Question 1

A mixture of 10.0 g of Ne and 10.0 g Ar has a total pressure of 1.6 atm.What is the partial pressure of Ne?

Accepted Answer

The partial pressure of a gas in a mixture is equal to the mole fraction of that gas multiplied by the total pressure. The mole fraction of Ne is 10.0 g / (10.0 g + 10.0 g) = 0.5. Therefore, the partial pressure of Ne is 0.5 * 1.6 atm = 0.8 atm.

Question 2

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

Accepted Answer

The root mean square velocity ($v_{rms}$) of a gas can be calculated using the formula $v_{rms} = \sqrt{\frac{3kT}{m}}$, where $k$ is the Boltzmann constant ($1.38 \times 10^{-23} J/K$), $T$ is the temperature in Kelvin, and $m$ is the mass of a single molecule in kilograms. For nitrogen ($N_2$), the molar mass is 28.02 g/mol, which is $28.02 \times 10^{-3} kg/mol$. Since there are $6.022 \times 10^{23}$ molecules in a mole (Avogadro's number), the mass of a single nitrogen molecule is $\frac{28.02 \times 10^{-3}}{6.022 \times 10^{23}} kg$. The temperature in Kelvin is $25°C + 273.15 = 298.15 K$. Substituting these values into the formula gives a $v_{rms}$ close to 515 m/s.

Question 3

Rank the following in order of decreasing rate of effusion. F₂ SF₆ CO Kr

Accepted Answer

The answer of Rank the following in order of decreasing...

Question 4

Calculate the ratio of effusion rates of Cl₂ to F₂.

Accepted Answer

The ratio of effusion rates is given by Graham's law: rate1/rate2 = sqrt(M2/M1). For Cl2 and F2, M1 = 70.9 g/mol (Cl2) and M2 = 38 g/mol (F2). Thus, the ratio is sqrt(38/70.9) = 0.73204.

Question 5

Identify the molecule that effuses the fastest.

Accepted Answer

According to Graham's law of effusion, the rate of effusion is inversely proportional to the square root of the molar mass of the gas. CH₄ has the lowest molar mass among the given options, so it effuses the fastest.

Question 6

A gas mixture contains CO,Ar and H₂.What is the total pressure of the mixture,if the mole fraction of H₂ is 0.35 and the pressure of H₂ is 0.58 atm?

Accepted Answer

The total pressure of the mixture can be calculated using the mole fraction and the partial pressure of H2. The mole fraction of H2 is 0.35, which means that the partial pressure of H2 is 0.35 * total pressure. The partial pressure of H2 is given as 0.58 atm, so the total pressure is 0.58 atm / 0.35 = 1.7 atm.

Question 7

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

Accepted Answer

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

Question 8

Which statement is true about kinetic molecular theory?

Accepted Answer

The principle of kinetic molecular theory is that gases are made up of tiny particles that have constant random motion. The collisions of particles with one another is completely elastic, meaning that there is no loss of energy or momentum during the collisions. A) is false because a single particle does move in a straight line unless it collides with another particle. B) is false because the size of the particle is negligible compared to the volume of the container. D) is false because the average kinetic energy of a particle is directly proportional to the temperature.

Question 9

The following reaction is used to generate hydrogen gas in the laboratory.If 243 mL of gas is collected at 25°C and has a total pressure of 745 mm Hg,what mass of hydrogen is produced? A possibly useful table of water vapor pressures is provided below. Mg(s)+ 2 HCl(aq)→ MgCl₂(aq)+ H₂(g)T (°C)P (mm Hg) 20 17.55 25 23.78 30 31.86

Accepted Answer

The answer of The following reaction is used to generate...

Question 10

A gas mixture consists of N₂,O₂,and Ne,where the mole fraction of N₂ is 0.55 and the mole fraction of Ne is 0.25.If the mixture is at STP in a 5.0 L container,how many molecules of O₂ are present?

Accepted Answer

The answer of A gas mixture consists of N₂,O₂,and Ne,where...

Question 11

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 atm).The molar mass of FeS₂ is 119.99 g/mol. 4 FeS₂(s)+ 11 O₂(g)→ 2 Fe₂O₃(s)+ 8 SO₂(g)

Accepted Answer

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

Question 12

Determine the volume of O₂ (at STP)formed when 50.0 g of KClO₃ decomposes according to the following reaction.The molar mass for KClO₃is 122.55 g/mol. 2 KClO₃(s)→ 2 KCl(s)+ 3 O₂(g)

Accepted Answer

The answer of Determine the volume of O₂ (at STP)formed...

