Molar volume---2013
1.
How many grams of oxygen gas is needed to produce 2.35 liters of gas at STP?
2.
How many liters are equivalent to having 65.2 grams of water vapor at STP?
3.
What is the density and molar mass of a gas if the gas has a mass of 3.55 grams and a volume of 4.25 liters at
STP? (2 answers required)
4.
A reaction produced 2.00 grams of gas occupying 1.50 liters when collected at STP. What is the density of the gas? Calculate the molar mass of the gas. (2 answers required)
5.
95.3 grams of ammonia (NH
3
) are recovered at STP, how many liters would this equal?
1.
If 600. ml of hydrogen gas is produced through a replacement reaction involving solid iron and sulfuric acid at
STP, how many grams of Iron (III) sulfate are produced?\
2.
If 14.7 grams of sulfuric acid were used in the above reaction, how many liters of hydrogen would be collected at STP?
3.
Using the equation Sulfur dioxide (g) and water (l)  Hydrogen sulfite (aq) -- If 95.0 grams of water was used, how many liters of the sulfur dioxide would be required if the reaction was performed at STP?
Potassium hydroxide reacts with ammonium sulfate to produce potassium sulfate (s), ammonia (g), and water (l)
4.
Using the above reaction, if 12.5 L of ammonia was produced at STP, how many grams of Potassium sulfate solution was used?
5.
If 2.25 L of ammonia was produced at STP how many grams of ammonium sulfate were used?
6.
When a 115 gram piece of aluminum metal is added to excess sulfuric acid how many liters of hydrogen gas is formed at STP?
7.
How many grams of Sulfuric acid are needed if 455 mL of hydrogen gas is formed at STP?

Ideal Gas Law
1.
A sample of ammonia contains .555 moles at 1.03 atm and 25 C. What is the volume of this gas?
2.
A 525 mL flask is completely filled with hydrogen gas. The experiment was performed at 23 C and 772 mm Hg.
How many moles of the gas was collected?
What is the mass of the gas that was collected?
What is the density of the gas?
3.
6.38 grams of oxygen was recovered during an experiment performed at 27 C. The volume of the gas was recorded as being 634 mL. What is the pressure at which this experiment was performed?
4.
What is the molar mass (grams/mole) of a gas that has a volume of 1.25 liters, a mass of 5.17 grams when collected at 28 C with a pressure of 742 mm Hg.?
5.
If a sample of nitrogen dioxide occupies 4.75 liters at 300. K and contains 0.860 moles, what pressure would be exerted on the gas?
6.
A sample of 750. mL of carbon dioxide contains .215 moles at 57 C. What pressure is used in the experiment?
7.
What temperature is required to produce .365 moles of hydrogen gas which is collected at 1.25 atm and has a volume of 6.75 liters?
8.
When a gas had a volume of 655 mL at a pressure of 752 mmHg, the number of moles were determined to be
.0275. What temperature in Celcius is being used in the experiment?
9.
What volume in liters, would 2.00 moles of oxygen gas occupy is the gas has a pressure of 1.25 atm at 300 K?
10.
If a 4.00 gram sample of oxygen gas exerts a pressure of 675 mmHg at 57 C. What is the volume in liters of this gas ?
11.
A 1.25 liter sample of gas exerts a pressure of 1.06 atm at a temperature of 250. K . How many moles of gas would be contained in this sample?
12.
The temperature of the gas being measured is -50c. (very cold). At this temperature the gas occupies 750. mL and has a pressure of 700 mm Hg. Determine the number of moles of gas.
13.
A 3.50 liter container is filled with NH
3
at 27 c and 700 mmHg. Determine the mass (number of grams) under these conditions.
14.
What is the molar mass of a 1.50 liter sample of gas that is collected at 320 K and has a pressure of 1.08 atm when the mass was found to be 3.50 grams?
15.
A 0.650 gram sample of an unknown gas was collected over water at 777 mmHg at a temperature of 18.0 C.
The volume of the gas was 525 mL. Under these conditions determine the molar mass of the gas
A reaction involving solid iron and sulfuric acid a produces Iron (III) sulfate and hydrogen gas
1.
When 950. mL of the hydrogen gas was collected over water at a temperature of 25 Celsius and at a barometric pressure of 765 mmHg, how many grams of sulfuric acid were needed?
2.
If using the above equation 95.6 grams of solid Fe were used, what volume of hydrogen gas would be produced at 1.05 atm and 22 Celsius?
Potassium hydroxide reacts with ammonium sulfate to produce potassium sulfate (s), ammonia (g), and water (l)
1.
If 15.0 grams of Potassium hydroxide reacts with ammonium sulfate to produce potassium sulfate (s), ammonia
(g), and water (l), what volume of ammonia would be collected over water at 775 mmHg and 30 Celsius?
2.
If 2.25 L of ammonia was produced at 1.10 atm and 25 Celsius, how many grams of ammonium sulfate were used?