Match the following items in List-$I$ with their corresponding expressions in List-$II$.
List-$I$ List-$II$ $A$. At constant volume the change in internal energy of a system $I$. $W = -2.303 nRT \log \frac{V_f}{V_i}$ $B$. Isothermal irreversible change $II$. $W_{adiabatic} = \Delta U$ $C$. Isothermal reversible change $III$. $q_V = \Delta U$ $D$. Adiabatic change $IV$. $W = -p_{ex} (V_f - V_i)$ $V$. $\Delta U = \Delta H - \Delta nRT$
| List-$I$ | List-$II$ |
| $A$. At constant volume the change in internal energy of a system | $I$. $W = -2.303 nRT \log \frac{V_f}{V_i}$ |
| $B$. Isothermal irreversible change | $II$. $W_{adiabatic} = \Delta U$ |
| $C$. Isothermal reversible change | $III$. $q_V = \Delta U$ |
| $D$. Adiabatic change | $IV$. $W = -p_{ex} (V_f - V_i)$ |
| $V$. $\Delta U = \Delta H - \Delta nRT$ |
- A$A-III, B-IV, C-I, D-II$
- B$A-IV, B-I, C-III, D-V$
- C$A-III, B-IV, C-I, D-V$
- D$A-III, B-V, C-I, D-II$
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Similar Questions
One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\,^oC$. If the work done during the process is $3\,kJ$,the final temperature will be equal to $(C_v = 20\,J\,K^{-1} \, mol^{-1})$
MediumAIIMS 2001
View SolutionThe free energy change for the following reactions are given below:
$C_2H_{2(g)} + \frac{5}{2}O_{2(g)} \to 2CO_{2(g)} + H_2O_{(l)}; \Delta G^o = -1234 \ kJ$
$C_{(s)} + O_{2(g)} \to CO_{2(g)}; \Delta G^o = -394 \ kJ$
$H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(l)}; \Delta G^o = -237 \ kJ$
What is the standard free energy change for the reaction $H_{2(g)} + 2C_{(s)} \to C_2H_{2(g)}$ in $kJ$?
$C_2H_{2(g)} + \frac{5}{2}O_{2(g)} \to 2CO_{2(g)} + H_2O_{(l)}; \Delta G^o = -1234 \ kJ$
$C_{(s)} + O_{2(g)} \to CO_{2(g)}; \Delta G^o = -394 \ kJ$
$H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(l)}; \Delta G^o = -237 \ kJ$
What is the standard free energy change for the reaction $H_{2(g)} + 2C_{(s)} \to C_2H_{2(g)}$ in $kJ$?
Medium
View SolutionMatch the following:
List-$I$ List-$II$ $(A) \Delta U = W_{ad}$ $I.$ Isothermal reversible expansion $(B) \Delta U = q - W$ $II.$ Wall is adiabatic $(C) \Delta U = -q$ $III.$ Thermally conducting walls $(D) \Delta U = 0$ $IV.$ Isolated system $V.$ Closed system
The correct answer is
| List-$I$ | List-$II$ |
|---|---|
| $(A) \Delta U = W_{ad}$ | $I.$ Isothermal reversible expansion |
| $(B) \Delta U = q - W$ | $II.$ Wall is adiabatic |
| $(C) \Delta U = -q$ | $III.$ Thermally conducting walls |
| $(D) \Delta U = 0$ | $IV.$ Isolated system |
| $V.$ Closed system |
The correct answer is
Calculate $\Delta H^{\circ}$ for the reaction, $Na_2O_{(s)} + SO_{3(g)} \longrightarrow Na_2SO_{4(s)}$, given the following reactions:
$(A) \ Na_{(s)} + H_2O_{(l)} \longrightarrow NaOH_{(s)} + \frac{1}{2}H_{2(g)} \quad \Delta H^{\circ} = -146 \ kJ$
$(B) \ Na_2SO_{4(s)} + H_2O_{(l)} \longrightarrow 2NaOH_{(s)} + SO_{3(g)} \quad \Delta H^{\circ} = +418 \ kJ$
$(C) \ 2Na_2O_{(s)} + 2H_{2(g)} \longrightarrow 4Na_{(s)} + 2H_2O_{(l)} \quad \Delta H^{\circ} = +259 \ kJ$
$(A) \ Na_{(s)} + H_2O_{(l)} \longrightarrow NaOH_{(s)} + \frac{1}{2}H_{2(g)} \quad \Delta H^{\circ} = -146 \ kJ$
$(B) \ Na_2SO_{4(s)} + H_2O_{(l)} \longrightarrow 2NaOH_{(s)} + SO_{3(g)} \quad \Delta H^{\circ} = +418 \ kJ$
$(C) \ 2Na_2O_{(s)} + 2H_{2(g)} \longrightarrow 4Na_{(s)} + 2H_2O_{(l)} \quad \Delta H^{\circ} = +259 \ kJ$
DifficultAP EAMCET 2009
View SolutionWhich of the following equations are correct?
$(A)$ $H = U + PV$
$(B)$ $G = H - TS$
$(C)$ $U = q + W$
$(A)$ $H = U + PV$
$(B)$ $G = H - TS$
$(C)$ $U = q + W$
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