Question 13

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 = 71.10 g/mol and K₂CO₃= 138.21 g/mol. 4 KO₂(s)+ 2 CO₂(g)→ 2 K₂CO₃(s)+ 3 O₂(g)

Accepted Answer

1) Calculate the moles of KO₂ and CO₂: - moles KO₂ = 27.9 g / 71.10 g/mol = 0.392 mol - moles CO₂ = 29.0 L (STP) x 1 mol/22.4 L = 1.295 mol 2) Calculate the limiting reagent: - According to the balanced equation, 4 moles of KO₂ reacts with 2 moles of CO₂. So, the number of moles of CO₂ needed to react with all the KO₂ is: 4/2 x 0.392 mol = 0.784 mol. Since the actual number of moles of CO₂ is greater than this value, CO₂ is in excess and KO₂ is limiting. 3) Calculate the theoretical yield: - According to the balanced equation, 4 moles of KO₂ produces 2 moles of product. So, the number of moles of product from the given amount of KO₂ is: 2/4 x 0.392 mol = 0.196 mol - Theoretical yield = 0.196 mol x 138.21 g/mol = 27.1 g 4) Calculate the percent yield: - Percent yield = (actual yield / theoretical yield) x 100% - Actual yield = 21.8 g - Percent yield = (21.8 g / 27.1 g) x 100% = 80.4%

Question 14

A gas sample contains 0.33 atm of Ne,0.45 atm of Ar,and 0.32 atm of CO.What is the total pressure?

Accepted Answer

The total pressure of a gas mixture is the sum of the partial pressures of each individual gas. Adding the partial pressures: 0.33 atm (Ne) + 0.45 atm (Ar) + 0.32 atm (CO) = 1.1 atm.

Question 15

A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure.A second syringe contains 473 mL of N₂ at 298 K and 2.6 atm.What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

Accepted Answer

First, we need to calculate the amount of CO and N2 gas that will be present in the 1.00 L container at STP.

For CO:
P1V1/T1 = P2V2/T2
1.2 atm x 0.589 L / 325 K = P2 x 1.00 L / 273 K
P2 = 0.433 atm

For N2:
P1V1/T1 = P2V2/T2
2.6 atm x 0.473 L / 298 K = P2 x 1.00 L / 273 K
P2 = 1.54 atm

Now we can calculate the total pressure of the mixture in the container:
Ptotal = PCO + PN2
Ptotal = 0.433 atm + 1.54 atm
Ptotal = 1.97 atm, which we can round to 1.7 atm.

Therefore, the final pressure is 1.7 atm (choice C).

Question 16

How many molecules of XeF₆are formed from 12.9 L of F₂ (at 298 K and 2.60 atm)according to the following reaction? Assume that there is excess Xe. Xe(g)+ 3 F₂(g)→ XeF₆(g)

Accepted Answer

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

Question 17

What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO₂ at 398 K?

Accepted Answer

The answer of What pressure would a gas mixture in...

Question 18

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

Accepted Answer

The answer of Determine the total pressure of all gases...

Question 19

Determine the volume of H₂S (at 375 K and 1.20 atm)needed to produce 55.0 g of S.Assume that there is excess SO₂ present. 2 H₂S(g)+ SO₂(g)→ 3 S(s)+ 2 H₂O(g)

Accepted Answer

To solve this problem, we need to use the ideal gas law to calculate the number of moles of H₂S needed to produce 55.0 g of S, and then use stoichiometry to convert that to the volume of H₂S at the given conditions. Step 1: Calculate the number of moles of S produced. 55.0 g S × (1 mol S/32.06 g S) = 1.718 mol S Step 2: Use stoichiometry to calculate the number of moles of H₂S needed. From the balanced equation, 2 H₂S(g) + SO₂(g) → 3 S(s) + 2 H₂O(g) we can see that 2 moles of H₂S produce 3 moles of S. Therefore, 1.718 mol S × (2 mol H₂S/3 mol S) = 1.145 mol H₂S Step 3: Use the ideal gas law to calculate the volume of H₂S at the given conditions. PV = nRT V = nRT/P V = (1.145 mol)(0.0821 L·atm/mol·K)(375 K)/(1.20 atm) V = 29.3 L Therefore, the answer is B.

Question 20

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...

Quiz 5: Gases

A mixture of 10.0 g of Ne and 10.0 g Ar has a total pressure of 1.6 atm.What is the partial pressure of Ne?

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

Rank the following in order of decreasing rate of effusion. F₂ SF₆ CO Kr

Calculate the ratio of effusion rates of Cl₂ to F₂.

Identify the molecule that effuses the fastest.

A gas mixture contains CO,Ar and H₂.What is the total pressure of the mixture,if the mole fraction of H₂ is 0.35 and the pressure of H₂ is 0.58 atm?

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

Which statement is true about kinetic molecular theory?

