Given the following equilibrium constants are given at 377°C,

1/2 N2(g) + 1/2 O2(g) NO(g) K1 = 110−17
1/2 N2(g) + O2(g) NO2(g) K2 = 110−11
N2(g) + 3/2 O2(g) N2O3(g) K3 = 210−33
N2(g) + 2 O2(g) N2O4(g) K4 = 410−17

determine the values for the equilibrium constants for the following reactions

Please help me, I am so confused

You didn't post the reaction.

NO(g) + NO2(g) N2O3(g)

N2O4(g) 2 NO2(g)

Sorry about that

To determine the equilibrium constants for the given reactions, we can use the concept of using reverse reactions and combining reactions.

1) Reverse Reaction:
The reverse reaction for the given reaction is obtained by reversing the direction of the equation and taking the reciprocal of the equilibrium constant.
For 1/2 N2(g) + 1/2 O2(g) ↔ NO(g), the reverse reaction is NO(g) ↔ 1/2 N2(g) + 1/2 O2(g).

Using K1 = 1.10−17, the equilibrium constant for the reverse reaction is:
K1_reverse = 1/K1 = 1/1.10−17

2) Combination of Reactions:
To determine the equilibrium constant for a combination of two or more reactions, we can multiply or divide the equilibrium constants of the individual reactions.

a) 2NO(g) ↔ N2(g) + O2(g):
This reaction can be obtained by multiplying the reverse reaction of the first reaction by two.
K_a = (K1_reverse)^2 = (1/1.10−17)^2

b) 2NO2(g) ↔ N2(g) + 2O2(g):
This reaction can be obtained by combining the reverse reaction of the second reaction with itself.
K_b = K2_reverse * K2_reverse = (1/1.10−11) * (1/1.10−11)

c) 2NO2(g) ↔ N2(g) + O2(g) + O2(g):
This reaction can be obtained by combining the reverse reaction of the second reaction with the first reaction.
K_c = K2_reverse * K1_reverse = (1/1.10−11) * (1/1.10−17)

d) NO2(g) + O2(g) ↔ N2(g) + 2O2(g):
This reaction can be obtained by combining the reverse reaction of the third reaction with itself.
K_d = K3_reverse * K3_reverse = (1/2.10−33) * (1/2.10−33)

e) NO2(g) + O2(g) + O2(g) ↔ N2(g) + 3O2(g):
This reaction can be obtained by combining the reverse reaction of the third reaction with the second reaction.
K_e = K3_reverse * K2_reverse = (1/2.10−33) * (1/1.10−11)

f) 2NO2(g) ↔ N2(g) + 3O2(g):
This reaction can be obtained by combining the reverse reaction of the third reaction with the first reaction.
K_f = K3_reverse * K1_reverse = (1/2.10−33) * (1/1.10−17)

g) NO2(g) + O2(g) ↔ N2(g) + 2O2(g) + O2(g):
This reaction can be obtained by combining the reverse reaction of the fourth reaction with itself.
K_g = K4_reverse * K4_reverse = (1/4.10−17) * (1/4.10−17)

Please note that the values of the equilibrium constants K_a, K_b, K_c, K_d, K_e, K_f, and K_g can be calculated by evaluating the corresponding expressions using the given values of the equilibrium constants K1, K2, K3, and K4.