How would Dalton's law be affected when there are two ideal gases in a container at different temperatures?
Determine total number of moles of air in bulbs:
$$n=\frac{PV}{RT}=\frac{(1)(0.4+0.2)}{(0.082)(293)}=0.025$$

Consider final state of system.  Let $P_F$ be the final equilibrium pressure, $n_1$ be the final number of moles in the larger bulb, and $n_2$ be the final number of moles in the smaller bulb:
$$n_1=\frac{(P_F)(0.4)}{(0.082)(373)}=0.0131P_F$$
$$n_2=\frac{(P_F)(0.2)}{(0.082)(273)}=0.0089P_F$$
$$n=n_1+n_2=0.022P_F=0.025$$
$$P_F=1.14\tag{atmospheres}$$