Solution

Assuming that hydrogen (H_2) behaves has an ideal gas
We have
$n=1mol$
$T=0\degree C=273K$
$P=const$
Q=nC_p\Delta T
we know that $C_p=\frac{(i+2)R}{2}$
where i is the number of degrees of freedom, which is 5 for hydrogen (diatomic gas)
$C_p=\frac{7R}{2}$
so $Q=\frac{7nR\Delta T}{2}$
and with Charles's Law ( $\frac{V}{T}=const$ )
$\frac{V}{T_1}=\frac{2V}{T_2}$
$T_2=2T_1$ , so $\Delta T=T_2-T_1=2T_1-T_1=T_1$
and substituting in the heat
$Q=\frac{7nRT_1}{2}$
$Q\approx 7948.5J$
and the work for a constant pressure
$W=P\Delta V=P(2V-V)=PV=nRT_1$
$W\approx 2271J$
It's an isobaric expansion work