calculate delta H for reaction: CH4 (g) + 2O2 (g) ---> CO2 (g) + 2H2O (l) given: CH4 + O2 ---> CH2O + H2O. delta H = -276 kJ CH2O2 + O2 ---> CO2 + H2O delta H = -530 kJ H2O (l) ---> H2O (g). delta H = 55 kJ
Added by Chad G.
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What is the estimated ΔH in kJ for the reaction, using the given information? CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) C-H = 413 kJ O=O = 495 kJ C=O = 799 kJ H-O = 463 kJ
Madhur L.
Determine the enthalpy of the reaction: 2CH4 → 2H2 + C2H4 Given: CH4 + 2O2 → CO2 + 2H2O ΔH = -891 kJ C2H4 + 3O2 → 2CO2 + 2H2O ΔH = -1411 kJ 2H2 + O2 → 2H2O ΔH = -571 kJ
Shaiju T.
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction is the conversion of methane to ethane: $$ 2 \mathrm{CH}_{4}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{H}_{2}(g) $$ Calculate the $\Delta H^{\circ}$ for this reaction using the following thermochemical data: $$ \begin{aligned} \mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) & \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) & \Delta H^{\circ} &=-890.3 \mathrm{~kJ} \\ 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l) & \Delta H^{\circ} &=-571.6 \mathrm{~kJ} \\ 2 \mathrm{C}_{2} \mathrm{H}_{6}(g)+7 \mathrm{O}_{2}(g) & \longrightarrow 4 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) & \Delta H^{\circ} &=-3120.8 \mathrm{~kJ} \end{aligned} $$
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