Explain how the following changes in a reaction conditions will affect the position of the equilibrium below.
A (g) + B (aq) C (s) + heat
1. The temperature of reaction is raised by 20 degrees C
2. As the reacton progresses, more of the compound B is added to the reaction chamber so how does that affect equilibrium.
This is physics?
since it is exothermic, raising the temp will drive the reaction backwards.
Add B? Drives it to the right, more product.
To determine how changes in reaction conditions affect the position of equilibrium, we need to consider Le Chatelier's Principle. According to this principle, when a system at equilibrium is subjected to a stress, it will react in a way to counteract that stress and restore equilibrium. In the given reaction A (g) + B (aq) ⇌ C (s) + heat, let's explore the effects of the changes in reaction conditions:
1. The temperature of the reaction is raised by 20 degrees Celsius:
When the temperature is increased, the equilibrium will shift in the direction that absorbs heat. In this case, heat is a product of the reaction. To counteract the increase in temperature, the equilibrium will shift to the left, towards the reactants (A and B in this case). This will result in an increase in the concentration of A and B and a decrease in the concentration of C.
2. More of the compound B is added to the reaction chamber as the reaction progresses:
Adding more reactant B to the reaction chamber will disturb the equilibrium. According to Le Chatelier's Principle, if reactant B is added, the equilibrium will shift towards the products side to counterbalance the increase. In this case, the equilibrium will shift to the right, resulting in an increase in the concentration of C and a decrease in the concentrations of A and B.
In summary, raising the temperature will favor the reactants, while adding more compound B will favor the products.