For the system 2A (g) + B( g) = 2C (g), if the initial concentration of pure C is 1.00 M, the equilibrium concentration is 0.40 M. What is the value of Kc?
Choose one answer.
a. 5.0
b. 0.45
c. 0.67
d. 2.2
e. 1.5
Set up an ICE chart and solve. Post your work if you get stuck.
2A + B= 2C
I 0 0 1.00
C 2X X -2X
E 2X X 1.00-2X
KC= 0.40= C^2/ A^2*B
square root 0.40 (x*x)=1.00-2x
0.40(X)^2 SQUARE ROOT 0.40-1.00
I ended up with 0.09 but when I plugged it back in then I don't get any of the above answers. I don't know what I was doing wrong.
2A + B ==> 2C
If Ceq = 0.4 and it was 1.0 initially, it must have changed by 1-0.4= 0.6
Therefore, B must have changed by +0.3 and A must hav changed by 0.6 so the final concns are
A = 0.6 M
B = 0.3 M
C = 0.4 M
Plug those in and calculate Kc.
In order to find the value of Kc for the given chemical reaction, we need to use the equilibrium concentrations of the substances involved. The equation for Kc is:
Kc = ([C]^2) / ([A]^2[B])
Given that the initial concentration of pure C is 1.00 M and the equilibrium concentration is 0.40 M, we can plug in these values into the equation to solve for Kc.
Kc = (0.40^2) / ([A]^2[B])
Unfortunately, the concentration of A and B are not provided, so we cannot calculate the exact value of Kc. Therefore, none of the answer options provided (a. 5.0, b. 0.45, c. 0.67, d. 2.2, e. 1.5) can be selected as the correct answer.