A reaction is determined to be second order with respect to its single reactant, A. The rate constant is found to be k = 2.57 * 10-2 M-1s-1. Answer the following questions. a Write the integrated rate law for this reaction. b. Determine how long it would take for this reaction starting at 1.34 M of A to reach 0.0875 M of A c. Determine the concentration remaining of A after 765 s if the initial concentration is 0.954 M.

5. A laboratory experiment was done for the reaction below and the following data was obtained: A→ Products a. Reaction order. Time (hours) Concentration of A, mg/L 0 1 Plot the data in Excel and determine the following: b. Reaction rate, k. 23468 135 119 104 88 73 41 10

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.

Be sure to answer all parts. Consider the reaction A+BProducts From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. A. JA] (M) (BỊ (M) Rate (Mis) 1.50 1.50 3.20 x 10 1.50 2.50 3.20 x 10 Reaction 3.00 1.50 6.40 x 10