Question

A gas mixture contains 1.32 g N2 and 0.87 g O2 in a 1.65-L container at 20 °C. Calculate the mole fraction of N2. Calculate the mole fraction of O2. Calculate the partial pressure of N2. Calculate the partial pressure of O2.

Name: a gas mixture contains 132 g n2 and 087 g o2 in a 165 l container at 20 c calculate the mole fraction of n2 calculate the mole fraction of o2 calculate the partial pressure of n2 calculate t 96388
Uploaded: 2023-08-05T06:51:26-08:00
Duration: 4 min 4 s
Channel: Madhur L
Description: a gas mixture contains 132 g n2 and 087 g o2 in a 165 l container at 20 c calculate the mole fraction of n2 calculate the mole fraction of o2 calculate the partial pressure of n2 calculate t 96388

          A gas mixture contains 1.32 g N2 and 0.87 g O2 in a 1.65-L container at 20 °C. 
Calculate the mole fraction of N2. 
Calculate the mole fraction of O2. 
Calculate the partial pressure of N2. 
Calculate the partial pressure of O2.

Added by Antonio A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

08/05/2023

Step 1

To do this, we need to use the ideal gas law: PV = nRT where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. We know that the volume is 1.65 L and the temperature is 20 °C, which is 293 K. We also Show more…

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A gas mixture contains 1.32 g N2 and 0.87 g O2 in a 1.65-L container at 20 °C. Calculate the mole fraction of N2. Calculate the mole fraction of O2. Calculate the partial pressure of N2. Calculate the partial pressure of O2.