How much heat in $KJ$ is released during the combustion of $112 \ L$ of water gas at $S.T.P.$? (Water gas is an equimolar mixture of $H_2$ and $CO$)
$H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_2O_{(g)}; \Delta H = -241.8 \ KJ$
$CO_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{2(g)}; \Delta H = -283 \ KJ$
$H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_2O_{(g)}; \Delta H = -241.8 \ KJ$
$CO_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{2(g)}; \Delta H = -283 \ KJ$
- A$241.8$
- B$283$
- C$1312$
- D$1586$
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Similar Questions
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:
Calculate the enthalpy change when $6 \text{ g}$ of $CO(g)$ reacts with sufficient $NO_2(g)$ according to the following reaction: $4 \text{ CO}(g) + 2 \text{ NO}_2(g) \rightarrow 4 \text{ CO}_2(g) + 2 \text{ N}_2(g)$; $\Delta_r H^0 = -1200 \text{ kJ}$ (in $\text{ kJ}$)
DifficultMHT CET 2026
View SolutionThe enthalpies of combustion of carbon and carbon monoxide are $-393.5 \, kJ \, mol^{-1}$ and $-283 \, kJ \, mol^{-1}$ respectively. The enthalpy of formation of carbon monoxide per mole is $....... \, kJ \, mol^{-1}$. (in $.5$)
MediumAIEEE 2004
View Solution$3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$
For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?
For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?
Medium
View SolutionFor an isothermal expansion of $2 \, \text{mol}$ of a gas at $298 \, K$ from $5 \, dm^3$ to $40 \, dm^3$ under constant external pressure,the work done $(W)$ and the reversible work $(W_{rev})$ are,respectively:
Difficult
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