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The rate law for the reaction 3A(g) → C(g) is rate-kAI2 where k = 4.36 x...
15. A. B. C. D. E. The rate law for the reaction 3A - 2B is rate = k[A] with a rate constant of 0.0447 hr What is the half-life of the reaction? 0.0224 hr 0.0645 hr 15.5 hr 22.4 hr 44.7 hr 4B is 600 x 10- 31 mol-1minHow long will
4) If the reaction SO2Cl2 → SO2 + Cl2 is first-order reaction. At 230oC, k = 0.125 hr-1. If the initial concentration of SO2Cl2 is 0.250 M, what is the concentration after 7.6 hours? How long will it take for the concentration of SO2Cl2 to drop to 0.0651 M? What is the half-life for this first order reaction?
The rate law for the reaction A B (unbalanced) is rate = k[A]2 with a rate constant of 0.25 M1 hr 1. What is the half-life of the reaction if the initial concentration is 0.275M? 1) 2.77 hr O2) 3.08 hr O 3) 16.2 hr O 4) 14.5 hr 5) 0.55 hr
4. The rate constant for the reaction 3AAR is 250 x 10 molminHow long will it take the concentration of A to drop from 0.75 M to 0.50 M? (6 points) 5. The rate constant for the reaction 3A - 2B is 0.0447 5. What is the half-life of the reaction? (2 points) 6. Consider the reaction 3A C. If the reaction is second order with a half-life of 20.0 hrs Starting the reaction with an initial concentration of A...
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
5. Consider the reaction below at 100°C T2U (g) --> 2T(g) + U (g) If given an initial reactant concentration [T2U]ο = 0.250 M, what is [T] after 15 minutes have elapsed? reaction rate is 9.30 x 10-3 M/s 5. Consider the reaction below at 100°C T2U (g) --> 2T(g) + U (g) If given an initial reactant concentration [T2U]ο = 0.250 M, what is [T] after 15 minutes have elapsed? reaction rate is 9.30 x 10-3 M/s rate law...
3. A reaction 2A 2B + C is known to follow second-order kinetics, with k = 7.20x10*M's' at 25.0 °C. (20 points) During one experiment, the initial concentration of A is [A]. = 0.120 M (a) Calculate the half-life (1,2), in hours, for this experiment. (b) Calculate the initial reaction rate (in M/s) for this reaction (4 points) (c) How long will it take (in hours) for the concentration of C to reach [C] = 0.0540 M (6 points) (d)...
For the simple decomposition reaction AB(g) → A(g) + B(g) rate = k[AB]2and k = 0.90 L/mol·s. How long will it take for [AB] to reach 1/3 of its initial concentration of 1.50 M? t = ___ s
1. For the reaction, A + 2B + C +2D, some measurements of the initial rate of reaction at varying concentration gave the following data. run # [A] [B] rate, moll's eman 19 1 0.100 0.200 0.000360 20.150 0.200 0.000540 3 0.150 0.250 0.001055 012 noite a. the rate law is therefore: rate = k[A[B] b. the rate law is therefore: rate = k[A][B]', UX physHouten c. the rate law is therefore: rate = K[A[B] d. the rate law is...
This reaction was monitored as a function of time: A rightarrow B + C A plot of ln[A] versus time yields a straight line with slope -0.0045/s. a. What is the value of the rate constant (k) for this reaction at this temperature? b. Write the rate law for the reaction. c. What is the half-life? d. If the initial concentration of A is 0.250 M, what is the concentration after 225 s?