Can anyone help with this electrochemistry question? The standard free energy of
ID: 860687 • Letter: C
Question
Can anyone help with this electrochemistry question?
The standard free energy of formation of nitric oxide, NO at 1000K is 78kJ/mol, calculate the equilibrium constant for this reaction at 1000K, N2(g) + O2(g) <--> 2NO(g)
Can anyone help with this electrochemistry question? I know we need to use delta G degree=-RT1nK and rearrange. but the question has the tempurature at 1000K so there's another step that needs to be done before or perhaps after plugging it into the formula. The answers posted to this question on this site from others were all incorrect answers so I'm a bit lost. Hopefully you can help. The standard free energy of formation of nitric oxide, NO at 1000K is 78kJ/mol, calculate the equilibrium constant for this reaction at 1000K, N2(g) + O2(g) 2NO(g)Explanation / Answer
Delta G = (78KJ)(2moles)(1000) = 156000J
K = e^-(156000*8.314*1000K)
K = 7.09*10^-9