Kinetics
What factor does NOT affect the rate of reaction as predicted by the collision model?
Why might increasing surface area lead to an increased reaction rate based on collision theory?
Which factor would not be expected to increase the number of effective collisions in a chemical reaction according to the collision model?
In terms of frequency of collisions, what effect does increasing pressure have on gases involved in a chemical reaction?
A lower activation energy can help increase the number of effective collisions. Which of the following contributes to that?
When more particles have a greater energy than it's activation energy, what happens to the reaction rate?
A student hypothesizes that stirring a solution containing two reacting liquids will speed up their chemical reaction; what is this hypothesis based on from a collision model perspective?
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A reaction is shown below: [CL(aq) + CIO^-(aq) + 2H^+(aq) → Cl2(g) + H20(l)]. By increasing [H^+] at a constant temperature, what effect will it have on the reaction?
What term describes the minimum energy that colliding particles need for a successful reaction?
What sets an ineffective collision apart from an effective collision? (A) there isn't enough force, (B), molecules move too slowly, (C), molecules aren't aligned right.