For the combustion of one mole of acetic acid,the work done at $298 \ K$ is (in $J$)

One mole of an ideal gas for which $C_v = (3/2)R$ is heated at a constant pressure of $1 \ atm$ from $25 \ ^oC$ to $100 \ ^oC$. The value of $\Delta H$ is $...... \ cal$.

$A$ thermodynamic cycle in the pressure $(p)-$ volume $(V)$ plane is given below. $A B$ and $C D$ are isothermal processes while $B C$ and $D A$ are adiabatic processes. The same cycle in the temperature $(T) -$ entropy $(S)$ plane is

The free energy change for the following reactions are given below:
$C_2H_{2(g)} + \frac{5}{2}O_{2(g)} \to 2CO_{2(g)} + H_2O_{(l)}; \Delta G^o = -1234 \ kJ$
$C_{(s)} + O_{2(g)} \to CO_{2(g)}; \Delta G^o = -394 \ kJ$
$H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(l)}; \Delta G^o = -237 \ kJ$
What is the standard free energy change for the reaction $H_{2(g)} + 2C_{(s)} \to C_2H_{2(g)}$ in $kJ$?

The heat of reaction for $C_2H_2 + H_2 \rightarrow C_2H_4$ is given by the following data:
$(i) \Delta H_f^o \text{ of } H_2O_{(\ell)} = -68.3 \ K \ cal \ mol^{-1}$
$(ii) \Delta H_{comb}^o \text{ of } C_2H_2 = -337.2 \ K \ cal \ mol^{-1}$
$(iii) \Delta H_{comb}^o \text{ of } C_2H_4 = -363.7 \ K \ cal \ mol^{-1}$

For the hypothetical reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$
$\Delta_r G^o$ and $\Delta_r S^o$ are $20 \ kJ/mol$ and $-20 \ J K^{-1} mol^{-1}$ respectively at $200 \ K$.
If $\Delta_r C_P$ is $20 \ J K^{-1} mol^{-1}$ then $\Delta_r H^o$ at $400 \ K$ is.....$kJ/mol$