The equilibrium constant for the following reaction is 0.16 M0.5 at 3000 K:
CO2(g) ↔ CO(g) + 0.5O2(g)
Determine Qc if the following amounts (in moles) of each component is placed in a 3.00 L container.
CO2 0.740
CO 0.470
O2 0.590
Give answer to 3 decimal places.
CO2(g) ↔ CO(g) + 0.5O2(g)
Quantities are given in mols and the volume is 3.00 L. Calculate M = moles/L for each, substitute each into the Qc expression and solve for Qc.
Qc = (CO)(O2)^1/2/(CO2)
Post your work if you get stuck.
That's my response with no name.
The equilibrium constant for the following reaction is 0.16 M0.5 at 3000 K:
I am unfamiliar with the notation of 0.16 M0.5. Please let me know what it means. Thanks
To determine Qc, we need to write the expression for the reaction quotient (Qc) using the given amounts of each component.
The expression for Qc is derived by dividing the product of the concentrations of the products (raised to their stoichiometric coefficients) by the product of the concentrations of the reactants (raised to their stoichiometric coefficients).
In this case, the reaction is:
CO2(g) ↔ CO(g) + 0.5O2(g)
The stoichiometric coefficients for the reactants and products in the balanced equation are 1 for CO2, 1 for CO, and 0.5 for O2.
Therefore, the expression for Qc is:
Qc = [CO]^1 * [O2]^0.5 / [CO2]^1
Substituting the given amounts into the expression:
Qc = (0.470)^1 * (0.590)^0.5 / (0.740)^1
Now we can calculate Qc:
Qc = (0.470) * (0.769) / (0.740)
Qc ≈ 0.379
So the value of Qc, when the given amounts are present in the 3.00 L container, is approximately 0.379.