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quantum chem
A reaction 2 A rightarrow P has a second-order rate law with k =...
A reaction 2A → P has a second-order rate law with kf = 1.44 dm3 mol-1...
A reaction 2A → P has a second-order rate law with kf = 1.44 dm3 mol-1 s -1 . Calculate the time required for the concentration of A to change from 0.460 mol dm-3 to 0.046 mol dm-3 .
The rate law of a reaction is rate =k[X]³. The units of the rate constant are
1)The rate law of a reaction is rate =k[X]³. The units of the rate constant areL mol-1 s-1mol² L-2 s-1mol L-1S-2L² mol-2 s-1mol L-1S-12)Given the following rate law, how does the rate of reaction change if the concentration of Z is tripled? Rate =k[X]³[Y]²[Z]⁰The rate of reaction will increase by a factor of136803)What data should be plotted to show that experimental concentration data fits a first-order reaction?1 / [reactant] vs. time[reactant] vs. timeln (k) vs. Ealn (k) vs. 1 / Tln [...
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is...
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
The second-order reaction, 2 Mn(CO)_5 rightarrow Mn_2 (CO)_10 is found to have a rate constant equal...
The second-order reaction, 2 Mn(CO)_5 rightarrow Mn_2 (CO)_10 is found to have a rate constant equal to 512 M^-1 S^-1. If the initial concentration of Mn(CO)_5 is 0.011 M, how long will it take for the reactant concentration to reach 0.0011 M? Units: s a. 1.6 b. 5.1 c. 0.020 d. 0.28 A plot of a 1/[A] versus time gave a straight line. This indicates that A rightarrow B + C a. the reaction is zero order in reagent A...
The reaction NO(g) + 7/2 Cl_2(g) rightarrow NOCl(g) is first-order in [Cl2] and second order with...
The reaction NO(g) + 7/2 Cl_2(g) rightarrow NOCl(g) is first-order in [Cl2] and second order with respect to [NO]. Under a given set of conditions, the initial rate of this reaction is 6.20 times 10^-6 mol/L s. What is the rate of this reaction if the concentration of NO is doubled and the concentration of Cl_2 is reduced to half the original value? 6.20 times 10^-6 mol/L s 2.48 X 10_5 mol/L s 1.24 times 10^-5 mol/L s 4.96 times...
For the reaction: A rightarrow B + C and a Rate Law of: Rate = k...
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
1. A reaction is second order in[A] and second-order in [B]: Rate,=K[A]^2[B]^2. what are the units...
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...
Be sure to answer all parts. The reaction 2A rightarrow B is second order in A...
Be sure to answer all parts. The reaction 2A rightarrow B is second order in A with a rate constant of 32.1 M^-1 s^-1 at 25 degree C. Starting with [A]0 = 0.00779 M, how long will it take for the concentration of A to drop to 0.001803M? s Calculate the half-life of the reaction for [A]_0 = 0.00779 M. s Calculate the half-life of the reaction for [A)0 = 0.00269 M.
The rate law for the decomposition of N2O5 is rate = k[N2O5] If k = 1.0...
The rate law for the decomposition of N2O5 is rate = k[N2O5] If k = 1.0 x 10-5 s-1, what is the reaction rate when the N2O5 concentration is 0.0091 mol L-1? 2.The decomposition of acetaldehyde, CH3CHO, was determined to be a second order reaction with a rate constant of 0.0771 M-1 s-1. If the initial concentration of acetaldehyde is 0.301 M , what will the concentration be after selected reaction times? a. What will the CH3CHO concentration be after...
1. Derive the second order rate law for the reaction 2 A →P, and an expression...
1. Derive the second order rate law for the reaction 2 A →P, and an expression for its half life, t 1/2, in terms of the initial concentration of A. State your assumptions and show each step. [See Atkins 10th ed, 20B2; Atkins 11th ed, 17B2]
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
The second-order reaction, 2 Mn(CO)_5 rightarrow Mn_2 (CO)_10 is found to have a rate constant equal to 512 M^-1 S^-1. If the initial concentration of Mn(CO)_5 is 0.011 M, how long will it take for the reactant concentration to reach 0.0011 M? Units: s a. 1.6 b. 5.1 c. 0.020 d. 0.28 A plot of a 1/[A] versus time gave a straight line. This indicates that A rightarrow B + C a. the reaction is zero order in reagent A...
The reaction NO(g) + 7/2 Cl_2(g) rightarrow NOCl(g) is first-order in [Cl2] and second order with respect to [NO]. Under a given set of conditions, the initial rate of this reaction is 6.20 times 10^-6 mol/L s. What is the rate of this reaction if the concentration of NO is doubled and the concentration of Cl_2 is reduced to half the original value? 6.20 times 10^-6 mol/L s 2.48 X 10_5 mol/L s 1.24 times 10^-5 mol/L s 4.96 times...
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
Be sure to answer all parts. The reaction 2A rightarrow B is second order in A with a rate constant of 32.1 M^-1 s^-1 at 25 degree C. Starting with [A]0 = 0.00779 M, how long will it take for the concentration of A to drop to 0.001803M? s Calculate the half-life of the reaction for [A]_0 = 0.00779 M. s Calculate the half-life of the reaction for [A)0 = 0.00269 M.
1. Derive the second order rate law for the reaction 2 A →P, and an expression for its half life, t 1/2, in terms of the initial concentration of A. State your assumptions and show each step. [See Atkins 10th ed, 20B2; Atkins 11th ed, 17B2]
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