Total enthalpy change for freezing of $1 \ mol$ of water at $10^{\circ} C$ to ice at $-10^{\circ} C$ is $..........$ (Given : $\Delta_{fus} H = x \ kJ / mol$,$C_{p}[H_2O_{(l)}] = y \ J \ mol^{-1} \ K^{-1}$,$C_{p}[H_2O_{(s)}] = z \ J \ mol^{-1} \ K^{-1}$)
- A$-x - 10y - 10z$
- B$-10(100x + y + z)$
- C$10(100x + y + z)$
- D$x - 10y - 10z$
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An electric heater of power $600 \, W$ takes $8 \, \text{minutes}$ to evaporate $80 \, mL$ of water. The enthalpy of vaporization of water is ......... $kJ \, mol^{-1}$.
Difficult
View SolutionAt the temperature $T$ $(K)$ for the reaction: $X_2O_{4(l)} \rightarrow 2XO_{2(g)}$,given $\Delta U = x \ kJ \ mol^{-1}$ and $\Delta S = y \ J \ K^{-1} \ mol^{-1}$. The Gibbs energy change for the reaction is: (Assume $X_2O_4$ and $XO_2$ are ideal gases)
Match the following:
$A$. Isothermal process $i$. $q = \Delta U$ $B$. Adiabatic process $ii$. $W = - P \times \Delta V$ $C$. Isobaric process $iii$. $W = \Delta U$ $D$. Isochoric process $iv$. $W = - nRT \ln \left(\frac{v_f}{v_i}\right)$
| $A$. Isothermal process | $i$. $q = \Delta U$ |
| $B$. Adiabatic process | $ii$. $W = - P \times \Delta V$ |
| $C$. Isobaric process | $iii$. $W = \Delta U$ |
| $D$. Isochoric process | $iv$. $W = - nRT \ln \left(\frac{v_f}{v_i}\right)$ |
Heat of combustion of $CH_4, C_2H_4$ and $C_2H_6$ are $-890, -1411$ and $-1560 \ kJ/mol$ respectively. Which has the lowest calorific value?
Medium
View SolutionOne mole of an ideal gas for which $C_v = (3/2)R$ is heated at a constant pressure of $1 \ atm$ from $25 \ ^oC$ to $100 \ ^oC$. The value of $\Delta H$ is $...... \ cal$.
Difficult
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