2) (18 points) A second-order reaction A B begins at 11:30AM with [A] 0.75 M. If...
A second order reaction A->B begins at 10:45 AM with [A]= 1.25 M. If the rate constant k= 0.032M^-1 s^-1, at what clock time does [A]= 0.05 M?
1. A reaction is second order in[A] and second-order in [B]: Rate,=K[A]^2[B]^2. what are the units of k for this reaction? If the concentration of air decreases by a factor of 2 and the concentration of b increases by a factor of 5 what happens to the rate? 2. for the forward reaction 2NO+Cl2=>2NOCl. determine the rate(m/s)for experiment #4 given [NO]°(M)=0.40M and [Cl2]°z(M)=0?20M. Rate? 3.The following data were collected over time for the forward reaction 2NO2=>2NO+O2 ( 1/[NO2]=100 at 0...
18. From the reaction data below, determine whether the reaction is first-order or second-order. Time (S) Reactant (M) 6.67 1.59 0.74 0.39 0.16 25 a. First-order. b. Second-order. c. Zero-order. d. Cannot determine. 19. In the Question 18, what is the rate constant for the reaction? a. 0.12 b. 0.15 c. 0.24 d. 0.72 20. In the Question 18, what is the half-life for the reaction? a. 0.2 sec b. 0.6 sec c. 1.0 sec d. 1.3 sec
s ) at 650 K and a 18. For a certain second order reaction, the rate constant has a value of 0.22 ( M value of 23 at 800 K. Calculate the activation energy (in kJ/mole) for this reaction. (A) 84 (B) 134 (C) 42 (D) 107 (E) 63
+ Half-life for First and Second Order Reactions 11 of 11 The half-life of a reaction, t1/2, is the time it takes for the reactant concentration A to decrease by half. For example, after one half-Me the concentration falls from the initial concentration (Alo to A\o/2, after a second half-life to Alo/4 after a third half-life to A./8, and so on. on Review Constants Periodic Table 11/25 For a second-order reaction, the half-life depends on the rate constant and the...
The following reaction is second order in [A] and the rate constant is 0.025 M-1s-1: The concentration of A was 0.65 M at 33 s. The initial concentration of A was ________ M. Select one: a. 0.24 b. 1.2 � 10-2 c. 0.27 d. 2.4 e. 1.4
The reaction 2HI → H2 + I2 is second order in [HI] and second order overall. The rate constant of the reaction at 700°C is 1.57 × 10−5 M −1s−1. Suppose you have a sample in which the concentration of HI is 0.75 M. What was the concentration of HI 8 hours earlier? A) 0.45 M B) 0.75 M C) 2.3 M D) 1.9 M
1. A reaction was shown to follow second-order kinetics. How much time is required for [A] to change from 0.500 M to 0.160 M? (k = 0.456 M⁻¹ s⁻¹) 2. A substance decomposes with a rate constant of 9.05 × 10⁻⁴ s⁻¹. How long does it take for 16.0% of the substance to decompose? 3. How long will it take for the concentration of A to decrease from 0.500 M to 0.100 M in the first-order reaction A → B?...
Question 6 (5 points) A reaction that is second order in a single reactant has an initial concentration of 0.910 M and a rate constant of 0.441 M-18-1. What is the concentration of this reactant at 94.0 s? 0.00907 M 0.157 M 0.420 M 0.365 M 0.0235 M
9. For second-order reactions the slope of a plot of 1A versus time is b. KTA kt ch 10. If the reaction 2A + 3D products is first order in A and second-order in D. then the rate law will have the form rate- a. K[ALDI KADC KIAFDd. KIAD 11. In the first-order reaction products, the initial concentration of AIN 1.56 M and the concentration is 0.869 M after 48.0 min. What is the value of the route constant, k....