for combustion of methane is –x kJ mol–1.
The value of for the same reaction would be:
The reaction of cyanamide, with dioxygen, was carried out in a bomb calorimeter, and ∆U was found to be at 298 K.
\(\small{\mathrm{NH}_2 \mathrm{CN}(\mathrm{s})+\frac{3}{2} \mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{N}_2(\mathrm{g})+\mathrm{CO}_2(\mathrm{g})+\mathrm{H}_2 \mathrm{O}(\mathrm{l})}\)
The enthalpy change for the reaction at 298 K would be:
The thermodynamic stability of NO(g) based on the above data is:
1. Less than NO2(g)
2. More than NO2(g)
3. Equal to NO2(g)
4. Insufficient data