DMS - Partial Pressure and Gas Stoichiometry

A mixture of gases contains 2.5 moles N2, 1.3 moles O2, and 0.75 moles Ar and has a total pressure of 0.879 atm. What is the partial pressure of O2 in the sample?

0.25 atm

The total pressure of a sample is 1.5 atm, and the partial pressure of He in the sample is 0.48 atm. What is the mole fraction of He in the sample?

0.32

The total pressure of a sample is 0.925 atm, and the partial pressure of CO2 in the sample is 0.302 atm. What is the mole fraction of CO2 in the sample?

0.326

The mole fraction of Ar in a mixture of gases is 0.829 with a partial pressure of 0.341 atm. What is the total pressure of the sample?

0.411 atm

A mixture of gases contains 4.25 grams of CO2 and 2.25 grams of CH4 and has a total pressure of 0.900 atm. What is the partial pressure of CH4?

0.533 atm

A mixture of gases contains 25.0 grams of CO2 and 3.75 grams of He and has a total pressure of 0.875 atm. What is the partial pressure of He?

0.545 atm

The total pressure of a sample is 1.35 atm, and the partial pressure of N2 in the sample is 0.742 atm. What is the mole fraction of N2 in the sample?

0.550

A mixture of gases contains 0.55 moles He, 0.45 moles Ne, and 0.95 moles Ar and a total pressure of 1.2 atm. What is the partial pressure of Ar in the sample?

0.59 atm

A mixture of gases contains 12.0 grams of N2 and 15.0 grams of Ar and has a total pressure of 1.32 atm. What is the partial pressure of N2?

0.704 atm

What is the partial pressure of nitrogen if a mixture of air contains 0.21 atm of oxygen and 0.008 atm of trace gases and the total pressure is 1.00 atm?

0.78 atm

A mixture of gases contains 1.3 moles H2, 1.9 moles N2, and 0.35 moles He and a total pressure of 2.2 atm. What is the partial pressure of H2 in the sample?

0.81 atm

What is the partial pressure of carbon dioxide if the total pressure of the mixture is 2.671 atm and the mixture contains carbon dioxide and 1.82 atm of oxygen?

0.85 atm

What is the partial pressure of carbon dioxide if the total pressure of the mixture is 2.671 atm and the mixture contains carbon dioxide and 1.82 atm of oxygen?

0.85 atm The partial pressure of carbon dioxide is 0.85 atm. According to Dalton's law of partial pressures, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each of the individual gases. Therefore, the partial pressure of carbon dioxide can be calculated as follows: PTotal = PCO2 + PO2 2.671 atm = PCO2 + 1.82 atm PCO2 = 0.85 atm

What volume of H2 is produced at 315 K and 1.25 atm when 3.50 grams of Zn reacts with excess HCl? Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq)

1.11 L

The mole fraction of CH4 in a mixture of gases is 0.285 with a partial pressure of 0.498 atm. What is the total pressure of the sample?

1.75 atm

What is the total pressure within a gas cylinder if the cylinder consists of 6.82 atm of helium, 7.3 atm of krypton, and 0.343 atm of neon?

14.5 atm

What is the partial pressure of xenon if the total pressure of the mixture is 7.524 atm and the mixture contains xenon, 3.78 atm argon and 1.46 atm of neon?

2.28 atm

What volume of CO2 is produced at 275 K and 0.950 atm when 12.5 grams of HNO3 reacts with excess Na2CO3? 2 HNO3(aq) + Na2CO3(aq) → 2 NaNO3(aq) + CO2(g) + H2O(l)

2.36 L

What volume of CO2 is produced at 275 K and 0.950 atm when 12.5 grams of HNO3 reacts with excess Na2CO3? 2 HNO3(aq) + Na2CO3(aq) → 2 NaNO3(aq) + CO2(g) + H2O(l)

2.36 L The volume of CO2 produced at 275 K and 0.950 atm is 2.36 L. First, determine the moles of CO2 produced using stoichiometry. Then, use the ideal gas law to determine the volume of CO2.

The mole fraction of He in a mixture of gases is 0.492 with a partial pressure of 1.25 atm. What is the total pressure of the sample?

