Question

Given constant volume, what pressure would `50*atm` of gas at `0` `""^@C`, develop at a temperature of `300` `""^@C`?

Answer 1

Gay Lusaac's law holds that at constant volume, `((P_1)/T_1 = (P_2)/T_2)` (i.e. pressure is proportional to temperature at constant volume).

Explanation:

So, `P_2` `=` `(P_1T_2)/T_1` `=` `(50.0*atmxx273K)/(573K)` `=`

`?? atmospheres`

This is reasonable on the basis that we would expect a given quantity of gas to exert less pressure at lower temperature. Note that I converted the temperature to the Kelvin scale in order to avoid multiplying by `0`.