For given problem first we need to add up the two reaction.
2 CO2 (g) + H2O (g) 2 O2 (g) + CH2CO (g) Kc = 6.1 * 108
+ CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g) Kc = 1.2 * 1014
Cancelling 2 O2 (g) and subtracting H2O (g) and CO2 (g) from both side, we get
CH4 (g) + CO2 (g) CH2CO (g) + H2O (g).
To find the Kc for combined reaction we need to multiply both the value.
Therefore Kc = 6.1 * 108 * 1.2 * 1014 = 7.32 * 1022.
After rounding off final answer will be 7.3 * 1022.
Therefore Kc for reaction CH4 (g) + CO2 (g) CH2CO (g) + H2O (g) is 7.3 * 1022.
If you find any mistake please mention in the comment box.
Thanks.
Given the following equilibrium equations and their corresponding equilibrium constants: 2CO2 (g)+H2O(g)⇌2O2 (g)+CH2CO(g) Kc=6.1x108 CH4(g)+2O2(g)⇌CO2 (g)+2H2O(g)...
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Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g).
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