Answer : The final pressure of the gas will be, 710.56 torr
Explanation :
According to the Charles' Law, the pressure of the gas is directly proportional to the temperature of the gas at constant volume and the number of moles of gas.
\(P\propto T\)
or,
\(\frac{P_1}{P_2}=\frac{T_1}{T_2}\)
where,
\(P_1\) = initial pressure of the gas = 660 torr
\(P_2\) = final pressure of the gas = ?
\(T_1\) = initial temperature of the gas = \(22^oC=273+22=295K\)
\(T_2\) = final temperature of the gas = \(44.6^oC=273+44.6=317.6K\)
Now put all the given values in the above formula, we get the final pressure of the gas.
\(\frac{660torr}{P_2}=\frac{295K}{317.6K}\)
\(P_2=710.56torr\)
Therefore, the final pressure of the gas will be, 710.56 torr
