Imagine that the system is allowed to come to equilibrium. How would each of the following changes affect the equilibrium? Indicate whether the change would favor the formation of more products, more reactants, or would not lead to any change?
1 Answer
Here is my reasoning.
Let's treat the heat as a product and rewrite the equation as
Now, we can apply Le Châtelier's Principle to answer the questions.
A. Increasing the temperature
Adding more heat (on the right) causes the position of equilibrium to shift to the left.
The change favours the formation of more reactant.
B. Increasing the partial pressure of
Increasing the partial pressure of
The change favours the formation of more product.
C. Adding more
Adding more
The change favours the formation of more product.
D. Adding more
Adding more
The change leads to no change in the position of equilibrium.
E. Adding
The net ionic equation is
Neither
The change leads to no change in the position of equilibrium.