H2(g) + I2(g) *)
2HI(g) + heat
Which response includes all the following
that will shift the equilibrium to the left, and
no others?
To determine the factors that will shift the equilibrium to the left in the given reaction, we need to consider Le Chatelier's Principle. According to this principle, changes in temperature, pressure, and concentration can affect the direction of a chemical equilibrium.
1. Decreasing temperature: Lowering the temperature will shift the equilibrium to the left because the reaction is exothermic, meaning it releases heat. The reaction will favor the side with fewer moles of gas (the reactant side), in this case, H2(g) + I2(g).
2. Increasing pressure: Since the reaction involves only gases, increasing the pressure will favor the side with fewer moles of gas. Again, shifting the equilibrium to the left, which means favoring the reactant side (H2(g) + I2(g)).
3. Increasing the concentration of HI(g): Adding more HI(g), which is a product, will result in an excess of products. According to Le Chatelier's Principle, the equilibrium will shift to the left to consume the excess HI(g) and restore equilibrium.
Therefore, the factors that will shift the equilibrium to the left (and no others) are decreasing temperature, increasing pressure, and increasing the concentration of HI(g).