Central High School Name ______

Honors Chemistry

Date______Block ______

Gas Laws #2

In Questions 1 through 3 the temperature and the amount of gas are both constant.

1. Which gas law can be applied to a gas under changing conditions of pressure and volume when the temperature and amount of gas remain constant?

2. Calculate the new pressure if a 2300 mL of a gas at a pressure of 1.88 atm is allowed to contract to a volume of 2.21 L.

3. Calculate the new volume if a 13.40 L of a gas at a pressure of 1.51 atm is subject to a new pressure of 65 mmHg.

In Questions 4 through 6 the pressure and the amount of gas are both constant.

4. Which gas law can be applied to a gas under changing conditions of volume and temperature when the pressure and amount of gas remain constant?

5. Calculate the new volume if 1.23 L of a gas at 32oC is subjected to a drop in temperature of 20 degrees Celsius.

6. Calculate the new volume if a 12.78 L of a gas at –50oC is heated to a temperature of 28oC.

In Questions 7 and 8, the pressure and temperature of gas are both constant.

7. Which gas law can be applied to a gas under changing conditions of volume and number of moles when the pressure and temperature remain constant?

8. What mass of oxygen gas occupies 10.8 L if 4.2 g of oxygen under the same conditions occupies 100 L?

In questions 9 and 10, assume the gas behaves ideally.

9. A sample of a group I bromide weighing 2g was vaporized at 504oC and 1 atm pressure to produce 1238.0 cm3 of vapor. Identify the group I metal present in the compound.

10. What volume does 1.24 g of oxygen gas occupy at 5.2oC and 2.04 atm?

11. If 5.0 g of nitrogen gas and 5.0 g of oxygen gas are placed in a 2.0 L container at 65oC, what will the partial pressure of each gas be?

12. What will the total pressure in the container in question 11 be?

13. Which gas law allows the simple calculation of the answer to question 12?

In questions 14 and 15, assume 1 mol of any gas occupies 22.4 L at standard temperature and pressure (s.t.p).

14. What volume of hydrogen is obtained when 13.00g Magnesium reacts with an excess of dilute sulfuric acid at s.t.p?

Mg(s) + H2SO4(aq) è MgSO4(aq) + H2(g)

15. What volume of oxygen, at s.t.p, is required to burn exactly 11.6 L of methane (CH4(g)), according to the reaction below?

CH4(g) + 2O2(g) è CO2(g) + 2H2O(g)

16. What is the Molar Mass of a vapor that effuses 1/5 as fast as hydrogen?

17. How much faster does Helium escape through a porous container than SO2?

18. Compare the velocity for Helium and Nitrogen at 20oC.

12. Small quantities of hydrogen gas can be prepared in the laboratory by the following reaction:

Zn(s) + 2HCl(aq) çè ZnCl2(aq) + H2(g)

Assume you carried out this experiment and collected 454 mL of hydrogen gas over water. The gas mixture collected includes hydrogen and water vapor. The temperature of this gas mixture was 23.0 °C and the total pressure was 712 mm Hg. How many moles of hydrogen did you prepare? The vapor pressure of water at 23.0°C is 19.8 mm Hg. (4)

13. Calculate which one of the following sulfides would effuse at a rate equal to 70.6% of the rate of a gas with a Molar Mass of 17 g/mol? H2S, Na2S or CaS.