Multiple Choice
Given the reaction 2NO(g) + 2H2(g) → N2(g) + 2H2O(g), which of the following represents the correct rate law if the reaction is first order in H2 and second order in NO?
597
views
15. Chemical Kinetics
Rate Law
Multiple Choice
Given the reaction A + 2B → C + 2D, which of the following is an incorrect statement about the rate of the reaction?
A
Rate of the reaction = Rate of production of C
B
Rate of the reaction = Δ[C]/Δt
C
Δ[A]/Δt = -Δ[B]/2Δt
D
Rate of the reaction = Δ[D]/2Δt
Verified step by step guidance1
Understand the stoichiometry of the reaction: A + 2B → C + 2D. This indicates that for every mole of A that reacts, 2 moles of B are consumed, producing 1 mole of C and 2 moles of D.
The rate of a reaction is typically expressed in terms of the change in concentration of reactants or products over time. For this reaction, the rate can be expressed as the change in concentration of A, B, C, or D over time.
The rate of disappearance of A can be expressed as Δ[A]/Δt, and since A is a reactant, this rate is negative.
The rate of disappearance of B can be expressed as Δ[B]/Δt, and since 2 moles of B are consumed for every mole of A, the rate of disappearance of B is twice that of A, hence Δ[B]/2Δt.
The rate of appearance of C and D can be expressed as Δ[C]/Δt and Δ[D]/2Δt respectively. Since C and D are products, these rates are positive. The statement Δ[A]/Δt = -Δ[B]/2Δt is incorrect because it does not correctly relate the stoichiometry of the reaction to the rate expressions.
Related Videos
Related Practice
