Absolutely, let's analyze the given chemical reaction step-by-step to determine what happens to the amount of HI when the reaction shifts to the right:
Given the reaction:
[tex]\[ 51.8 \, \text{kJ} + H_2(g) + I_2(g) \rightleftharpoons 2 \, HI(g) \][/tex]
This reaction can be interpreted as follows:
- [tex]\( H_2(g) \)[/tex] and [tex]\( I_2(g) \)[/tex] are the reactants.
- [tex]\( 2 \, HI(g) \)[/tex] is the product.
- The reaction is endothermic, meaning it absorbs heat (51.8 kJ) during the formation of [tex]\( HI(g) \)[/tex].
When the reaction shifts to the right, here's an explanation of the changes:
1. Shift to the Right Explanation:
- A shift to the right signifies that the reaction is proceeding in the forward direction.
- In a forward direction, more reactants (hydrogen gas [tex]\( H_2 \)[/tex] and iodine gas [tex]\( I_2 \)[/tex]) are being converted into products (hydrogen iodide [tex]\( HI \)[/tex]).
2. Impact on HI:
- As the reaction progresses to the right, the quantities of the reactants ([tex]\( H_2 \)[/tex] and [tex]\( I_2 \)[/tex]) will decrease because they are being used to form more products.
- Simultaneously, the quantity of the product, which is [tex]\( HI(g) \)[/tex], will increase because more [tex]\( HI \)[/tex] is being produced from the reactants.
Thus, when the reaction shifts to the right:
- The production of [tex]\( HI \)[/tex] increases, indicating that the amount of [tex]\( HI \)[/tex] (hydrogen iodide gas) will go up.
Therefore, the correct answer is:
[tex]\[ \boxed{\text{A. The amount of HI goes up.}} \][/tex]
