Question

Ideal Gas Law and Partial Pressures Name Directions: Calculate/answer the following: 1. 7.70 moles of Argon at a pressure of 0.190 atm and at a temperature of 65.8 °C, what is the volume of the container that the gas is in? 2. A sample of gas is 17.0 moles at a temperature of 77.0 °C, and a volume of 98.9 liters, what is the pressure of the gas? 3. 28.0 moles of gas held at a pressure of 580 atm and a temperature of 500. K, what is the volume of the gas? 4. If 4.0g of He is at a pressure of 5.6 atm with a volume of 12.0 L, what is the temperature? 1111111111111 5. If 48.0 g CH, gas in a container with a volume of 60.0 liters and at a temperature of 400. K, what is the pressure inside the container? 6. If an unknown mass of Ne is at a pressure of 1.25 atm, a volume of 31.5 L, and a temperature of 870 "C, calculate the mass of Ne? 7. An unknown quantity of gas at a pressure of 0.500 atm, a volume of 25.0 liters, and a temperature of 300. K. how many grams of gas do I have if it's Hz? 8. How many moles of O, in a 15.0 L tank at 22.0°C with a pressure of 50.0 atm? 9. What is meant by partial pressures? Give Dalton's Law of Partial Pressures and explain in simple terms. 10. The partial pressures of 3 gases are 1.2 atm, 45 atm, and 2.1 atm, what is the total pressure? 11. What is the partial pressure of CO2 in a mixture containing 35% CO, with a total pressure or 50 atm? 12. O, is collected via the water displacement method at 25°C. In the collection vessel, what 2 gases present? If the total pressure is 790.5 mmHg. what is the pressure of the dry gas (just from the O) 13. The air we breathe is a mixture of N. O, and small amounts of others. Assuming 1 atm, if the 21%, the others are 1%, what is the partial pressure of N.? 107 is

Answer 1

1) = 7.70 moles R = 0.082 Lata Korean Pa 0.190 atm. T - 65.8°C = 338.8 K (65.8 +338.84) V = ? we know ? - PV = nRT ») 0.190) v - 67.70) (0.082) (338.8) V= 7.70 40.082 x 338.8 0.190 9) V : 213.91 L 0.190 & v e 1125.84 1 n = 17.0 moles T = 71.000 = 350K vr 98.9 L (77 + 273k) we know, Pvz nRT P = nRT y P ? 17.0 X 0.082 X 350 98.9 3) PS 4.93 atm

3) ms 28.0 moles P- 5810 atom T 500 K v= 2 we know :- PV = nRT va RRT d) V = 28.0% 0.082 x 500 L 58.0 = 19.79 L a 19.8 L. 2) v - 4 as w where, we given moss) Ma notar mass) & 4.0 I given mors of He = 4.0 4.0 (molar moss of He 24.0) P 5.6 aton vr 12.0L T27 we knows & PV = nRT & T PV = 5.6 x 1210 k 1 x 0.082 T a 819.5k