see experiment 1 and 3:
[A] becomes 3 times
[B] is constant
rate becomes 9 times
so, order of A is 2
see experiment 1 and 2:
[A] is constant
[B] doubles
rate is constant
so, order of B is 0
overall order = 2 + 0 = 2
Rate law is:
rate = k*[A]^2
Put values from 1st row of table in rate law
rate = k*[A]^2
2.83 = k*0.273^2*499.0^0
k = 37.97 M-1.s-1
Answer: 37.97
Calculate the rate coefficient (mol-1 dms-2) for the following reaction: A+B → Products Experiment [A] (mol...
Part A The data in the table below were obtained for the reaction: A + B → P Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.273 0.763 2.83 2 0.273 1.526 2.83 3 0.819 0.763 25.47 The magnitude of the rate constant is ________. The data in the table below were obtained for the reaction: A + B → P Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.273 0.763 2.83 2 0.273 1.526 2.83...
The data below were obtained for the reaction A + B —> P Experiment number [A] (M)) [B] (M) Initial rate (M/s) 1 0.273 0.763 2.83 2 0.273 1.526 2.83 3 0.819 0.763 25.47 (C) What is the overall order of the reaction? (D) Write the rate law for this reaction. (E) Please calculate the rate constant for the reaction.
The data below were obtained for the reaction A + B —> P Experiment number [A] (M)) [B] (M) Initial rate (M/s) 1 0.273 0.763 2.83 2 0.273 1.526 2.83 3 0.819 0.763 25.47 (A) What is the order of the reaction with respect to A? (B) What is the order of the reaction with respect to B? (C) What is the overall order of the reaction?
we - Google Given the following data, determine the rate law for the following reaction 2A+B+2C - products Experiment 2 [A] 0.273 0.819 0.273 0.273 [B] [C] Rate (M/s) 0.763 0.400 3.0 0.763 0.400 9.0 1.526 0.400 12.0 0.763 0.800 4 6.0 Rate = k[A][B][C] Rate = k[A][B][C] Rate = K[A] [B]*C]2 Rate = K[A]2[B] [CH Rate = k[A] [B][C] Question 16 5 pts SOCl2 gas dissociates into SO2 and Cly via the following reaction: SOCI2(e) + SO2(g) + Cl2(8)...
Select the rate law that corresponds to the data shown for the following reaction. A+B Products Experiment [A] (mol dm3) 0.012 0.024 0.024 0.012 [B] (mol dm3) 0.035 0.070 0.035 2 3 4 Initial Rate(mol dm-3 3-1) 0.10 0.80 0.10 0.80 Rate = k[B] Rate = K[B] Rate = k [A] [B]3 Rate = k[A] [B]
For the overall reaction A+B+C products the following initial rate data were obtained: Rate, mol L-'s-1 Experiment # [A] [B]. [C]. 0.200 0.200 0.200 0.300 0.200 0.200 0.200 0.400 0.200 0.300 0.200 0.400 How many of the following statements are correct? 2.00 2.83 4.00 1) the reaction is first order in A 2) the overall reaction is second order 3) the rate of the reaction is proportional to [B]"2 4) the value of the specific rate constant, k, is 50.0...
The reaction between A and B was investigated by a student who claimed to have obtained the following data: Trial A] (M) 0.273 0.273 0.546 0.763 1.526 0.763 Rate (M/s) 2.63 6.63 4.18 2 3 What reaction orders for A and B, respectively, did the student obtain from the data? O3/4, 2/3 3/2,5/4 O 2/3, 1/2 2/3,4/3 4/3,1/2
7. Given the following data for the reaction: NOrg) Expt.TAIIM +1/2 CHE)-NOCU8 BIM 0273 0.819 0.273 0.273 0.763 1526 0.763 0.400 0400 0.800 3.0 9.0 12.0 (a) Calculate the order with respect to each reactant. Om, n.p) 6.0 (b) Calculate k. (3 pts) (c) Write the rate law. (3 pts) 8. The reaction of NO with H2 is thought to occur in three elementary steps: NO + H2N+H2O (slow) N+NO N20 N20 +H2N2+H20 (fast) (a) Identify the reaction intermediate )....
A reaction 2A → P has a second-order rate law with kf = 1.44 dm3 mol-1 s -1 . Calculate the time required for the concentration of A to change from 0.460 mol dm-3 to 0.046 mol dm-3 .
For a reaction A + B → products, the following data were collected. Experiment Number Initial Concentration of A (M) Initial Concentration of B (M) Observed Initial Rate (M/s) 1 3.44 4.04 1.97 ✕ 10−4 2 4.69 4.04 3.66 ✕ 10−4 3 3.44 5.36 1.97 ✕ 10−4 Calculate the rate constant for this reaction. M−1·s−1