the reaction A + B --> C + D rate = k[A][B]^-2 has an initial rate of 0.0670 M/s, what will the initial rate be if [A] is tripled and [B] is halved

The reaction A+B longrightarrow C+D; rate=k[A][B]^ 2 has an initial rate of 0.0690 M /s. What will the initial rate be if [A] is halved and [B ] is tripled? And what will the initial rate be if [A] is tripled and [B] is halved?

Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.220 0.260 0.0189 2 0.220 0.520 0.0189 А + 2B → C+ D 3 0.440 0.260 0.0756 Units 0.0484 k M-'s-1 Incorrect

Given the information based on time and concentration, determine the order of the reaction and the rate constant k when graphing the following data: A--> C+D Time (s) (A] M 10 0.1000 50 0.0856 100 0.0749 200 0.0598 350 0.0460 500 0.0373 800 0,0271

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?

A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [4.] initial rate of reaction x10 1.91 M 0.885 M 0.894 M/s olo 0.813 M 0.885 M I|| M/s Ar 0.213 M 7.92 M

Consider the following rate law: Rate = k[B] Which of the following equations could be used to find the concentration of B at some time (t) in the reaction? A) [B] = [B]₀ - kt B) [B] = [B]₀ × e^(-kt) C) 1/[B] = 1/[B]₀ + 2kt D) All of the above

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCII → OI¯ + Cl¯ This rapid reaction gives the following rate data: |[OCI¯] (M) [I¯] (M) Initial Rate (M/s) 1.36 × 10-4 1.5 × 10- -3 3.0 × 10-³ 1.5 x 10- -3 1.5 x 10 -3 1.5 × 10-³ 3.0 × 10-³ 2.72 × 10-4 2.72 × 10-4 Calculate the rate constant with proper units. Express the rate constant to two significant figures. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash (e.g. ft * lb or ft-lb). k Submit Part C HÅ Value Request Answer Units ? Calculate the rate when [OC] = 2.3 × 10-³ and [I¯] = 6.0 × 10-4 Express the rate in molarity per second to two significant figures.

A+ B+ 2C - 2D+ 3E where the rate law is A[A] k[A][B]* Rate = - %3D At An experiment is carried out where [A], = 1.0 x 10-2 M, [B, = 6.0 M, and [C, = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. k%3= L mols 1 b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 17.0 seconds. Concentration= M d. Calculate the concentration of C after 17 seconds. Concentration=

A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [#] |H, Initial rate of reaction x10 1.23 M 1.86 M 3 4.00 x 10 Mls | M/s 1.23 M 0.309 M 0.716 M O Mis Mls 3.20 м do Ar