The enthalpy of combustion of methane, graphite, and dihydrogen at 298 K are, –890.3 kJ mol1 , –393.5 kJ mol–1, and –285.8 kJ mol–1 respectively. The enthalpy of formation of CH4(g) is-

1. –74.8 kJ mol–1 2. –52.27 kJ mol–1
3. +74.8 kJ mol–1 4. +52.26 kJ mol–1
Subtopic:  Thermochemistry |
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The enthalpy of combustion of carbon to CO2 is –393.5 kJ mol-1. The amount of heat released upon formation of 35.2 g of CO2 from carbon and dioxygen gas would be:

1. –393.5 kJ mol–1 2. –314.8 kJ mol–1
3. +314.8 kJ mol–1 4. –320.5 kJ mol–1
Subtopic:  Thermochemistry |
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The enthalpy of formation of COg, CO2g, N2Og , and N2O4g are–110 kJ mol-1, – 393 kJ mol-1, 81 kJ mol-1, and 9.7 kJ \(\text{mol}^{- 1}\) respectively.

The value of \(\left(\Delta\right)_{r} H\) for the reaction would be:

\(\mathrm{N_{2} O_{4 \left(g\right)} + 3 \left(CO\right)_{\left(g\right)} \rightarrow N_{2} O_{\left(g\right)} + 3 \left(CO\right)_{2 \left(g\right)}}\)

1. \(- 777 . 7\) \(kJ\) \(\text{mol}^{- 1}\) 2. \(\) \(+ 777 . 7\) \(kJ\) \(\text{mol}^{- 1}\)
3. \(\) \(+ 824 . 9\) \(kJ\) \(\text{mol}^{- 1}\) 4. \(-\) \(345 . 4\) \(kJ\) \(\text{mol}^{- 1}\)
Subtopic:  Thermochemistry |
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 N2 + 3 H2  2NH3 ; rH° = -92.4 kJ mol-1. The standard enthalpy of formation of NH3 gas in the above reaction would be:

1. -92.4 J (mol)-1 2. -46.2 kJ (mol)-1
3. +46.2 J (mol)-1 4. +92.4 kJ (mol)-1
Subtopic:  Thermochemistry |
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The standard enthalpy of the formation of CH3OH(l) from the following data is:

\(\small{\mathrm{CH}_3 \mathrm{OH}_{(l)}+\frac{3}{2} \mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{CO}_2(\mathrm{g})+2 \mathrm{H}_2 \mathrm{O}_{(l)} \text {; }}\)
\( \Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-726 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}\)
\(\small{\mathrm{C}(\mathrm{s})+\mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{CO}_2(\mathrm{g}) \text {; } }\)
\(\Delta_{\mathrm{c}} \mathrm{H}^{\circ}=-393 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}\)
\(\small{\mathrm{H}_{2(\mathrm{g})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{g})} \rightarrow \mathrm{H}_2 \mathrm{O}_{(l)} \text {; } } \)
\(\Delta_{\mathrm{f}} \mathrm{H}^{\circ}=-286 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
 
1. −239 kJ mol−1 2. +239 kJ mol−1
3. −47 kJ mol−1 4. +47 kJ mol−1
Subtopic:  Thermochemistry |
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vapH° (CCl4) = 30.5 kJ mol-1
fH° (CCl4) = - 135.5 kJ mol-1
aH° (C) = 715.0 kJ mol-1
aH° (Cl2)= 242 kJ mol-1

The enthalpy change for the reaction

 CCl4 (g)  C(g) + 4Cl (g) would be:

1. 326 kJ mol-1 2. 1304 kJ mol-1
3. -328 kJ mol-1 4. -1304 kJ mol-1
Subtopic:  Thermochemistry |
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