To understand what happens to the amount of [tex]\( \text{SO}_3 \)[/tex] when the reaction shifts to the right, let's analyze the given chemical reaction:
[tex]\[
2 \text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2 \text{SO}_3(g) + 198 \text{kJ}
\][/tex]
1. Balanced Chemical Equation:
- Reactants: [tex]\( 2 \text{SO}_2(g) \)[/tex] and [tex]\( \text{O}_2(g) \)[/tex]
- Products: [tex]\( 2 \text{SO}_3(g) \)[/tex] and heat (198 kJ)
2. Shifting to the Right:
- A shift to the right in a chemical equilibrium means that the reaction is proceeding in the forward direction - towards the formation of more products from the reactants.
3. Formation of Products:
- As the reaction shifts to the right, more [tex]\( \text{SO}_2(g) \)[/tex] and [tex]\( \text{O}_2(g) \)[/tex] are being converted into [tex]\( \text{SO}_3(g) \)[/tex].
- Since [tex]\( \text{SO}_3 \)[/tex] is a product, the amount of [tex]\( \text{SO}_3 \)[/tex] will increase.
Thus, when the reaction shifts to the right, the amount of [tex]\( \text{SO}_3 \)[/tex] goes up.
Given the choices:
A. The amount of [tex]\( \text{SO}_3 \)[/tex] goes down.
B. The amount of [tex]\( \text{SO}_3 \)[/tex] does not change.
C. The amount of [tex]\( \text{SO}_3 \)[/tex] goes up.
The correct answer is:
C. The amount of [tex]\( \text{SO}_3 \)[/tex] goes up.
