10. The density of an unknown gas is 0.089 g/L at STP. What is the molar mass of

Question

10. The density of an unknown gas is 0.089 g/L at STP. What is the molar mass of gas? 11. The larger the density of a gas, the (larger, smaller, same) will be the molar mass of the gas. EXPLAIN. 12. Air is 78% N2 and 21902 (w/w). What is the approximate density of air at STP? will a balloon filled with argon sink or float in air? HINTS: a. Find the approximate weighted average molar mass of air. b. Find the STP density of air. c. Find the STP density of argon. d. Compare the densities. A gas having a heavier density will sink in a gas with a lighter density 13. 15.6 mL of O2 gas at a pressure of 750 torr and 23°C is collected when a 1.0 g sample of a mixture of H,02 and water is treated with KMnO via the reaction: What is the percent H202 of the sample? HINTS: a From the volume, temperature and pressure of O2 gas, calculate the moles of O2 collected. Use R 62.4 L tom/K mol b. From the equation, what is the mole relationship of H 0; to O2? Use it to determine c. Calculate grams of H2O2 in the sample, then % H02 in the sample. the moles of H202 in the sample. 278

Explanation / Answer

10)

At stp, pressure is 1 atm and temperature is 273 K

P = 1 atm

T = 273 K

density = 0.089 g/L

Lets derive the equation to be used

use:

p*V=n*R*T

p*V=(mass/molar mass)*R*T

p*molar mass=(mass/V)*R*T

p*molar mass=density*R*T

Put Values:

1 atm * MM = 0.089g/L * 0.08206 atm.L/mol.K *273.0 K

MM = 1.9938 g/mol

Answer: 1.99 g/mol

11)

We have:

p*molar mass=density*R*T

molar mass and density are directly proportional

So, large density implies greater molar mass

Answer: larger molar mass

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