For the equation shown below, use Le Chatelier's principle to identify if the changes indicated will cause the reaction to A) shift left B) shift right C) have no change or D) no way to predict a change.
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A. shift left B. shift right C. have no change D. no way to predict a change
17. adding oxygen (O2)
18. taking away hydrogen (H2)
19. reducing the temperature
A. shift left (decrease in reactant to restore equilibrium)
B. shift left (decrease in reactant to restore equilibrium)
C. shift right (endothermic reaction will shift to absorb heat)
To use Le Chatelier's principle to identify the effect of the changes indicated, we need to analyze each change individually.
17. Adding oxygen (O2): In the equation shown, adding oxygen (O2) will not directly affect the reaction, as it is not directly involved in the balanced equation. Therefore, the answer is C) have no change.
18. Taking away hydrogen (H2): In the equation, removing hydrogen (H2) will disrupt the balanced equation. If hydrogen is a reactant, removing it will cause the equilibrium to shift to the right to replenish the reactant. On the other hand, if hydrogen is a product, removing it will cause the equilibrium to shift to the left to reestablish the balance. Without knowing if hydrogen is a reactant or product, we cannot determine the direction. Therefore, the answer is D) no way to predict a change.
19. Reducing the temperature: According to Le Chatelier's principle, decreasing the temperature will cause the reaction to shift in the direction that generates heat. This is because the decrease in temperature can be seen as removing heat from the system, and the reaction will try to counteract that by generating more heat. Therefore, the answer is C) have no change.
In summary:
17. Adding oxygen (O2) - C) have no change.
18. Taking away hydrogen (H2) - D) no way to predict a change.
19. Reducing the temperature - C) have no change.