Consider the following rection and rate law:
\(2 A+3 B+C \rightarrow 4 D\)
rate \(=\mathrm{k}[\mathrm{A}][\mathrm{C}]^{3}\)
If you were to increase the amount of \(\mathrm{A}\) by 16 , increase the amount of \(\mathrm{B}\) by 10 , and cut the amount of \(\mathrm{C}\) in half, what would that do to the rate of the reaction?
new rate \(=\quad \mathrm{x}\) old rate.
2) 16 marks] Consider the reaction 4A+ B+ 2C D +3E where the rate law is defined as d[B] k[A][B][C]3 dt An experiment is carried out where [A]o = [C]o = 2.00 M and [Blo = 1.00 x 103 M If after 200. seconds, [B] = 2.35 x 10-5 M. (a) Calculate the value of k (b) Calculate the half-time for this experiment. 2) 16 marks] Consider the reaction 4A+ B+ 2C D +3E where the rate law is defined...
Consider the reaction X Y +Z Which of the following is a possible rate law? a) Rate = k[X] b) Rate = K[Y] c) Rate = k[Y][Z] Rate = k[X][Y] Rate = k[Z] e) Rate 3. What are the units for the rate constant for an overall third order reaction? a) L/mol:s b) LP/mol.s mol/L'S e) L2 For which order reaction is the half-life of the reaction inversely proportional to k, the rate constant? a) zero order b) first order...
22. The rate law for the chemical reaction shown below has been determined experimentally: Rate = k[O3][CI]. What is the overall order of the reaction? 03(g) + Cl(g) → O2(g) + ClO(g) a. 3 b. 5 d. 2 8. The following data were obtained for the hypothetical reaction A+B → products. [A]o (M) 4.0 2.0 4.0 [B]. (M) 6.0 6.0 3.0 Initial Rate (M/s) 1.60 0.80 0.40 What is the overall order of this reaction? a. 3 b. 12 c....
Consider the following reaction and its associated rate law A + B - C; rate = k[A]2 Which of the following will not increase the rate of the reaction? Select one: a. increasing the concentration of reactant A O b. increasing the concentration of reactant B O c. increasing the temperature of the reaction d. adding a suitable catalyst O e. all of the above
Consider the hypothetical reaction: A + B +2C -------> 2D + 3E, where the rate law is: Rate = -delta[A] / delta t = k[A][B]^2. An experiment is carried out where [A]0 = 1.0*10^-2M, [B]0 = 3.0M, [C]0 = 2.0M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8*10^-3M. a) Calculate the value of k for the reaction. b) Calculate the half-life for this experiment. c) Calculate the concentration of A after 13.0 seconds d)...
The reaction between peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) and iodide in basic solution is proposed to occur according to the following mechanism:Step \(1: \mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{I}^{-} \rightarrow \mathrm{HOl}+\mathrm{OH}^{-}\) slowStep \(2: \mathrm{OH}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{H}_{2} \mathrm{O}\) fastStep \(3: \mathrm{HOl}+\mathrm{H}^{+}+\mathrm{I}^{-} \rightarrow \mathrm{I}_{2}+\mathrm{H}_{2} \mathrm{O}\) fastThe rate law for this mechanism would be?Select one:O. Rate \(=\mathrm{k}\left[\mathrm{H}_{2} \mathrm{O}_{2}\right][\mathrm{I}]\left[\mathrm{OH}^{-}\right]\left[\mathrm{H}^{+}\right]\)0. Rate \(=k\left[\mathrm{H}_{2} \mathrm{O}_{2}\right]\)O C. Rate \(=k[\mathrm{OH}]\left[\mathrm{H}^{+}\right]\)O d. Rate \(=k\)O e. Rate \(=\mathrm{k}\left[\mathrm{H}_{2} \mathrm{O}_{2}\right][\mathrm{I}]\)
Consider the reaction A ⟶ Products. The rate law for this reaction is rate = k[A] where k= 3.00 X × 10-3 s-1 at a particular temperature. If the initial [A] = 0.500 M, what will be the concentration of A after 2.00 minutes
Given the following proposed mechanism, predict the rate law for the overall reaction. A_2 + 2B rightarrow 2AB (overall reaction) A) Rate = k[A][B] B) Rate = k[A_2][B] C) Rate = k[A_2][B]^1/2 D) Rate = k[A_2] E) Rate = k[A_2]^1, 2 [B]
For the reaction: A rightarrow B + C and a Rate Law of: Rate = k [A]^X, determine the value of x in each of the following cases: WHY? a. There is no rate change when [A] is tripled b. The rate increases by a factor of 9 when [A] is tripled c. When [A] is doubled, the rate increases by a factor of 8
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)...