2.c and 2.d 2. The rate law for the reaction A+B a. Write the rate law...
Consider the following reaction: A+B+C→D The rate law for this reaction is as follows: Rate=k[A][C]2[B]1/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.19×10−2 mol⋅L−1⋅s−1 . What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled?
Consider the following reaction: A + B + C +D The rate law for this reaction is as follows: Rate = k Alla B11/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.14x10-2 M/s. Part A What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? VO AED A O O ? Rate 2 = M/s Submit Request Answer
answer all The reaction A+B +C+D rate = k[A] [B]? has an initial rate of 0.0730 M/s. What will the initial rate be if [A] is halved and (B) is tripled? initial rate: 0.3163 M What will the initial rate be if (A] is tripled and (B) is halved? initial rate: 0.0937 For the reaction 2 H2O(g) = 2H2(g) + O2(g) the equilibrium concentrations were found to be [H,O] = 0.250 M, [H] = 0.330 M, and (0,] = 0.800...
The reaction A+B rightarrow C+D rate=k[A][B]^2 has an initial rate of 0.0300 M/s. What will the initial rate be if [A] is halved and [B] is tripled? What will the initial rate be if [A] is tripled and [B] is halved?
Review Constants Periodic Table Consider the following reaction: A + B + C D The rate law for this reaction is as follows: Part A Rate = k., A][C] B1/2 What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.19x10-2 M/s. 18 AU A O O ? Rate 2 =...
a. Given these data for the reaction A + B → C, write the rate-law expression. Use k for the rate constant.) b. What is the value, with units, for the specific rate constant? The specific rate constant- Initial Rate of Initial [A] Initial [B] Formation of C Expt. (M) (M.s-1) 0.30 0.30 0.60 0.20 0.40 0.80 4.0 x 10-5 1.6 x 10-4 2.6 x 10-3
The reaction A + B -> C + D has been found to obey the following rate law: rate=k[A][B]2 and has an initial rate of 0.0130 M/s. What will be the rate of the reaction if [A] is tripled and [B] is halved?
If the rate law for a reaction is rate = k[A]2[B] a. What is the overall order of the reaction? b. If the concentration of A is doubled and the concentration of B is tripled, how will this affect the rate of the reaction? c. How will doubling the concentration of B while holding A constant affect the value of k (assuming that temperature remains constant)?
1. Initial rate data at 25.0 °C are listed below for the reaction: 2 HgCl2 (aq) + C,042 (aq) → 2 (aq) + 2 CO2(g) + HgCl(s) Expt. [HgCl2]0 [C:02) Initial rate/Ms? 0.100 0.20 0.100 0.40 3.1 x 105 1.2 x 104 6.2 x 10-5 0.050 0.40 Use the data to determine the rate law for the reaction. 2. At 500 °C, cyclopropane (C3H.) rearranges to propene (CH:CH-CH2): CH. (g) → CH,CH=CH2 (8) The reaction is first order and the...
a. Write the rate law for this reaction. b. Calculate the rate constant. c. At what rate does KI disappear if the initial concentrations are [KI] = 0.0450 M and [(NH4)2S2O8] = 0.120 M? d. At what rate does (NH4)2S2O8 disappear under the conditions given in part c? The powers of 10 in the last boxes are 10^-3 Some data for this reaction follows: Experiment INHA.SoJON) T [Kn Initial Rate of Appearance of KL CMU's) 0200 0100 4.76 x 10...