Consider the reaction:
1/2 N2(g) +
O2(g)<<<----->>>NO2(g)
Write the equilibrium constant for this reaction in terms of the
equilibrium constants, Ka and
Kb, for reactions a
and bbelow:
| a.) | N2O4(g) | <-------> | 2NO2(g) | Ka | |
| b.) | N2(g) + 2 O2(g) | <------> | N2O4(g) | Kb |
| K = |
N2O4(g) <-------> 2NO2(g) Ka = [NO2]^2/[N2O4]
N2(g) + 2 O2(g) <-----> N2O4(g) Kb = [N2O4]/[N2][O2]^2
-----------------------------------------------------
N2(g) + 2 O2(g)<<<----->>> 2NO2(g) K1 = [NO2]^2/[N2][O2]^
--------------------------------------------------------------
SO that,
K1 = Ka*Kb
for 1/2 X ( N2(g) + 2O2(g)<<<----->>> 2NO2(g) )
K = (Ka*Kb)^1/2
Get Answers For Free
Most questions answered within 1 hours.