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........$k \ cal \ mol^{-1}$

Find the heat required to convert $10 \ g$ of ice at $0.0^{\circ} C$ into water at $30^{\circ} C$. (Enthalpy of fusion of ice $= 333.5 \ J \ g^{-1}$,$C_p$ of water $= 4.18 \ J \ g^{-1} \ K^{-1}$) (in $kJ$)

The difference between enthalpy change and internal energy change for the combustion of one mole of ethyl alcohol is

The heat associated with the combustion of liquid benzene at constant volume is $-3268 \ kJ \ mol^{-1}$. Calculate the change in enthalpy when this reaction occurs at $300 \ K$ $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$.

Chloroform has $\Delta H_{vaporization} = 29.2 \ kJ/mol$ and boils at $61.2 \ ^oC$. What is the value of $\Delta S_{vaporization}$ for chloroform? $...... \ J/mol \ K$

The heat evolved in the combustion of methane is given by the following equation: $CH_{4(g)} + 2O_{2(g)} \to CO_{2(g)} + 2H_2O_{(l)}$; $\Delta H = -890.3 \ kJ$. How many grams of methane would be required to produce $445.15 \ kJ$ of heat of combustion?