An ideal gas expands by performing $200 \ J$ of work,during this internal energy increases by $432 \ J$. What is the enthalpy change (in $J$)?

Which of the following is the correct expression of the first law of thermodynamics for adiabatic processes?

For an isothermal reversible expansion process,the value of $q$ can be calculated by the expression

The volume of an ideal gas contracts from $10.0 \ L$ to $2.0 \ L$ under an applied pressure of $2.0 \ atm$. During contraction,the system also evolved $900 \ J$ of heat. The change in internal energy (in $J$) involved in the system is $(1 \ L \ atm = 101.3 \ J)$:

Which of the following relations is correct for the reaction $S(s) + O_2(g) \rightarrow SO_2(g)$?

An ideal gas,$\overline{C}_{V} = \frac{5}{2} R$,is expanded adiabatically against a constant pressure of $1 \ atm$ until it doubles in volume. If the initial temperature and pressure are $298 \ K$ and $5 \ atm$,respectively,then the final temperature is . . . . . . $K$ (nearest integer). [$\overline{C}_{V}$ is the molar heat capacity at constant volume]