The relationship between kp and kc is as follows:
kp = kc (RT)^∆n
∆n is the difference in number of moles in product side and the number of moles in reactant side.
∆n = 2-1 = 1
Kp= kc* (0.08206*298) = 4.61*10^-3*
= 0.1127
N2O4 | 2NO2 | |
Initial | 2.6 | 0 |
Change | -x | +2x |
Equilibrium | 2.6-x | 2x |
Kp = p(NO2)^2/p(N2O4) = (2x)^2/(2.6-x)
0.1127(2.6-x) = 4x^2
0.293 - 0.1127x = 4x^2
x = 0.2569
Equilibrium total pressure = 2.6-x + 2x = 2.6+x
= 2.6+0.2569 = 2.8569 atm
Answer: 2.8569 atm
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number 8 please
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