You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions:   Experiment [A] (M) [B] (M) Rate (M/s)   1 1.6 0.4   2 3.2 0.4   (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A]x [B]y? Choose all correct possibilities. [A] = 3.2 and [B] = 0.8 [A] = 1.6 and [B] = 1.2 [A] = 3.2 and [B] = 0.4 [A] = 3.2 and [B] = 1.2 [A] = 4.8 and [B] = 0.4 [A] = 6.4 and [B] = 0.4 [A] = 8.0 and [B] = 0.4 [A] = 1.6 and [B] = 0.8 (b) For a reaction of the form, A + B + C --> Products, the following observations are made: tripling the concentration of A increases the rate by a factor of 3, doubling the concentration of B has no effect on the rate, and tripling the concentration of C increases the rate by a factor of 27. Select the correct rate law for this reaction from the choices below. Rate = k[A][B][C]Rate = k[A][C]     Rate = k[A]2 [C]Rate = k[A][C]2Rate = k[A]2 [C]2 Rate = k[A]3 [C] Rate = k[A][C]3 (c) By what factor will the rate of the reaction described in part (b) above change if the concentrations of A, B, and C are all halved (reduced by a factor of 2)? The rate will be the original rate multiplied by a factor of .___

For the reaction: 2X + Y → W, the reaction rate law is R = k [X]2[Y] By what factor does the rate of the reaction increase if the concentration of X is doubled and the concentration of AND?   12   18   6   5

For a hypothetical reaction: A + 2B + C>D +E The rate law has been determined and is as follows: Rate = k[A][B]? What happens to the reaction rate when we make each of the following concentration changes? a) We triple the concentration of A without changing the concentration of B or C. b) We triple the concentration of B without changing the concentration of A or C. c) We triple the concentration of C without changing the concentration of A or B. d) We triple the concentrations of A, B and C simultaneously. e) We triple the concentration of D.

Consider the rate law: Rate = k [A]2[B][C]1/2. How does the rate of the reaction change if theconcentration of C is doubled? a) The rate increases by a factor of 1.414b) The rate increases by a factor of 1.732c) The rate reduces by a factor of 1.732d) The rate triplese) The rate reduces by a factor of 1.414

An experiment produced the data presented in the following Table Write the rate law for the reaction of N2 with O2. N2(g)  +  O2(g)  →  2NO(g) Determine the overall reaction order. Determine the rate constant and its units.

2) Can some one explain the question

Part A(iii)

2 A(aq) + 3 B(aq) A2B3(aq) An experiment is conducted at 25 C and the rate of appearance of the product ABa(aq) is measured as the concentrations of the reactants were varied. Data from the trials are shown below. Initial Rate of Trial [A] (M) [B] (M) Appearance of A2B3 (M/s) 5.0 x 10 4.5 x 10 1.0 x 10 0.200 0.300 0.200 0.900 0.400 0.300 4 0.135 0.225 ??? Determine the rate law for the reaction. Justify your answer. Determine the value of k, including units. Determine the rate of Trial 4. a. b. с. d. Determine the initial rate of disappearance of A for trial 2. A possible reaction mechanism has a 1" elementary step as shown below: e. A +BAB Could this first step be the rate determining step? Explain your reasoning. In the reaction mechanism the compound MnO2 appears. A student makes the claim f. "The order of MnO2 must be zero since it does not appear in the overall balanced equation". Do you agree or disagree with the student? Explain your reasoning. g. In trial 1, 10 mL of A and 10…

A reaction has a rate law of Rate = (1.25 M⁻²s⁻¹)[A][B]². What concentration of [B] would give the reaction a rate of 0.0455 if the concentration of [A] is 0.250 M?

Consider the reaction A → P where the rate constant is k.a) If the reaction is half a degree with respect to [A], then the integrated rate equation for this reactionwhat?b) How would you create a graph to determine the rate constant k for the reaction?c) What is the half-life of this reaction? Does the reactant depend on the initial concentration?