The enthalpy of combustion of carbon monoxide at $17 ^\circ C$ and constant volume is $-283.3 \ kJ$. Calculate the enthalpy of combustion at constant pressure in $kJ$.

Enthalpy of combustion of $CH_4, C_2H_6$ and $C_3H_8$ are $-210.8, -368.4$ and $-526.2 \ k \ cal \ mol^{-1}$ respectively. Enthalpy of combustion of hexane can be predicted as........$k \ cal \ mol^{-1}$

Enthalpy of sublimation of iodine is $24 \ cal \ g^{-1}$ at $200 \ ^oC$. If specific heat of $I_{2(s)}$ and $I_{2(vap)}$ are $0.055$ and $0.031 \ cal \ g^{-1} K^{-1}$ respectively,then enthalpy of sublimation of iodine at $250 \ ^oC$ in $cal \ g^{-1}$ is

The $C_p$ of an ideal gas is $10.314 \ J \ mol^{-1} \ K^{-1}$. One mole of this gas is expanded against a constant pressure of $p \ atm$. The change in temperature during expansion is $1.0 \ K$. The values of $q$ (in $J$) and $\Delta H$ (in $J \ mol^{-1}$) are respectively

What is the value of $\Delta S_{\text{total}}$ for the following reaction at $300 \ K$:
$Fe_{2}O_{3(s)} + 3CO_{(g)} \longrightarrow 2Fe_{(s)} + 3CO_{2(g)}$
$\Delta H^{\circ} = -25 \ kJ, \Delta S^{\circ} = 15 \ J \ K^{-1}$ (in $J \ K^{-1}$)

The enthalpy of formation of $H_2O$ is $-68 \ k.cal/mol$. Calculate the enthalpy of formation of $OH^-$. Given that the enthalpy of neutralization of $H^+$ and $OH^-$ is $-13.7 \ k.cal/mol$.