Calculate the equilibrium constant for the following reaction:
CO2(g) + H2(g) ↔ CO(g) + H2O(g)
where:
[CO2] = 0.0954M
[H2] = 0.0454M
[CO] = 0.0046M
[H2O] = 0.0046M
Select one:
a. 4.9 · 10–3
b. 4.9 · 10–2
c. 0.049
d. 2.04 · 102

Question

Calculate the equilibrium constant for the following reaction:
CO2(g) + H2(g) ↔ CO(g) + H2O(g)
where:
[CO2] = 0.0954M
[H2] = 0.0454M
[CO] = 0.0046M
[H2O] = 0.0046M
Select one:
a. 4.9 · 10–3
b. 4.9 · 10–2
c. 0.049
d. 2.04 · 102

jordanloveangel · Answer

attachment

aaronq · Answer

^ lol wat

first write the equilibrium expression

For a general reaction where lowercase a, b, c and d are coefficients and uppercase A, B C and D the species:
 
$\sf a ~A+ b~B\rightleftharpoons c~C+d~D$

$\sf K=\dfrac{[products]}{[reactants]}=\dfrac{[C]^c[D]^d}{[A]^a[B]^b}$