Calculating Concentrations of Gases at Equilibrium: A Chemistry Problem Solving
What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 9.91 L?
The concentrations of the three gases once equilibrium has been reestablished, after compressing the equilibrium mixture to a volume of 9.91 L, are: [COCl2] = 0.274 M [CO] = 0.105 M [Cl2] = 0.105 M
Understanding Equilibrium Concentrations
Initial Conditions: An equilibrium mixture of the three gases in a 17.7 L container at 617 K contains initial concentrations as follows: [COCl2] = 0.154 M [CO] = 5.92E-2 M [Cl2] = 5.92E-2 M
Application of Le Chatelier's Principle: When the equilibrium mixture is compressed to a volume of 9.91 L at constant temperature, we need to determine the concentrations of the gases once equilibrium is reestablished. The principle of Le Chatelier allows us to predict the shift in equilibrium to relieve the imposed stress (change in volume).
Calculating New Concentrations: By using the ideal gas law, we can relate the initial and final concentrations based on the volumes: [COCl2]2 = [COCl2]1 * (V1 / V2) [CO]2 = [CO]1 * (V1 / V2) [Cl2]2 = [Cl2]1 * (V1 / V2)
Final Concentrations: Calculating the new concentrations after compression: [COCl2] = 0.154 M * (17.7 L / 9.91 L) = 0.274 M [CO] = 5.92E-2 M * (17.7 L / 9.91 L) = 0.105 M [Cl2] = 5.92E-2 M * (17.7 L / 9.91 L) = 0.105 M
Conclusion: The concentrations of COCl2, CO, and Cl2 reach 0.274 M, 0.105 M, and 0.105 M, respectively, once equilibrium is reestablished after the compression of the mixture. This calculation demonstrates the application of equilibrium concepts in chemistry problem-solving.
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