Using this data,
2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10-3
NO2(g) == NO(g) + ½ O2(g) Kc = 3.93
calculate a value for Kc for the reaction,
NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g)
A. 20.2
B. 2.06 X 10-4
C. 4.49
D. 4.84 X 10-3
E. 0.223
equation 1--reverse it and take 1/2. Then Kc for the new rxn is 1/sqrt Kc = k1
equation 2--reverse it. Kc for new reaction is 1/Kc = k2.
Add the two new equations to obtain the desired equation.
Kc for the new equation is k1*k2.
To calculate the value of Kc for the reaction:
NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g)
We can use the equilibrium expressions and the given equilibrium constants for the two reactions.
First, we can write the equilibrium expression for the reaction:
Kc = [NO2] * [Cl2^(0.5)] / [NOCl] * [O2^(0.5)]
Now, let's substitute the equilibrium expressions for the individual reactions:
Kc = ([NO] * [O2^(0.5)] / [NOCl]^2) * ([NO2] / [NO])
We can simplify this expression further:
Kc = [(NO]^2 * [O2^(0.5)] / [NOCl]^2 * [NO])
Now we can substitute the values of the equilibrium constants, Kc1 and Kc2, for the individual reactions:
Kc = (3.93 / 1) * (3.20 * 10^-3 * 1) / (1)
Simplifying further:
Kc = 1.2576 * 10^-2
Therefore, the value of Kc for the given reaction is approximately 1.2576 * 10^-2.
The answer would be:
D. 4.84 X 10^-3
To calculate the value of Kc for the given reaction, we can use the principle of equilibrium and the equilibrium constants of the given reactions. The value of Kc for a reaction can be determined by multiplying the individual equilibrium constants of its constituent reactions.
The given reaction is:
NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g)
The equilibrium constants for the given reactions are:
1. 2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10^(-3)
2. NO2(g) == NO(g) + ½ O2(g) Kc = 3.93
We need to create the balanced equation for the given reaction by combining the two given reactions:
2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10^(-3) (Multiply this equation by 1/2 to balance the number of Cl atoms.)
NO2(g) == NO(g) + ½ O2(g) Kc = 3.93
Now, let's multiply these two equations to obtain the balanced equation for the given reaction:
(1/2) * (2 NO(g) + Cl2(g)) * (NO2(g) == NO(g) + ½ O2(g))
After simplifying, the balanced equation becomes:
NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g)
Now, we can determine the value of Kc for the given reaction by multiplying the equilibrium constants of the constituent reactions. Therefore:
Kc = Kc1 * Kc2
Kc = (3.20 X 10^(-3)) * (3.93)
Kc = 1.2576 X 10^(-2)
The value of Kc for the given reaction is 1.2576 X 10^(-2).
None of the given options match this value directly. However, option C (4.49) is the closest approximation to the calculated value.