For the reaction $C_3H_8(g) + 5O_2(g) \rightarrow 3CO_2(g) + 4H_2O(l)$,the value of $\Delta H - \Delta U$ is:

The work done to contract a gas in a cylinder is $462 \, J$. $128 \, J$ of energy is evolved in the process. What will be the internal energy change in the process? (in $J$)

Calculate the change in enthalpy in a chemical reaction when work done is $-800 \ J$ and increase in internal energy is $600 \ J$. (in $J$)

If $Q$ is the heat liberated from the system and $W$ is the work done on the system,then the first law of thermodynamics can be written as:

“The mass and energy both are conserved in an isolated system”,is the statement of

The enthalpy of vapour is $10 \ kcal/mole$ higher than liquid at $350 \ K$ and $2 \ atm$. Under given conditions,the difference in internal energy of vapour and liquid will be $...... \ cal$.