1. If a gas at 37 degrees Celcius occupies 2.9 L at a pressure of 380 torr, what will be the new
volume at a pressure of 1.5 atm?
LAW:

0.96 litre will be the new volume of the gas at a pressure of 1.5 atm.

Explanation:

Data given:

initial temperature of the gas = 37 degrees

initial pressure P1 = 380 torr or  0.5 atm

initial volume of gas  V1= 2.9 litre

final volume V2 = ?

final pressure P2 = 1.5 atm

Assuming that temperature remains constant, the formula used is of Boyle's Law:

P1V1 = P2V2

Rearranging the equation to know the value of final volume of the gas:

V2 =

V2 =

V2 = 0.96 LITRE

the volume of the gas decreases as the pressure of the  gas increases.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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