A constant volume of gas is heated from 25.0ºC to 150.ºC. If the initial pressure was 760. torr, what is the final pressure?

The final pressure of the gas is 1078.79 torr

Explanation:

The initial pressure (P₁)= 760 torr

The initial temperature (T₁)=25°C

The final temperature (T₂)=150°C

The final pressure (P₂)

Since the temperature of the gas is  in °C, we need to convert them to Kelvin units

We know that 0°C=273 K

Thus T₁=273+25=298K

Similarly T₂ =273+150=423K

From the Gay-Lussac's law, we know that-

P₁/T₁ = P₂/T₂

Where P₁,P₂,T₁,T₂ covey the meaning as described earlier

Substituting the value we get-

(760/298) = P₂/423

P₂=(760*423)/298

Thus the final pressure of the gas is 1078.79 torr.

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explanation:

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