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18 Nov 2019
Consider the reaction: Br2 + Cl2 <-----> 2BrCl
The Kc for the reaction at 400 degrees C is 7.00
If you place 0.50 moles of bromine gas and 0.50 moles of chlorine gas in a 1 liter container, what will be the concentration of BrCl at equilibrium? What will be the concentration of Br and Cl at equilibrium?
Using the same reaction, you decide to repeat the experiment using 0.10 moles of Br, 0.10 moles of Cl, and 0.10 moles of BrCl all in a one liter container.
Is this reaction at equilibrium?
What are the equilibrium concentrations of each component of the reaction?
Consider the reaction: Br2 + Cl2 <-----> 2BrCl
The Kc for the reaction at 400 degrees C is 7.00
If you place 0.50 moles of bromine gas and 0.50 moles of chlorine gas in a 1 liter container, what will be the concentration of BrCl at equilibrium? What will be the concentration of Br and Cl at equilibrium?
Using the same reaction, you decide to repeat the experiment using 0.10 moles of Br, 0.10 moles of Cl, and 0.10 moles of BrCl all in a one liter container.
Is this reaction at equilibrium?
What are the equilibrium concentrations of each component of the reaction?
Jean KeelingLv2
12 Sep 2019
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