A gas mixture consists of N₂,O₂,and Ne,where the mole fraction of N₂ is 0.55 and the mole fraction of Ne is 0.25.If the mixture is at STP in a 5.0 L container,how many molecules of O₂ are present?

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 atm) .The molar mass of FeS₂ is 119.99 g/mol. 4 FeS₂(s) + 11 O₂(g) → 2 Fe₂O₃(s) + 8 SO₂(g)

Determine the volume of O₂ (at STP) formed when 50.0 g of KClO₃ decomposes according to the following reaction.The molar mass for KClO₃is 122.55 g/mol. 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

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 = 71.10 g/mol and K₂CO₃= 138.21 g/mol. 4 KO₂(s) + 2 CO₂(g) → 2 K₂CO₃(s) + 3 O₂(g)

A gas sample contains 0.33 atm of Ne,0.45 atm of Ar,and 0.32 atm of CO.What is the total pressure?

A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure.A second syringe contains 473 mL of N₂ at 298 K and 2.6 atm.What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

How many molecules of XeF₆are formed from 12.9 L of F₂ (at 298 K and 2.60 atm) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3 F₂(g) → XeF₆(g)

What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO₂ at 398 K?

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

Determine the volume of H₂S (at 375 K and 1.20 atm) needed to produce 55.0 g of S.Assume that there is excess SO₂ present. 2 H₂S(g) + SO₂(g) → 3 S(s) + 2 H₂O(g)

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

Quiz 5: Gases

A mixture of 10.0 g of Ne and 10.0 g Ar has a total pressure of 1.6 atm.What is the partial pressure of Ne?

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

Rank the following in order of decreasing rate of effusion. F2 SF6 CO Kr

Calculate the ratio of effusion rates of Cl2 to F2.

Identify the molecule that effuses the fastest.

A gas mixture contains CO,Ar and H2.What is the total pressure of the mixture,if the mole fraction of H2 is 0.35 and the pressure of H2 is 0.58 atm?

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

Which statement is true about kinetic molecular theory?

A gas mixture consists of N2,O2,and Ne,where the mole fraction of N2 is 0.55 and the mole fraction of Ne is 0.25.If the mixture is at STP in a 5.0 L container,how many molecules of O2 are present?

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 atm) .The molar mass of FeS2 is 119.99 g/mol. 4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g)

Determine the volume of O2 (at STP) formed when 50.0 g of KClO3 decomposes according to the following reaction.The molar mass for KClO3 is 122.55 g/mol. 2 KClO3(s) → 2 KCl(s) + 3 O2(g)

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 = 71.10 g/mol and K2CO3 = 138.21 g/mol. 4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g)

A gas sample contains 0.33 atm of Ne,0.45 atm of Ar,and 0.32 atm of CO.What is the total pressure?

A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure.A second syringe contains 473 mL of N2 at 298 K and 2.6 atm.What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.60 atm) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3 F2(g) → XeF6(g)

What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO2 at 398 K?

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

Determine the volume of H2S (at 375 K and 1.20 atm) needed to produce 55.0 g of S.Assume that there is excess SO2 present. 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g)

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

Rank the following in order of decreasing rate of effusion. F₂ SF₆ CO Kr

Calculate the ratio of effusion rates of Cl₂ to F₂.

A gas mixture contains CO,Ar and H₂.What is the total pressure of the mixture,if the mole fraction of H₂ is 0.35 and the pressure of H₂ is 0.58 atm?

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

A gas mixture consists of N₂,O₂,and Ne,where the mole fraction of N₂ is 0.55 and the mole fraction of Ne is 0.25.If the mixture is at STP in a 5.0 L container,how many molecules of O₂ are present?

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 atm) .The molar mass of FeS₂ is 119.99 g/mol. 4 FeS₂(s) + 11 O₂(g) → 2 Fe₂O₃(s) + 8 SO₂(g)

Determine the volume of O₂ (at STP) formed when 50.0 g of KClO₃ decomposes according to the following reaction.The molar mass for KClO₃is 122.55 g/mol. 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

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 = 71.10 g/mol and K₂CO₃= 138.21 g/mol. 4 KO₂(s) + 2 CO₂(g) → 2 K₂CO₃(s) + 3 O₂(g)

A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure.A second syringe contains 473 mL of N₂ at 298 K and 2.6 atm.What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

How many molecules of XeF₆are formed from 12.9 L of F₂ (at 298 K and 2.60 atm) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3 F₂(g) → XeF₆(g)

What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO₂ at 398 K?

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

Determine the volume of H₂S (at 375 K and 1.20 atm) needed to produce 55.0 g of S.Assume that there is excess SO₂ present. 2 H₂S(g) + SO₂(g) → 3 S(s) + 2 H₂O(g)