Question

Classwork: Ch. Gases Name 1. A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmg What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 ml? 2. A sample of carbon monoxide gas occupies 3.20 L at 125°C. At what temperature will the gas occupy a volume of 154 Lif the pressure remains constant? 3. What is the volume (in liters) occupied by 49.8 g of HCl at STP? 4. Argon is an inert gas used in lightbulbs to retard the vaporization of the filament. A certain lightbulb containing argon at 1.20 atm and 18 °C is heated to 85°C at constant volume. What is the final pressure of argon in the lightbulb (in atm)? 5. A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and 27.0°C. What is the molar mass of the gas? 6. What is the volume of CO2 produced at 37°C and 1.00 atm when 5.60 g of glucose are used up in the reaction: CH3O4 (8) + 60 (8) Bộ 6CO2 (g) + 6HẠO (1) 7. A sample of natural gas contains 8.24 moles of CH., 0421 moles of He, and 0.116 moles of CHs. If the total pressure of the gases is 1.37 atm, what is the partial pressure of propane (C.H.)?

Answer 1

- PV = P2 a 726x946 = P₂ x 154 = [4459 7 mon of Hy 73 v= nRT v 49.5% Doxa 14 273 130.62 1.0x36.5 & PU=ART a pre Mall RT Man RT M M= mass XRT pv 4.65X 0.0831X300 2.108 lo - [5405 g/mol © moles of glucose = 5:00 0.0311 may mores of Cog formed - 6x0.0311= 0.187 mot V=MRT V O - MRT VE 0-187 x 0. 08214310 14.75/2 1.o
7)
= 0.0132 0.116 0.11 6+ 0.421 +8-24 mole fraction of C3Hg(x ) = Platte = XAR = 0.0 Bax 1.37 -10. 0187 ctm