Asample of hydrogen gas at a temperature of 275 k and a pressure of 0.456 atm is allowed to expand to a pressure of 845 mmhg. what is the new temperature of the gas?

Let's assume that volume of the gas is a constant.

We can use Gay-lussac's pressure temperature law to solve this problem.

It says the pressure of a given amount of gas is directly proportional to its temperature in Kelvin when the volume is a constant.
P α T 

Where P is the pressure and T is the temperature in Kelvin of the gas. We can use this for two situations as,

P₁/T₁ = P₂/T₂

P₁ = 0.456 atm

T₁ = 275 K

P₂ = 845 mmHg = 1.112 atm

T₂ = ?

By applying the formula,
0.456 atm / 275 K = 1.112 atm / T₂                  

                   T₂  = (1.112 atm / 0.456 atm) x 275 K
                   T₂  = 670.6 K

Hence, the temperature of the hydrogen gas is 670.6 K

 

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