Consider the reaction: 2CO2(g)=2CO(g) + O2(g). A reaction mixture in a 5.0 L flask at a certain temperature. At equilibrium there are 85 g of CO2(g), 1.20 g of CO, and 0.688 g of O2(g). Calculate Kc.
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To calculate the equilibrium constant (Kc) for the given reaction, we need to use the molar concentrations of the reactants and products at equilibrium. However, we are only given the masses of the substances.
To find the molar concentrations, we need to first convert the given masses of CO2(g), CO(g), and O2(g) into moles. This can be done using the molar masses of the substances.
The molar mass of CO2 = 44.01 g/mol
The molar mass of CO = 28.01 g/mol
The molar mass of O2 = 32.00 g/mol
1. Convert the mass of CO2(g) to moles:
Mass of CO2(g) = 85 g
Moles of CO2(g) = Mass of CO2(g) / Molar mass of CO2
Moles of CO2(g) = 85 g / 44.01 g/mol
2. Convert the mass of CO(g) to moles:
Mass of CO(g) = 1.20 g
Moles of CO(g) = Mass of CO(g) / Molar mass of CO
Moles of CO(g) = 1.20 g / 28.01 g/mol
3. Convert the mass of O2(g) to moles:
Mass of O2(g) = 0.688 g
Moles of O2(g) = Mass of O2(g) / Molar mass of O2
Moles of O2(g) = 0.688 g / 32.00 g/mol
Now, we have the moles of CO2(g), CO(g), and O2(g). We can use these values to calculate the molar concentrations (M) by dividing the moles by the volume of the flask in liters (5.0 L in this case).
Molar concentration (M) = Moles / Volume
Remember, in this case, the volume is given as 5.0 L.
4. Calculate the molar concentrations of CO2(g), CO(g), and O2(g):
Molar concentration of CO2(g) = Moles of CO2(g) / Volume
Molar concentration of CO(g) = Moles of CO(g) / Volume
Molar concentration of O2(g) = Moles of O2(g) / Volume
Now that we have the molar concentrations, we can write the equilibrium constant expression for the given reaction:
Kc = [CO]^2 * [O2] / [CO2]^2
Substitute the calculated molar concentrations into the expression and calculate Kc:
Kc = ([CO]^2 * [O2]) / [CO2]^2
Calculating Kc with the given values will provide you with the equilibrium constant for the reaction.