When $200 \ cm^3$ of $0.1 \ M \ H_2SO_4$ is mixed with $150 \ cm^3$ of $0.2 \ M \ KOH$,the heat produced is ..... $kJ$.

Calculate the difference between heat of combustion of carbon monoxide gas at constant pressure and at constant volume at $27^{\circ} C$ (in $cal$)? $(R = 2 \ cal \ K^{-1} \ mol^{-1})$

Benzene burns according to the following equation at $300 \ K$ $(R = 8.314 \ J \ mol^{-1} K^{-1})$: $2 C_6H_{6(l)} + 15 O_{2(g)} \to 12 CO_{2(g)} + 6 H_2O_{(l)}$,$\Delta H^o = -6542 \ kJ/mol$. What is the $\Delta E^o$ for the combustion of $1.5 \ mol$ of benzene in $kJ$?

If $100$ mole of $H_2O_2$ decomposes at $1$ bar and $300$ $K$,the work done $(kJ)$ by $50$ mole of $O_{2(g)}$ as it expands against $1$ bar pressure is............. $kJ$
$2H_2O_{2(l)} \rightleftharpoons 2H_2O_{(l)} + O_{2(g)}$
$(R = 8.3 \ J \ K^{-1} \ mol^{-1})$

For the reaction $2Cl_{(g)} \rightarrow Cl_{2(g)}$,the signs of $\Delta H$ and $\Delta S$ are respectively:

$A$ gas expands from $3 \ dm^{3}$ to $5 \ dm^{3}$ against a constant pressure of $3 \ atm$. The work done during this expansion is used to heat $10 \ mol$ of water at $290 \ K$. What will be the final temperature of the water in $K$? (Specific heat of water = $4.184 \ J \ g^{-1} \ K^{-1}$)