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 $kJ$)

$4 \ g$ of $NH_4NO_3$ were dissolved in $196 \ g$ of water at constant pressure in a calorimeter with a heat capacity of $160 \ J \ K^{-1}$. The temperature fell by $1.3 \ K$. The specific heat of the solution is $4.2 \ J \ K^{-1} \ g^{-1}$. The enthalpy of solution of $NH_4NO_3$ is $......$ $kJ \ mol^{-1}$.

For the process $H_2O_{(l)} (1 \ bar, 373 \ K) \rightarrow H_2O_{(g)} (1 \ bar, 373 \ K)$,the correct set of thermodynamic parameters is:

For a spontaneous process, the correct statement$(s)$ is (are):

The internal energy change (in $J$) when $90 \ g$ of water undergoes complete evaporation at $100^{\circ} C$ is........
(Given: $\Delta H_{vap}$ for water at $373 \ K = 41 \ kJ/mol$,$R = 8.314 \ J \ K^{-1} mol^{-1}$)

The standard enthalpies of formation of $1,3-butadiene(g)$,$CO_{2(g)}$,and $H_2O_{(l)}$ at $298 \ K$ are $-30$,$-94$,and $-68 \ kcal/mol$ respectively. If the magnitude of resonance enthalpies of $1,3-butadiene$ and $CO_2$ are $10$ and $20 \ kcal/mol$ respectively,the enthalpy of combustion of $1,3-butadiene(g)$ at $298 \ K$ is $........ \ kcal/mol$. (Enthalpy of vaporization of $H_2O_{(l)}$ at $298 \ K = 10 \ kcal/mol$)