Two mole of an ideal gas is expanded isothermally and reversibly from $1 \ L$ to $10 \ L$ at $300 \ K$. The enthalpy change (in $kJ$) for the process is .....$kJ$

What is the constant external pressure of an ideal gas when expanded from $2 \times 10^{-2} \ m^3$ to $3 \times 10^{-2} \ m^3$,if the work done by the gas is $-5.09 \ kJ$?

Identify the state functions and path functions out of the following: enthalpy,entropy,heat,temperature,work,free energy.

$6$ moles of an ideal gas expand isothermally and reversibly from a volume of $1 \ L$ to a volume of $10 \ L$ at $27 \ ^oC$. What is the maximum work done? (in $kJ$)

For the reaction of nitrogen with hydrogen to form ammonia,$\Delta H^o = -92.2 \ kJ/mol$. If the reaction is carried out at a constant pressure of $20.0 \ atm$ and a volume change of $-1.16 \ L$,calculate the change in internal energy $(\Delta U)$ in $kJ$.

In an endothermic reaction,the value of $\Delta H$ is