<p>Name______Per______Date______</p><p>Honors Chemistry: Gas Laws Review Worksheet</p><p>Combined Gas Laws</p><p>1. A gas is at 1.33 atm of pressure and a volume of 682 mL. What will the pressure be if the volume is reduced to 0.419 L? (2.16 atm)</p><p>2. Nitrogen gas is being held in a 14.3 m3 tank at a temperature of 62oC. What will the volume be when the temperature drops to 24oC? (12.6 m3)</p><p>3. A gas storage tank is a 1.72 atm and 35oC. What temperature is the gas at if the pressure increases to 2.00 atm? (354 K)</p><p>4. A gas with a volume of 1.00 L is at 135oC and 844 mm Hg. What is the volume if the conditions change to 14o C and 748 mm Hg? (0.794L)</p><p>5. Calculate the mass of 162 L of chlorine gas, measured at STP. (513 g)</p><p>Dr. Mihelcic Honors Chemistry 1 2008-2009 Ideal Gas Law</p><p>6. Find the pressure in mm Hg produced by 2.35 g of carbon dioxide in a 5.00 L flask at 18oC. (194 mm Hg)</p><p>7. How many grams of carbon monoxide must be placed into a 40.0 L tank to develop a pressure of 965 mm Hg at 23oC? (58.5 g)</p><p>Ideal Gas Law: Density and Molar Mass</p><p>8. At what Celsius temperature will argon have a density of 10.3 g/L and a pressure of 6.43 atm? (31 deg. C)</p><p>9. The density of an unknown gas at 20oC and 749 mm Hg is 1.31 g/L. Calculate the molar mass of the gas. (32.0 g/mol)</p><p>10. Two organic liquids are analyzed, and both are found to be 85.7% carbon and 14.3% hydrogen by weight. At 750 mm Hg and 150oC, both are vapors. At these conditions, an 800.0 mL bottle holds 1.60 g of Compound A, while the same bottle holds 2.22 g of Compound B. Determine the molecular formulas of both compound A and B. (Emp. Formula = CH2; molecular formulas = C5H10 and C7H14)</p><p>Dr. Mihelcic Honors Chemistry 1 2008-2009 Gas Laws and Stoichiometry </p><p>11. Given the following UNBALANCED equation:</p><p>NO (g) + O2 (g)  N2O4 (g)</p><p> a) At constant T and P, how many L of NO will react with 2.4 L of O2 to form N2O4? (4.8 L)</p><p> b) At STP, how many L of N2O4 are formed from the reaction of 4.0 moles of NO? (44.8 L)</p><p>12. a) Write the balanced equation for the decomposition of liquid water to its elements.</p><p> b) How many liters of hydrogen gas, measure at 0.940 atm and 32oC, will result from the decomposition of 10.0 mL of liquid water? (14.8L)</p><p>Graham’s Law</p><p>13. Rank the following from the highest rate of effusion/diffusion to the lowest: C2H6, CH4, C2H4, and C3H8, and then explain your reasoning. (C3H8 > C2H6 > C2H4 > CH4 ranked by molar mass)</p><p>Dr. Mihelcic Honors Chemistry 1 2008-2009</p>