1. 18.0 g of oxygen gas occupies 10.5 L in an expandable container at a particul

Question

1. 18.0 g of oxygen gas occupies 10.5 L in an expandable container at a particular temperature and pressure. What volume will the the gas occupy if 54.0 g of oxygen are added to container. Assume the pressure and temperature are held constant.

2. 12.0 g of nitrogen gas exerts a pressure of 1.05 atm in a rigid container at a particular temperature. What pressure will the the gas exert if 24.0 g of nitrogen are added to container. Assume the volume and temperature are held constant.

3. What is the volume of a mixture of 30.0 g of N2 and 58.0 g of O2 at 31.5°C and 660. mm Hg? Assume the gases do not react with each other.

Explanation / Answer

Ans 1.

The total amount of gas after adding 54 g = 18 + 54 = 72 g

According to the ideal gas law ,

pV = nRT

So you may see volume is directly related to number of moles of gas , if all other values are kept constant.

n1 for 18 g = 18/16

n2 for 72g = 72/16

V1 n2 = V2 n1

10.5 x 72/16 = V2 x 18/16

V2 = 42 L

So the volume of gas is now 42 L

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