Show the equation you used. I don't know the one you used.
Show the work you did.
I'll find the error.
Help me set up this problem. I have been looking at a few examples of similar problems and I keep getting the wrong answers. I'm getting really confused.
Q: The standard free energy change ΔG∘ and the equilibrium constant K for a reaction can be related by the following equation:
ΔG∘=−RTlnK
where T is the Kelvin temperature and R is equal to 8.314J/(mol⋅K).
a. Calculate the equilibrium constant for the reaction forming nitric oxide at room temperature, 25 ∘C.
Express your answer numerically.
A: What I got was 1.93*10^-71, which is wrong. I can't figure out where I went wrong.
2 answers
The standard free energy change, ΔG∘, and the equilibrium constant K for a reaction can be related by the following equation:
ΔG∘=−RTlnK
where T is the Kelvin temperature and R is equal to 8.314 J/(mol⋅K).
Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C:
N2(g)+O2(g)→2NO(g)
I'm also having trouble with this question, my incorrect answer is 1.94x10^-31
ΔH= 182.6 kJ/mol
ΔS= 2.48x10^-2 kJ/mol*K
ΔG= 1.73x10^2 kJ/mol*K
The equation I thought I was suppose to use is this one.
K = e^(-ΔG/RT)
Thanks in advance for your help. :)
ΔG∘=−RTlnK
where T is the Kelvin temperature and R is equal to 8.314 J/(mol⋅K).
Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C:
N2(g)+O2(g)→2NO(g)
I'm also having trouble with this question, my incorrect answer is 1.94x10^-31
ΔH= 182.6 kJ/mol
ΔS= 2.48x10^-2 kJ/mol*K
ΔG= 1.73x10^2 kJ/mol*K
The equation I thought I was suppose to use is this one.
K = e^(-ΔG/RT)
Thanks in advance for your help. :)
2 answers