Multiple Choice
The gas-phase reaction CH3NC → CH3CN has been studied in a closed vessel, and the rate equation was found to be: Rate = −Δ[CH3NC]/Δt = k[CH3NC]. Which one of the following actions is least likely to cause a change in the rate of the reaction?
A) Lowering the temperature
B) Adding a catalyst
C) Using a larger initial amount of CH 3NC in the same vessel
D) Using a bigger vessel, but the same initial amount of CH 3NC
E) Continuously removing CH 3CN as it is formed
Correct Answer:
Verified
Correct Answer:
Verified
Q1: For the reaction 3A(g) + 2B(g) →
Q2: A catalyst accelerates a reaction because<br>A)it increases
Q3: The reaction CH<sub>3</sub>NC(g) → CH<sub>3</sub>CN(g) is first-order
Q4: Sulfur trioxide can undergo decomposition according to
Q6: Ammonia will react with oxygen in the
Q7: Which of the following sets of units
Q8: The kinetics of the decomposition of dinitrogen
Q9: The units of the rate of reaction
Q10: What is the molecularity of the following
Q11: Cyclopropane is converted to propene in a