Open Question
What is the half-life for this reaction at the initial concentration?
Ch.14 - Chemical Kinetics
Chapter 14, Problem 85
Consider the reaction: A + B + C → D. The rate law for this reaction is: Rate = k [A][C]^2 [B]^1/2. Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 0.0115 M/s. What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled?
Verified step by step guidance1
Identify the given rate law: Rate = k [A][C]^2 [B]^{1/2}.
Note the initial rate of the reaction: 0.0115 M/s.
Determine the effect of doubling the concentration of A: The rate will be multiplied by 2, since the reaction is first order with respect to A.
Determine the effect of doubling the concentration of C: The rate will be multiplied by 2^2 = 4, since the reaction is second order with respect to C.
Determine the effect of tripling the concentration of B: The rate will be multiplied by (3)^{1/2}, since the reaction is half order with respect to B.
Related Practice
Textbook Question
The tabulated data were collected for this reaction at a certain temperature: X2Y → 2 X + Y a. Determine the order of the reaction and the value of the rate constant at this temperature.
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Textbook Question
The tabulated data were collected for this reaction at a certain temperature: X2Y → 2 X + Y c. What is the concentration of X after 10.0 hours?
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Textbook Question
Consider the reaction: 2 O3(g) → 3 O2( g) The rate law for this reaction is: Rate = k [O3]2 [O2] Suppose that a 1.0-L reaction vessel initially contains 1.0 mol of O3 and 1.0 mol of O2. What fraction of the O3 will have reacted when the rate falls to one-half of its initial value?
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Open Question
At 700 K, acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction is: CH3CHO(g) → CH4(g) + CO(g). A sample of CH3CHO is heated to 700 K and the pressure is measured as 0.22 atm before any reaction takes place. The kinetics of the reaction are followed by measurements of total pressure and these data are obtained: t (s) 0 1000 3000 7000; PTotal (atm) 0.22 0.24 0.27 0.31. Find the rate law, the rate constant, and the total pressure after 2.00 × 10^4 s.
Open Question
At 400 K, oxalic acid decomposes according to the reaction: H2C2O4(g) → CO2(g) + HCOOH(g). In three separate experiments, the initial pressure of oxalic acid and the final total pressure after 20,000 seconds are measured. Experiment: 1) PH2C2O4 at t = 0: 65.8, PTotal at t = 20,000 s: 94.6; 2) PH2C2O4 at t = 0: 92.1, PTotal at t = 20,000 s: 132; 3) PH2C2O4 at t = 0: 111, PTotal at t = 20,000 s: 160. Find the rate law of the reaction and its rate constant.