0.500 moles of NOCl is placed in a 1.00L vessel at 700K,and after the system comes to equilibrium,the concentration of the NOCl is .440M. Calculate the value of Kc for the reaction @NOCl(g)->2NO(g)+Cl2(g)?
To calculate the value of Kc, we need to use the equation for the equilibrium constant:
Kc = [NO]^2[Cl2] / [NOCl]
First, we need to determine the equilibrium concentrations of each species.
Given:
Initial moles of NOCl = 0.500 moles
Initial volume = 1.00 L
Equilibrium concentration of NOCl = 0.440 M
Since we are given the volume and the equilibrium concentration of NOCl, we can calculate the molar concentration of NOCl by using the formula:
Molarity (M) = moles / volume
Concentration of NOCl = 0.500 moles / 1.00 L = 0.500 M
Now we can set up the equation for Kc:
Kc = ([NO]^2[Cl2]) / [NOCl]
We know that the stoichiometric ratio between NO and NOCl is 2:1. Therefore, the concentration of NO is equal to twice the concentration of NOCl.
[NO] = 2 × [NOCl] = 2 × 0.440 M = 0.880 M
Since the stoichiometric ratio between Cl2 and NOCl is 1:1, the concentration of Cl2 is equal to the concentration of NOCl.
[Cl2] = [NOCl] = 0.440 M
Now we can substitute the values into the equilibrium expression:
Kc = ([NO]^2[Cl2]) / [NOCl]
= (0.880 M)^2 × 0.440 M / 0.440 M
= 0.880 M
Therefore, the value of Kc for the reaction NOCl(g) -> 2NO(g) + Cl2(g) at 700K is 0.880.
To calculate the value of Kc for the reaction, you need to use the equilibrium concentrations of the reactants and products. The balanced equation for the reaction is:
2NOCl(g) ⇌ 2NO(g) + Cl2(g)
The reaction can be represented by the equation:
Kc = [NO]^2[Cl2] / [NOCl]^2
Given that the equilibrium concentration of NOCl is 0.440 M, you can substitute this value into the equation as [NOCl]. Since the stoichiometric coefficient of NOCl is 1, this concentration can also be considered as the concentration of NOCl.
Now, you need to find the equilibrium concentrations of NO and Cl2. Since the stoichiometric coefficients of both NO and Cl2 are 2 in the balanced equation, the equilibrium concentrations of NO and Cl2 will be half the equilibrium concentration of NOCl.
Equilibrium concentration of NO = 0.440 M / 2 = 0.220 M
Equilibrium concentration of Cl2 = 0.440 M / 2 = 0.220 M
Now, substitute these values into the equation:
Kc = [NO]^2[Cl2] / [NOCl]^2
= (0.220 M)^2 * (0.220 M) / (0.440 M)^2
= 0.048
Therefore, the value of Kc for the reaction is 0.048.