Given Kc values:
N2(g)+1/2 O2(g)<->N2O(g) Kc=2.7* 10^-18
N2O4(g)<->2NO2(g)
Kc=4.6*10^-3
1/2N2(g)+O2(g)<->NO2(g)
kc=4.1*10^-9
What is the Kc value for:
2N2O(g)+3O2(g)<->2N2O4(g)
The answer is wrong.
Kc (Equilibrium Constant) is always <1.
The answer may be wrong due to a math error I might have made, but Kc can certainly be greater than 1.
This is essentially an algebra problem. Using the concentration ratios you have been given, calculate the Kc for the indicated reaction.
To find the Kc value for the reaction: 2N2O(g) + 3O2(g) <-> 2N2O4(g), you can use the concept of combining reactions and their associated Kc values.
Step 1: Combine the given reactions
By examining the given reactions, you can notice that two of them involve N2O and NO2. To achieve the desired reaction, you can combine the first and second reactions:
N2(g) + 1/2 O2(g) <-> N2O(g) Kc = 2.7 * 10^(-18) (Reaction 1)
N2O(g) <-> 2NO2(g)
Kc = 4.6 * 10^(-3) (Reaction 2)
Step 2: Determine the desired reaction
Now, you need to use the given reactions to deduce the desired reaction:
2N2O(g) + 3O2(g) <-> 2N2O4(g)
To achieve this, you can multiply Reaction 1 by 2 and Reaction 2 by 2:
2[N2(g) + 1/2 O2(g) <-> N2O(g)] (Reaction 1) x 2
2[N2O(g) <-> 2NO2(g)] (Reaction 2) x 2
Step 3: Multiply the Kc values
To obtain the overall Kc value for the desired reaction, multiply the Kc values determined in Step 2:
Kc(desired) = Kc(Reaction 1)^(coefficient in desired reaction) x Kc(Reaction 2)^(coefficient in desired reaction)
Kc(desired) = [2.7 * 10^(-18)]^2 x [4.6 * 10^(-3)]^2
Simplifying the expression will give you the final Kc value for the reaction 2N2O(g) + 3O2(g) <-> 2N2O4(g).
[NO2]^2/[N2O4] = 4.6*10^-3
[N2O4]/[NO2]^2 = 217.4
[N2O4]^2 = 4.73*10^4 [NO2]^4
= 4.73*10^4 *[N2]^2[O2]^4
Now use the fact that
[N2O]^2 = [N2]^2*[O2]*7.29*10^-36
[N2]^2*[O2] = 1.37*10^35 [N2O]^2
[N2O4]^2 = 4.73*10^4*1.37*10^35 [N2O]^2*[O2]^3
= 6.49*10^39 [N2O]^2*[O2]^3
Kc = 6.49*10^39
check my math