Answered

Westonci.ca is the ultimate Q&A platform, offering detailed and reliable answers from a knowledgeable community. Discover a wealth of knowledge from experts across different disciplines on our comprehensive Q&A platform. Discover in-depth answers to your questions from a wide network of professionals on our user-friendly Q&A platform.

Select the correct answer.

How can we increase the rate of collisions between the reactants in this reaction?

[tex]\[ Mg + 2 HCl \rightarrow MgCl_2 + H_2 \][/tex]

A. Increase the concentration of [tex]\( H_2 \)[/tex] in the reaction mixture.
B. Decrease the temperature of the reactants in the reaction mixture.
C. Increase the concentration of [tex]\( Mg \)[/tex] in the reaction mixture.
D. Decrease the temperature of the entire reaction mixture.
E. Decrease the concentration of [tex]\( HCl \)[/tex] in the reaction mixture.

Sagot :

GinnyAnswer
To increase the rate of collisions between the reactants in the given reaction:

[tex]\[ Mg + 2HCl \rightarrow MgCl_2 + H_2 \][/tex]

we need to consider the factors that influence collision frequency according to the collision theory. The collision theory states that for a chemical reaction to occur, reactant particles must collide with sufficient energy and proper orientation. The factors that can increase the rate of collisions include:

1. Increasing the concentration of reactants: Higher concentration means more reactant particles are available per unit volume, which increases the likelihood of collisions.
2. Increasing the temperature: Higher temperature increases the kinetic energy of the reactant molecules, causing them to move faster and collide more frequently and with greater energy.
3. Catalysts: Catalysts can provide an alternative pathway with a lower activation energy for the reaction, thus increasing the rate of reaction.

Given the options:
- A. Increase the concentration of [tex]\( H_2 \)[/tex] in the reaction mixture.
- Increasing the product concentration ([tex]\( H_2 \)[/tex]) does not alter the rate of reactant collisions.
- B. Decrease the temperature of the reactants in the reaction mixture.
- Decreasing the temperature would decrease the kinetic energy and reduce the rate of collisions.
- C. Increase the concentration of [tex]\( Mg \)[/tex] in the reaction mixture.
- Increasing the concentration of [tex]\( Mg \)[/tex] will increase the number of [tex]\( Mg \)[/tex] atoms available to collide with [tex]\( HCl \)[/tex] molecules, leading to an increased rate of collisions.
- D. Decrease the temperature of the entire reaction mixture.
- Similar to option B, decreasing the temperature will reduce the kinetic energy and the collision frequency.
- E. Decrease the concentration of [tex]\( HCl \)[/tex] in the reaction mixture.
- Decreasing the concentration of [tex]\( HCl \)[/tex] would result in fewer [tex]\( HCl \)[/tex] molecules, thereby reducing the rate of collisions.

The correct answer is:

C. Increase the concentration of [tex]\( Mg \)[/tex] in the reaction mixture.

This will increase the rate of collisions between the reactants, leading to a faster reaction rate.
Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. Westonci.ca is here to provide the answers you seek. Return often for more expert solutions.