2.54 atm

What pressure of O2 is needed at 298 K in a volume of 10.00 L container to completely combust 10.0 grams of C2H6? 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)

2.84 atm

What pressure of O2 is needed at 298 K in a volume of 10.0 L container to completely combust 10.0 grams of CH4? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)

3.06 atm

What volume of SO2 is produced at 325 K and 1.35 atm when 15.0 grams of HCl reacts with excess K2SO3? 2 HCl(aq) + K2SO3(aq) → 2 KCl(aq) + H2O(l) + SO2(g)

4.07 L

What is the total pressure within a gas cylinder if the cylinder consists of 6.2 atm of sulfur dioxide and 1.205 atm of helium?

7.4 atm

What is the total pressure within a gas cylinder if the cylinder consists of 4.54 atm of oxygen, 1.2 atm of nitrogen, and 2.61 atm of argon?

8.4 atm

How many moles of hydrogen gas, H2, are present if the reaction conditions are 295 K, 1.1 atm, and 0.35 L of hydrogen, H2? 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g) Now, how many grams of hydrogen gas, H2, are present?

n = 0.016 moles of H2 grams = 0.032 g of H2

How many moles of ethane, C2H6, are present if the reaction conditions are 305 K, 1.3 atm, and 2.5 L of ethane, C2H6? If it burns in the presence of excess oxygen, O2, according to the chemical reaction shown below, how many grams of carbon dioxide, CO2, are formed? 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)

n = 0.13 moles of C2H6 grams = 11 g of CO2

How many moles of carbon dioxide, CO2, are produced if the reaction conditions are 325 K, 1.6 atm, and 5.3 L? If the carbon dioxide, CO2, is produced according to the chemical reaction shown below, how many grams of propane, C3H8, were required? 2 C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)

n = 0.32 moles of CO2 grams = 9.4 g of C3H8

How many moles of carbon dioxide, CO2, are produced if the reaction conditions are 325 K, 1.6 atm, and 5.3 L? If the carbon dioxide, CO2, is produced according to the chemical reaction shown below, how many grams of propane, C3H8, were required? 2 C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)

n = 0.32 moles of CO2 grams = 9.4 g of C3H8 Using the ideal gas law, the moles of carbon dioxide, CO2, produced for the reaction would be 0.32 moles. All of the variables are in the correct units, so no additional conversions were required. The calculation would be completed as follows: Using stoichiometry, the number of grams of propane, C3H8, that would be required is 9.4 g. The calculation would be completed as follows, using the balanced chemical equation: 2 C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)

How many moles of nitrogen dioxide, NO2, are present if the reaction conditions are 330 K, 2.46 atm, and 4.8 L? If the nitrogen dioxide, NO2, reacts in the presence of excess water, H2O, according to the chemical reaction shown below, how many grams of oxygen, O2, are formed? 4 NO2(g) + 6 H2O(g) →7 O2(g) + 4 NH3(g)

n = 0.44 moles of NO2grams = 25 g of O2

How many moles of oxygen, O2, are present if the reaction conditions are 425 K, 3.43 atm, and 5.72 L? If the oxygen, O2, reacts with excess hydrogen, H2, according to the chemical reaction shown below, how many grams of water, H2O, are formed? 2 H2(g) + O2(g) → 2 H2O(g)

n = 0.562 moles of O2 grams = 20.3 g of H2O

How many moles of iodine, I2, are present if the reaction conditions are 250 K, 2.00 atm, and 11.7 L? If the iodine, I2, reacts according to the chemical reaction shown below, how many grams of nitrogen triiodide, NI3, are formed? N2(g) + 3 I2(g) → 2 NI3(g)

n = 1.1 moles of I2grams = 290 g of NI3

How many moles of methane, CH4, are present if the reaction conditions are 398 K, 2.78 atm, and 13.6 L? If the methane, CH4, is produced according to the chemical reaction shown below, how many grams of hydrogen sulfide, H2S, are formed? CS2(g) + 4 H2(g) → CH4(g) + 2 H2S(g)

n = 1.16 moles of CH4 grams = 79.1 g of H2S