Calculate the approximate volume (in liters) of a 0.400 mol sample of gas at 20.0 °C and a pressure of 2.43 atm.

Example #1: A sample of gas at 25.0 °C has a volume of 11.0 L and exerts a pressure of 660.0 mmHg. How many moles of gas are in the sample?

Example #2: A sample of gas at 28.0 °C has a volume of 6.20 L and exerts a pressure of 720.0 mmHg. How many moles of gas are in the sample?

Example #3: Calculate the approximate volume of a 0.400 mol sample of gas at 11.0 °C and a pressure of 2.43 atm.

Example #4: Calculate the approximate temperature of a 0.300 mol sample of gas at 780. mmHg and a volume of 6.00 L.

Example #5: What is the pressure exerted by 2.3 mol of a gas with a temperature of 40. °C and a volume of 3.5 L?

Example #6: A sample of dry gas weighing 2.1025 grams is found to occupy 2.850 L at 22.00 °C and 740.0 mmHg. How many moles of the gas are present?

Example #7: Using the problem above, what is the molar mass of the gas?

Example #8: At STP, a 5.00 L flask filled with air has a mass of 543.251 g. The air in the flask is replaced with another gas and the mass of the flask is 566.107 g. The density of air is 1.29 g/L. What is the gas that replaced the air?

Example #9: A vessel at 25.0 °C is evacuated to a point where the amount of gas remaining is 5.00 x 109 molecules per m3. What is the pressure in the vessel?

Example #10: Of the following gases, which has density of 0.906 g/L at 315 K and 1.16 atm.

Example #11: A 0.105 g sample of an unknown diatomic gas contained in a 125 mL vessel has a pressure of 560 torr at 23 &175;C. What is the molar mass of the gas? What is the identity of the gas?

Example #12: If 1.0 g of each of the following gases is taken at STP, which one would occupy the greatest volume?

(a) CO

(b) H2O

(c) CH4

(d) NO

(e) They would all occupy the same volume.

Example #13: If 12.8 g of liquid helium at 1.7 K is completely vaporized. What volume does the helium occupy at STP?

Example #14: An elemental gas (meaning that it is made from one element) has a mass of 10.3 grams. It occupies 58.4 L at 1.00 atm and 2.50 °C. Identify the gas.

Example #15: An elemental gas (meaning that it is made from one element) has a mass of 10.3 grams. It occupies 4.27 L at 1.00 atm and 85.0 °C. Identify the gas.

Explanation:

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)