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
Maggie Manganese has 0.0056 g of paper clips, what would this represent in ng?
To determine the value of Kc for the given reaction and determine whether the reaction favors products or reactants, we need to calculate the reaction quotient (Qc) and compare it to Kc.
The reaction quotient, Qc, is calculated by substituting the molar concentrations of the reactants and products into the expression for the reaction quotient.
The general formula for the reaction quotient for the given reaction is:
Qc = ([CO]^2 x [O2]) / ([CO2]^2)
Let's calculate the values of Qc for each option provided:
Option A: [CO2] = 1.5 M, [CO] = 1.2 M, [O2] = 0.05 M
Qc = (1.2^2 x 0.05) / (1.5^2)
Option B: [CO2] = 8.3 M, [CO] = 0.05 M, [O2] = 0.50 M
Qc = (0.05^2 x 0.50) / (8.3^2)
Option C: [CO2] = 0.05 M, [CO] = 0.75 M, [O2] = 0.07 M
Qc = (0.75^2 x 0.07) / (0.05^2)
Now, to determine whether the reaction favors products or reactants, we compare Qc to Kc.
If Qc < Kc, it means that there are more reactants than products, and the reaction favors the formation of products.
If Qc > Kc, it means that there are more products than reactants, and the reaction favors the formation of reactants.
If Qc = Kc, it means that the reaction is in equilibrium, with equal amounts of reactants and products.
So, calculate Qc for each option and compare it to Kc = e^(-deltaH/RT).
Without knowing the temperature (T) value, we cannot calculate the actual Kc value or determine whether Qc is greater or smaller than Kc. Therefore, we are unable to determine which option favors products or reactants without the temperature information.