The heat of neutralization of a strong acid and a strong alkali is $-57.0 \ kJ \ mol^{-1}$. The heat released when $0.5 \ mole$ of $HNO_3$ solution is mixed with $0.2 \ mole$ of $KOH$ is ....$kJ$

One mole of Argon is heated using $PV^{5/2} = \text{constant}$. By what amount is heat absorbed during the process,when the temperature changes by $\Delta T = 26 \ K$ (in $J$)? (Take $R = 8.314 \ J \ mol^{-1} K^{-1}$)

Assertion $(A)$: If heat of combustion of $C_2H_6$ is $X \ kJ \ mol^{-1}$,heat liberated on combustion of $150 \ g$ of $C_2H_6$ is $5X \ kJ$.
Reason $(R)$: Enthalpy is an extensive property.

At constant volume,$5 \, mol$ of a gas shows an increase in temperature by $3.5 \, K$ upon providing $437.5 \, J$ of heat. What will be the molar heat capacity for the gas at constant pressure in $J \, K^{-1} \, mol^{-1}$?

One mole of an ideal monoatomic gas undergoes two reversible processes ($A \rightarrow B$ and $B \rightarrow C$) as shown in the given figure:
$A \rightarrow B$ is an adiabatic process. If the total heat absorbed in the entire process ($A \rightarrow B$ and $B \rightarrow C$) is $R T_2 \ln 10$,the value of $2 \log V_3$ is . . . . . [Use,molar heat capacity of the gas at constant pressure,$C_{p, m} = \frac{5}{2} R$ ]

Consider the following reaction:
$C_6H_{6(l)} + \frac{15}{2} O_{2(g)} \to 6 CO_{2(g)} + 3 H_2O_{(g)}$
What are the signs of $\Delta H$,$\Delta S$,and $\Delta G$ for the above reaction?