5. The reaction A → B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, h 0 2 4 8 16 20 24 [A]. M 1.50 x 10-¹ 1.35 x 10-¹ 1.21 x 10-¹ 9.74 x 10-² 6.32 x 10-2 5.09 x 10-² 4.10 x 10-² (a) What is the average rate of reaction between 2 and 8 h? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 16 h. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.

B 8. D Trial 1 2 3 4 [A₂] 0.10 0.20 0.30 0.30 [B] 0.50 0.50 0.05 0.10 An experiment was conducted to determine the rate law for the reaction A2(g) + B(9) A₂B(g). The table above shows the data collected. Based on the data in the table. which statement is correct? Initial rate (Ms-¹) 2.5 x 10 5.0 x 10-4 5.0 × 10-5 1.0 x 10-4 Since the rate law can be expressed as ratek[A₂), tripling the concentration of A2 will cause a 9-fold increase in the rate of the reaction. Since the rate law can be expressed as rate k[A₂][B], doubling the concentrations of A₂ and B will quadruple the rate of the reaction. Since the rate law can be expressed as rate k[A] [B], tripling the concentration of A2 while keeping the concentration of B constant will triple the rate of the reaction. Since the rate law can be expressed as rate=k[A₂][B], doubling the concentration of B while keeping the concentration of A₂ constant will double the rate of the reaction.

The following data were collected for a certain reaction of the type A +B → products. Determine the specific rate constant for this reaction. [A]o, mol L-1 [B]o, mol L-1 Initial rate, mol L-1 s-1 Run i 0.200 0.300 2.44 x 10-2 ii 0.200 0.450 2.44 x 10-2 i 0.300 0.450 5.49 x 10-2 O A. 0.610 L mol s-1 B. 0.960 L mol1 s-1 C. 0.271 L mol-1 s-1 D. 0.407 L mol-1 s-1 O E. 0.120 L mol-1 s-1

Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A] (M) 0.00 0.450 0.50 0.300 1.00 0.225 1.50 0.180 2.00 0.150 2.50 0.130 3.00 0.115 3.50 0.100 4.00 0.090

1. Given the following data, determine the orders (m and n) with respect to the concentrations of A and B in the reaction Orders: [A] 0.020 M 0.020 M 0.010 M 0.010 M m= A+B products Rate = k[A][B]" [B] 0.020 M 0.010 M 0.020 M 0.010 M n = Time for reaction 19 sec 19 sec 76 sec 76 sec What time would you predict if both concentrations of A and B were made to be 0.040 M?

2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|

Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A](M) 0 0.5 1.5 0.42 3 0.335 4.5 0.25 6 0.17 7.5 0.085 9 0.003