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.

6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179

The reaction A → C was performed and the concentration vs. time data below collected.   time, s 0 1 2 3 4 5 6 7 8 [A], mol/L 0.9541 0.5884 0.3629 0.2238 0.1380 0.08512 0.05250 0.03238 0.01997   Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]x rate constant (without units) =

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.

Q6. Answer the following questions based on the data provided: N203(g) - NO,(g) + NO,(g) Time (s) (N,O.] (M) 1.000 25 0.822 50 0.677 75 0.557 100 0.458 0.377 125 150 0.310 0.255 0.210 175 200 a. What is the overall order of the reaction? b. Calculate the value of the rate constant. c. What is the concentration of dinitrogen monoxide at 250s?

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?|

The reaction A →B is found to be first order. At 650 K, 45 % of A has been converted to B in 75.0 minutes. At 650 K, calculate the rate constant of this reaction with the unit s O A. 1.77 x 1045-1 O B. 3.59 x 102 s-1 O. 2.72 x 10-6 5-1 O D. 1.33 x 1045-1 E. 1.82 x 10-6 5-1