The following 4 questions refer to a reaction involving three reactants A, B, C.

Question

The following 4 questions refer to a reaction involving three reactants A, B, C. Select from choices below: a. Rate = k[A]^2 b. Rate = k[A] c. Rate = k [A]^0[B]^0 d. Rate = k [A] [B]^2[C]^2 e. Rate = k [A]^0[B]^2 A graph of the concentration versus time produces a straight line. A rate law where the half-life is independent of the initial concentration. A rate law for a reaction that is independent of concentration. A rate law that represents a reaction where doubling the concentration of A will lead to a four-fold increase in the rate Consider the reaction 2 A(g) rightarrow B(g) +3 C(g), a. Write the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products: b. When B is increasing at a rate of 0.044 M/s How fast is C increasing? Equation: Substitution: Rate of decrease: How fast is A decreasing? Equation: Substitution: Rate of decrease:

Explanation / Answer

6) The graph of concentration vs time is straight line for zero order reaction. Out of the options given, option c is zero orser rate law. So, correct option is a.

7) Half life is independent of initial concentration in first order reaction. option b is correct.

8) Rate law is independent of concentration for zero order and it is true for option c.

9) If the rate depends on square of [A], then the rate will become four times on doubling the [A]. So, correct option is a.

10) a) The rate of the reaction: rate = 1/2(-d[A]/dt) = (d[B]/dt) = 1/3(d[C]/dt)

b) 1) equation: (d[B]/dt) = 1/3(d[C]/dt)

Substitution: 0.044 M/s = 1/3(d[C]/dt)

Rate of decrease = d[C]/dt = 3(0.044) = 0.132 M/s

2) equation: 1/2(-d[A]/dt) = (d[B]/dt)

Substitution: 1/2(-d[A]/dt) = 0.044

Rate of decrease = -d[A]/dt = 2(0.044) = 0.088 M/s

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