Calculate the final volume when $2$ moles of an ideal gas expand from $3 \ dm^3$ at constant external pressure $1.6 \ bar$ and the work done in the process is $800 \ J$. (in $dm^3$)

When $1 \ mole$ of gas is heated at constant volume,the temperature rises from $273 \ K$ to $546 \ K$. If heat supplied to the gas is $x \ J$,then find the correct statement from the following.

One mole of gas absorbs $200 \ J$ of heat at constant volume,then its temperature rises from $298 \ K$ to $308 \ K$. The change in internal energy will be $... \ J$.

At the $1$ bar pressure,the volume of a gas is $0.6 \ L$. If the gas receives $122 \ J$ of heat at $1$ bar pressure,the volume becomes $2 \ L$. Calculate the change in its internal energy. $(1 \ L \cdot bar = 101.32 \ J)$

The work done by a system is $8 \ J$,when $40 \ J$ heat is supplied to it. What is the increase in internal energy of the system in $J$?

For the reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$ at constant temperature and pressure,if $\Delta H$ and $\Delta U$ are the enthalpy and internal energy changes for the reaction,which of the following equations is correct?