The reactions in the table are all zero order and follow the same general reaction process of A products. Half-life, 11/2 (s) Rate constant, k (M · s-1) Initial concentration, [A]o (M) Reaction 1 5.51 0.0671 Reaction 2 ? 0.0451 0.851 Reaction 3 5.31 ? 0.411 Reaction 4 4.91 0.0411 ? Reaction 5 4.11 0.611 Calculate the missing values for half-life (t1/2), rate constant (k), and initial concentration, [A]o. reaction 1 initial concentration, [A]o: M reaction 2 half-life, t12: reaction 3 rate constant, k: M.s-1 reaction 4 initial concentration, [A]o: M reaction 5 rate constant, k: M. s-1

The reactions in the table are all zero order and follow the same general reaction process of A products. Half-life, 11/2 (s) Rate constant, k (M · s-1) Initial concentration, [A]o (M) Reaction 1 5.51 0.0671 Reaction 2 ? 0.0451 0.851 Reaction 3 5.31 ? 0.411 Reaction 4 4.91 0.0411 ? Reaction 5 4.11 0.611 Calculate the missing values for half-life (t1/2), rate constant (k), and initial concentration, [A]o. reaction 1 initial concentration, [A]o: M reaction 2 half-life, t12: reaction 3 rate constant, k: M.s-1 reaction 4 initial concentration, [A]o: M reaction 5 rate constant, k: M. s-1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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 0.240 0.220 0.0170 2 0.240 0.440 0.0170 3 0.480 0.220 0.0680 k=?
Methyl acetate (CH3COOH3) reacts with water in the presence of an acid to produce methanol and acetate as described in the following equation: CH3COOH3(g) + H2O(g) → CH3OH(g) + CH3COOH(g). The reaction is first order with a rate constant of 1.26 x 10-4/s at 25oC. How long will it take for the reaction to produce 65.0% product?
The hydrolysis of cisplatin is a first order reaction. Given that k = 2.50 x 10-5 s-1, what is the half-life of the reaction? If the initial concentration of cisplatin is 0.00225 M, what is the concentration of cisplatin after one half- life?
Cyclobutane, C4H8, consisting of molecules in which four carbon atoms for a ring, decomposes when heated to give ethylene. C4H8(g) → 2C2H4(g) The reaction is first order. In an experiment, the initial concentration of cyclobutane was (3.500x10^-3) M. After heating at 450 °C, for (5.55x10^2) s, this was reduced to (2.6090x10^-3) M. What was the concentration of cyclobutane after a total of (1.008x10^3) s? Express your answer to three significant figures. Just enter the number (e.g. 2.48x10^-4) and the unit.
The following initial rate data was obtained for the reaction between oxygen and nitric oxide. 2 NO(g) + O2(g) → 2 NO2(g) [O2] (M) [NO] (M) Rate (M s 1) 0.0100 0.0100 10.0 0.0150 0.0100 22.5 0.0150 0.0200 45.0 What is the rate law for this reaction under these conditions? Rate = k [O2] [NO]2 Rate = k [O2]2 [NO]2 Rate = k [O2] [NO] Rate = k [O2]² [NO]
Determine half-life, order, and k from concentration-time data. The following data were collected for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g)-CH₂(g) + H₂(g) + CO(g) [CH3OCH 3], M 7.02x10-² time, min 0 3.51x10-2 22.20 K 1.76x10-² 44.40 8.80×10-3 66.60 (a) What is the half-life for the reaction when [CH3OCH3] = 7.02x10-² M? (b) What is the half-life for the reaction when [CH3OCH3] = 3.51x10-² M? (c) Is the reaction first order? If so, what is the rate constant for the reaction? (If not first order leave blank). min min min-1
The reaction A → B + C is known to be zero order in A with a rate constant of 5.2 × 10–2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 3.2 × 10–3 M. What is the half-life for the reaction? A) 1.3× 101 s B) 2.6× 10–2 s C) 8.3× 10–2 s D) 6.0× 104 s E) 3.1× 10–2 s
What is the half life of the following reaction, given the following set of conditions (Hint: observe the units for the rate constant to determine the order of the reaction!): 2 HI (g) → H2 (g) + I2 (g) Initial concentration of HI = 1.00 M k = 1.2 x 10-3 M-1 s-1
A certain first order reaction has k = 2.51 s-1 . If the initial concentration of the reactant is 6.50 M, how much will be left after two half lives (in M)? Give your answer to three sig figs
The gas phase decomposition of hydrogen iodide at 700 K HI(g)- →½ H2(g) + ½ I2(g) is second order in HI. In one experiment, when the initial concentration of HI was 2.23 M, the concentration of HI dropped to 0.656 M after 591 seconds had passed. Based on these data, the rate constant for the reaction is M-1 s-1.
Experimental data for the reaction A + 2B → C have been plotted in the following three different ways. 0.05 -3.0 0.04 0.03 0.02 0.01 0 IvI 0 2 Time (s) 1/[A] 100 80 40 20 0 In[A] -3.5 -4.0 -4.5 -5.0 0 2 Time (s) 2 Time (s) What is the order of the reaction, and what was the initial concentration of A? O first-order, initial concentration = 10 M second-order, initial concentration = 10 M zero-order, initial concentration = 10 M O second-order, initial concentration = 0.1 M O first-order, initial concentration = 0.1 M
b The half-life of a reaction, t1/2t1/2, is the time it takes for the reactant concentration [A][A] to decrease by half. For example, after one half-life the concentration falls from the initial concentration [A]0[A]0 to [A]0/2[A]0/2, after a second half-life to [A]0/4[A]0/4, after a third half-life to [A]0/8[A]0/8, and so on. on.