Name: Nuclear Chemistry and Gases Review Worksheet Nuclear Chemistry Section: 1. Define radioactivity. 2. What are the three types of radiations? Give their notations and charges

3. Write the balanced nuclear equations for the following: a. Alpha decay of Fluorine-20 b. Beta decay of Neptunium-239 4. What is half-life of a radioactive sample?

5. A skull believed to belong to an early human being is found to have a carbon-14 content of 3.125 % of that found in living organisms. How old is the skull? The half-life of carbon-14 is 5730 years.

6. Radium-223 decays with a half-life of 11.4 days. How long will it take for a 0.240 mol sample of radium to decay to 1.50x10-2 mol?

7. A radioactive sample contains 1.55 g of an isotope with a half-life of 3.8 days. How much of the isotope in grams will remain after 11.4 days?

8. A radioactive sample contains 23.22 g of an isotope with a half-life of 22 minutes. How much of the isotope in grams will remain after 50 minutes?

9. Define: a. Nuclear fission –

b. Nuclear Fusion –

10. Give two uses of radioactivity.

Behavior of Gases Section: 1. What are the four variable used to describe a gases? Mention two common units for each variable that you have used.

2. Convert the following: Show your work: a. 45 °C = __________ K

b. 452.1 mL = _____________ L

c. 3.45 atm = ____________ mm Hg

d. 12 g of Nitrogen gas = _________ mols

e. 785 mm Hg = ____________ kPa

f. 2.84 mols of carbon dioxide gas = __________

g g. 345 K = ___________ °C

h. 802 torr = ___________ atm

3. A gas occupies 27.5 mL at a pressure of 792.5 mm Hg. Determine the volume if the pressure is reduced to 0.813 atm. Assume temperature and moles of the gas are constant.

4. 300 mL of O2 are collected at a pressure of 645 mm Hg. What volume will this gas have at 760 mm Hg pressure?

5. The temperature of a 6.25 L sample of gas is changed from 25.0 °C to 40.0 °C. What will the volume of this gas be at the new temperature if the pressure is held constant?

6. If a gas in a closed container is pressurized from 15.0 atmospheres to 150.0 atmospheres and its original temperature was 25.0 °C, what would the final temperature of the gas be?

7. What is the final volume of a 500.0 mL gas sample that is subjected to a temperature change from 22.0 °C to 32.0 °C and a pressure change from 760.0 mm Hg to 350.0 mm Hg?

8. Determine the number of grams of carbon dioxide in a 450.0 mL tank at 1.80 atm and -12.0 °C.

9. 6.89 g of H2 is contained in a 2.00 L container at 30.0 °C. What is the pressure in this container in mm Hg?

10. A container holds three gases: nitrogen, carbon dioxide, and helium. The partial pressures of the three gases are 3.00 atm, 5.00 atm, and 7.00 atm, respectively. What is the total pressure inside the container?

11. If 60.0 L of nitrogen dioxide gas is collected over water at 40.0 °C when the atmospheric pressure is 768.0 mmHg, what is the partial pressure (pressure of dry gas) of the nitrogen? The water vapor pressure at 40.0 °C is 55.324 mm Hg.

12. A mixture of 18.0 grams of hydrogen, 74.0 grams of nitrogen, and 3.0 moles of oxygen are placed in a flask. When the partial pressure of the oxygen is 98.00 mm Hg, what is the total pressure in the flask?

13. A tank contains 5.00 moles of O2, 8.00 moles of neon, 6.00 moles of H2S, and 4.00 moles of argon at a total pressure of 1620.0 mmHg. Complete the following table O2

Ne

H2 S

Ar

Total

Moles Mole Fraction Partial Pressure

14. If equal amounts of oxygen and nitrogen gases are placed in a porous container and allowed to escape, which gas will escape faster and how much faster?

15. If an unknown gas diffuses 0.25 times that of Helium gas, what is the molar mass of the unknown gas?

16. Chlorine trifluoride, ClF3, is a valuable reagent because it can be used to convert metal oxides to metal fluorides: 6 NiO(s) + 4 ClF3(g) à 6 NiF2(s) + 2 Cl2(g) + 3 O2(g) If 50.00 g of NiO is used in the reaction, what volume (in liters) of ClF3 gas is required to complete the reaction at a pressure of 250 mm Hg and 20 °C?

17. Sodium azide required for automobile air bags is made by the reaction of sodium metal with dinitrogen oxide in liquid ammonia: 3 N2O(g) + 4 Na(s) + NH3(l) à NaN3(s) + 3 NaOH(s) + 2 N2(g) What is the mass of Na that is required to react with 35.0 L of N2O in a container with a pressure of 2.12 atm and 23 °C.

18. State the postulates of Kinetic Molecular theory.

19. State the difference in behavior between real gases and ideal gases.

20. Under what conditions does a real gas behave as an ideal gas? Explain why?

21. List all the equations used to understand gaseous behavior.