Consider the equilibrium:
2NOBr (g) <=> 2NO (g) + Br2 (g)
If nitroxyl bromide (NOBr) is 34% dissociated at 25oC and the total pressure at equilibrium is 0.25 atm, calculate Kp for the dissociation at this temperature. Report your answer with two significant figures.
I tried taking 66% of the .25 atm = .165 and then splitting the remaining pressure up 3 ways, 2/3 to the NO and 1/3 to the Br2.
This wasn't correct. I'm not sure what to do, help please?
2NOBr (g) <=> 2NO (g) + Br2 (g)
If nitroxyl bromide (NOBr) is 34% dissociated at 25oC and the total pressure at equilibrium is 0.25 atm, calculate Kp for the dissociation at this temperature. Report your answer with two significant figures.
I tried taking 66% of the .25 atm = .165 and then splitting the remaining pressure up 3 ways, 2/3 to the NO and 1/3 to the Br2.
This wasn't correct. I'm not sure what to do, help please?