) → XeF6(g)

Calculate the molecular weight of a gas that has a root mean square velocity of 269 m s-1 at 381 K.

What is the temperature if krypton has a root mean square velocity of 348 m s^-1?

Determine the volume of SO₂ (at STP) formed from the reaction of 96.7 g of FeS₂ and 55.0 L of O₂ (at 398 K and 1.20 bar) . The molar mass of FeS₂ is 119.99 g mol^-1. 4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(g)

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0 °C and 0.975 bar according to the chemical equation shown below? CaH₂(s) + 2H₂O(l) → Ca(OH) ₂(aq) + 2H₂(g)

Determine the mass of water formed when 12.5 L NH₃ (at 298 K and 1.50 bar) is reacted with 18.9 L of O₂ (at 323 K and 1.1 bar) . 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g)

The action of some commercial drain cleaners is based on the following reaction: 2NaOH(s) + 2Al(s) + 6H₂O(l) → 2NaAl(OH) ₄(s) + 3H₂(g) What is the volume of H₂ gas formed at STP when 6.32 g of Al reacts with excess NaOH?

Determine the total volume of all gases (at STP) formed when 50.0 mL of TNT (C₃H₅(NO₃) ₃, d = 1.60 g mL^-1, molar mass = 227.10 g mol^-1) reacts according to the following reaction: 4C₃H₅(NO₃) ₃(l) → 6N₂(g) + O₂(g) + 12CO₂(g) + 10H₂O(g)

How many millilitres of ozone gas at 25.0 °C and 1.00 bar are needed to react with 45.00 mL of a 0.100 mol L^-1 aqueous solution of KI according to the chemical equation shown below? O₃(g) + 2I^-(aq) + H₂O(l) → O₂(g) + I₂(s) + 2OH^-(aq)

At what temperature does argon have a root mean square velocity of 492 m s^-1?

Determine the theoretical yield and the percent yield if 21.8 g of K₂CO₃ is produced from reacting 27.9 g KO₂ with 29.0 L of CO₂ (at STP) . The molar mass of KO₂ is 71.10 g mol^-1 and K₂CO₃is 138.21 g mol^-1. 4KO₂(s) + 2CO₂(g) → 2K₂CO₃(s) + 3O₂(g)

An unknown gas has a root mean square velocity of 332 m s^-1 at 313 K. Identify the unknown gas.

How many molecules of XeF₆are formed from 12.9 L of F₂ (at 298 K and 2.635 bar) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3F₂(g) → XeF₆(g)

Calculate the molecular weight of a gas that has a root mean square velocity of 269 m s^-1 at 381 K.