Trial 1 2 3 [A] (M) 0.200 0.400 0.200 A+BAB What is the rate constant for the reaction above? [B] (M) 0.200 0.200 0.400 Rate (M/s) 2.00 x 10-² 8.00 x 10-² 4.00 x 10-²
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- Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.360 0.290 0.0144 2 0.360 0.580 0.0144 3 0.720 0.290 0.0576 k=Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.340 0.210 0.0204 2 0.340 0.420 0.0204 3 0.680 0.210 0.0816 ?=Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.360 0.330 0.0164 2 0.360 0.660 0.0164 3 0.720 0.330 0.0656 ?=? Units =?
- Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+DA+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.2100.210 0.3000.300 0.02210.0221 2 0.2100.210 0.6000.600 0.02210.0221 3 0.4200.420 0.3000.300 0.08840.08842. The initial rate of a reaction A + B → C was measured for several different starting concentrations of A and B, and the results are as follows: Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.100 0.100 4.0x10-5 2 0.200 0.200 4.0x10-5 3 0.200 0.100 16.0x10-5 Using these data, determine (a) the rate law for the reaction, (b) the rate constant, (c) the rate of the reaction when [A] = 0.050 M and [B] = 0.100 M.Fast pls i will give u like for sure solve this question correctly in 5 min i will give u like for sure The reaction rate between 6 s and 10 s is V = _______________ = -d[A]/second. (use 2 sig figs) The rate constant is k = ___________________(use units of s-1 and/or M-1 as needed, round to 2 sig. figs).
- Consider the reaction A+2B⇌CA+2B⇌C whose rate at 25 ∘C∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A][A](MM) [B][B](MM) Rate(M/sM/s) 1 0.20 0.010 4.8×10−4 2 0.20 0.020 9.6×10−4 3 0.40 0.010 1.9×10−3 Calculate the initial rate for the formation of CC at 25 ∘C∘C, if [A]=0.50M[A]=0.50M and [B]=0.075M[B]=0.075M. Express your answer numerically in molar per second using two significant figures.A certain first-order reaction ( A --> B) is 25% complete in 42 min at 25oC. What is its rate constant? ( Answer in min-1 with 2 sig figs.)For the reaction A à B + C, the time required to cause a concentration change of 2.4 x 10-4 M was measured. What is the reaction order for the reaction given following data: Trial 1: [A] = 0.50 M ; Time needed is 120.0 sec Trial 2: [A] = 1.00 M ; Time needed is 30.0 sec
- The initial rate of the reaction 2 A + 2 B → C + D is determined for several different initial conditions. The results obtained are tabulated below. Trial [A] [B] rate (M/s) 1 0.210 0.115 6.30 x 10-4 2 0.210 0.230 2.51 x 10-3 3 0.420 0.115 1.25 x 10-3 4 0.420 0.230 5.13 x 10-3 a) Determine the rate law and the rate constant from these data. b) Determine the specific rate constant from the data.Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?] (?) [?] (?)[) Rate (M/s) 1 0.370 0.390 0.0234 2 0.370 0.936 0.135 3 0.592 0.390 0.0374 ?= ? units= ?In a temperature-jump experiment to investigate the kinetics of an isomerization reaction that is first-order in both directions, the relaxation t ime was measured as 27.6 μS. The rate constant for the forward reaction is known to be 12.4 ms-1. Ca lcu late the rate constant for the reverse reaction.