Match List-$I$ with List-$II$
List-$I$ List-$II$ $A$. Spontaneous process $I$. $\Delta H < 0$ $B$. Process with $\Delta P = 0; \Delta T = 0$ $II$. $\Delta G_{T, P} < 0$ $C$. $\Delta H_{reaction}$ $III$. Isothermal and isobaric process $D$. Exothermic process $IV$. [Bond energies of molecules in reactants] - [Bond energies of product molecules]
Choose the correct answer from the options given below:
| List-$I$ | List-$II$ |
| $A$. Spontaneous process | $I$. $\Delta H < 0$ |
| $B$. Process with $\Delta P = 0; \Delta T = 0$ | $II$. $\Delta G_{T, P} < 0$ |
| $C$. $\Delta H_{reaction}$ | $III$. Isothermal and isobaric process |
| $D$. Exothermic process | $IV$. [Bond energies of molecules in reactants] - [Bond energies of product molecules] |
Choose the correct answer from the options given below:
- A$A-III, B-II, C-IV, D-I$
- B$A-II, B-III, C-IV, D-I$
- C$A-II, B-III, C-I, D-IV$
- D$A-II, B-I, C-III, D-IV$
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For a diatomic ideal gas in a closed system,which of the following plots does not correctly describe the relation between various thermodynamic quantities?
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View SolutionThe reaction of cyanamide,$NH_2CN_{(s)}$,with dioxygen was carried out in a bomb calorimeter,and $\Delta U$ was found to be $-742.7 \ kJ \ mol^{-1}$ at $298 \ K$. Calculate the enthalpy change for the reaction at $298 \ K$.
$NH_2CN_{(s)} + \frac{3}{2}O_{2_{(g)}} \to N_{2_{(g)}} + CO_{2_{(g)}} + H_2O_{(l)}$
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View SolutionThe reaction of cyanamide,$NH_{2}CN_{(s)}$ with oxygen was run in a bomb calorimeter and $\Delta U$ was found to be $-742.24 \ kJ \ mol^{-1}$. The magnitude of $\Delta H_{298}$ for the reaction
$NH_{2}CN_{(s)} + \frac{3}{2} O_{2(g)} \rightarrow N_{2(g)} + CO_{2(g)} + H_{2}O_{(l)}$
is $............ \ kJ$. (Rounded off to the nearest integer)
[Assume ideal gases and $R = 8.314 \ J \ mol^{-1} K^{-1}$]
$NH_{2}CN_{(s)} + \frac{3}{2} O_{2(g)} \rightarrow N_{2(g)} + CO_{2(g)} + H_{2}O_{(l)}$
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View SolutionCalculate $\Delta H^{\circ}$ for the reaction, $Na_2O_{(s)} + SO_{3(g)} \longrightarrow Na_2SO_{4(s)}$, given the following reactions:
$(A) \ Na_{(s)} + H_2O_{(l)} \longrightarrow NaOH_{(s)} + \frac{1}{2}H_{2(g)} \quad \Delta H^{\circ} = -146 \ kJ$
$(B) \ Na_2SO_{4(s)} + H_2O_{(l)} \longrightarrow 2NaOH_{(s)} + SO_{3(g)} \quad \Delta H^{\circ} = +418 \ kJ$
$(C) \ 2Na_2O_{(s)} + 2H_{2(g)} \longrightarrow 4Na_{(s)} + 2H_2O_{(l)} \quad \Delta H^{\circ} = +259 \ kJ$
$(A) \ Na_{(s)} + H_2O_{(l)} \longrightarrow NaOH_{(s)} + \frac{1}{2}H_{2(g)} \quad \Delta H^{\circ} = -146 \ kJ$
$(B) \ Na_2SO_{4(s)} + H_2O_{(l)} \longrightarrow 2NaOH_{(s)} + SO_{3(g)} \quad \Delta H^{\circ} = +418 \ kJ$
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