initially 1 mol each of gaseous carbon dioxide, co2(g) and hydrogen h2(g) is inhected into a 10.0L reaction chamber at 986 degrees. What is the predicted concentration of each entity at equilibrium?
the equation is as follows:
co2(g)+ h2(g)= co(g)+h20 (g)
k=1.60 at 986 degrees
You need to locate the caps key on yur keyboard and use it.
The concn is 1mol/10 L = 0.1M
........CO2 + H2 --> CO + H2O
I.......0.1...0.1....0.....0
C.......-x....-x.....x.....x
E......0.1-x..0.1-x..x.....x
Substitute the E line into the K expression and solve for x, then evaluate 0.1-x for the others.
thanks for replying back
Keq=(x)(x)/(0.1-x)(0.1-x)
Keq=x^2/x^2-0.2x+0.01
do i take the square root of each side and then...
Yes you would; however, you have expanded the (0.1-x)(0.1-x) unnecessarily. I would have done it this way. It's less work.
Keq = (x)(x)/(0.1-x)(0.1-x)
Keq = x^2/(0.1-x)^2
sqrt (Keq) = x/0.1-x and go from there.
To determine the predicted concentration of each entity at equilibrium, we need to use the equilibrium constant (K) and the initial concentrations of carbon dioxide (CO2(g)) and hydrogen (H2(g)).
The general equation for the equilibrium constant (K) expression is:
K = [C]^c [D]^d / [A]^a [B]^b
In this case, the equation is:
CO2(g) + H2(g) = CO(g) + H2O(g)
The equilibrium constant (K) is given as 1.60.
To set up our equation, we let x be the amount of CO(g) and H2O(g) formed at equilibrium. This means that the amount of CO2(g) and H2(g) consumed is also x. Therefore, the concentration of CO2(g) and H2(g) at equilibrium is the initial concentration minus x.
So, the equilibrium concentrations are as follows:
[CO2(g)] = [initial conc. CO2(g)] - x
[H2(g)] = [initial conc. H2(g)] - x
[CO(g)] = x
[H2O(g)] = x
Now, we can substitute these values into our equilibrium constant expression:
K = [CO(g)][H2O(g)] / [CO2(g)][H2(g)]
⇒ 1.60 = x * x / ([initial conc. CO2(g)] - x) * ([initial conc. H2(g)] - x)
To solve this quadratic equation, we can rearrange it and solve for x:
1.60 * ([initial conc. CO2(g)] - x) * ([initial conc. H2(g)] - x) = x^2
Simplify further:
1.60 * [initial conc. CO2(g)] * [initial conc. H2(g)] - 1.60 * ([initial conc. CO2(g)] + [initial conc. H2(g)]) * x + 1.60 * x^2 = 0
Once we solve for x, we can substitute it back into the equilibrium concentrations equations to find the concentrations of each entity at equilibrium.