Answer
$1.25\ atm$
Work Step by Step
Given;
Initial temperature $T_1 =5^{\circ} C$
We then convert initial temperatures degree to kelvins:
$T_1 = 5+273 = 278\ k$
Also,
Final temperate $T_2 =75^{\circ} C$
We convert final temperature degree to kelvins:
$T_2 =75+273 =348\ K$
From ideal gas equation, we have:
$PV =nRT$
At constant volume, $P\propto T$.
Then,
$\frac{P_1}{P_2} = \frac{T_1}{T_2}$
$P_2 =P_1 (\frac{T_2}{T_1})$
$P_2 =1\ atm (\frac{348\ k}{278\ k})$
$P_2 =1.25\ atm$
