1) WHAT IS STP CONDITION? 2) Calculate the density of xenon gas at a pressure of 742 mmHg and a temperature of 45 °C. 3) A gas has a density of 1.43 g/L at a temperature of 23 °C and a pressure of 0.789 atm. Calculate its molar mass. 4) A sample of gas has a mass of 827 mg. Its volume is 0.270 L at a temperature of 88 °C and a pressure of 975 mmHg.Find its molar mass. 5) A 1.00-L mixture of helium, neon, and argon has a total pressure of 662 mmHg at 298 K. If the partial pressure of helium is 341 mmHg and the partial pressure of neon is 112 mmHg, what mass of argon is present in the mixture? 6) A sample of hydrogen gas is mixed with water vapor. The mixture has a total pressure of 755 torr, and the water vapor has a partial pressure of 24 torr. What amount (in moles) of hydrogen gas is contained in 1.55 L of this mixture at 298 K? 7) 12.5-L scuba diving tank contains a helium-oxygen (heliox) mixture of 24.2 g of He and 4.32 g of O2 at 298 K. Calculate the mole fraction and partial pressure of each component in the mixture and the total pressure of the mixture 8) A common way to make hydrogen gas in the laboratory is to place a metal such as zinc in hydrochloric acid. The hydrochloric acid reacts with the metal to produce hydrogen gas, which is then collected over water. Suppose a student carries out this reaction and collects a total of 154.4 mL of gas at a pressure of 742 mmHg and a temperature of 25 °C. What mass of hydrogen gas (in mg) does the student collect? 9) A sample of N2 has 1.70 moles and occupies 3.80 L at 25.0˚C. What volume will it occupy with 2.60 moles? How many moles are in a sample that occupies 1.45 L? 10) 22.00 g of CO2 has a volume of 50.00 L and a pressure of 0.8210 atm. What must be the  11) Find ΔHrxn for the reaction:3 H2(g) + O3(g) 3 H2O(g) Use these reactions with known ΔH values: 2 H2(g) + O2(g) 2 H2O(g) ΔH = –483.6 kJ, 3 O2(g) 2 O3(g) ΔH = +285.4 kJ 12) A 55.0-g aluminum block initially at 27.5 °C absorbs 725 J of heat. What is the final temperature of the aluminum? 13) What mass of butane in grams is necessary to produce 1.5 × 103 kJ of heat? What mass of CO2 is produced? C4H10(g) + O2(g) 4 CO2(g) + 5 H2O(g) ΔHrxn = –2658 kJ  14) A cylinder equipped with a piston expands against an external pressure of 1.58 atm. If the initial volume is 0.485 L and the final volume is 1.245 L, how much work (in J) is done?

Chem 1A

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