Question
The number of molecular collisions increases when Responses A products are removed.products are removed. B more reactants are added.more reactants are added. C the reaction temperature is lowered.the reaction temperature is lowered. D the reacting molecules have an incorrect orientation upon impact.
Answers
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GPT-4o mini
The number of molecular collisions increases when **B) more reactants are added.**
Adding more reactants increases the concentration of molecules in a given volume, leading to a higher probability of collisions between the reactive molecules.
Here's a brief explanation of the other options:
- **A) Products are removed:** This can shift the equilibrium position according to Le Chatelier's principle but does not directly increase the number of collisions among reactants.
- **C) The reaction temperature is lowered:** Lowering the temperature generally decreases molecular motion and kinetic energy, leading to fewer collisions.
- **D) The reacting molecules have an incorrect orientation upon impact:** This statement implies that while collisions may occur, they are not effective in leading to a reaction if the orientation is incorrect. Thus, this also doesn't increase the number of effective collisions.
Therefore, option **B** is the best answer regarding the increase in molecular collisions.
Adding more reactants increases the concentration of molecules in a given volume, leading to a higher probability of collisions between the reactive molecules.
Here's a brief explanation of the other options:
- **A) Products are removed:** This can shift the equilibrium position according to Le Chatelier's principle but does not directly increase the number of collisions among reactants.
- **C) The reaction temperature is lowered:** Lowering the temperature generally decreases molecular motion and kinetic energy, leading to fewer collisions.
- **D) The reacting molecules have an incorrect orientation upon impact:** This statement implies that while collisions may occur, they are not effective in leading to a reaction if the orientation is incorrect. Thus, this also doesn't increase the number of effective collisions.
Therefore, option **B** is the best answer regarding the increase in molecular collisions.