2CO2(G)--->2CO(g)+O2(g), deltaH=566kj
what is Kc and state whether the reaction favors products or reactants?
A.)[CO2]=1.5M, [CO]=1.2M, [O2]=0.05M
B.)[CO2]=8.3M, [CO]=0.05M, [O2]=0.50M
C.)[CO2]=0.05M, [CO]=0.75M, [O2]=0.07M
any work would be much appreciated!!!thank you
Kc = (right side)/(left side) with coefficients as exponents.
Kc = (CO)^2(O2)/(CO2)^2
Plug in values and calculate. If k is >1, products favored. If Kc<1, reactants favored.
To find the value of Kc for the given reaction, we need to set up the equilibrium expression using the concentrations of the reactants and products.
The general equilibrium expression for a reaction is given by:
Kc = [C]^c [D]^d / [A]^a [B]^b
Where A, B, C, and D represent the reactants and products, and a, b, c, and d represent the stoichiometric coefficients of the balanced equation.
In this case, the balanced equation is:
2CO2(g) --> 2CO(g) + O2(g)
The stoichiometric coefficients are:
[A] = [CO2], [B] = [CO], [C] = [CO], and [D] = [O2]
a = 2, b = 2, c = 2, and d = 1
Therefore, the equilibrium expression becomes:
Kc = ([CO]^2 [O2]) / ([CO2]^2)
Now, let's calculate the value of Kc for each option by plugging in the given concentrations:
Option A:
[CO2] = 1.5 M, [CO] = 1.2 M, [O2] = 0.05 M
Kc = (1.2^2 * 0.05) / (1.5^2)
Option B:
[CO2] = 8.3 M, [CO] = 0.05 M, [O2] = 0.50 M
Kc = (0.05^2 * 0.50) / (8.3^2)
Option C:
[CO2] = 0.05 M, [CO] = 0.75 M, [O2] = 0.07 M
Kc = (0.75^2 * 0.07) / (0.05^2)
Now, to determine whether the reaction favors the products or reactants, we compare the calculated values of Kc for the given options:
- If Kc > 1, it means there are higher concentrations of products, and the reaction favors the products.
- If Kc < 1, it means there are higher concentrations of reactants, and the reaction favors the reactants.
- If Kc = 1, it means the concentrations of reactants and products are equal, and the reaction is at equilibrium.
By calculating the values of Kc for each option, we can determine which one favors the products or reactants.