Potentially Useful Reference Information-EaJR = 8.314k = A· e RTmol·KCalculate the rate constant (k) for a reaction where a 0.1 M first order reactant and a0.3 M second order reactant result in a rate of 4.5 x 103 M/sec.Report your answer with one significant figure; you do not need to include any units,just the value of k.The molarities given are the initial concentrations for each reactant.

rate = 4.5 X 10-3 M/sec Concentration of A = 0.1 M Concentration of B = 0.3 M

-Ea J R = 8.314 k = A·e RT mol·K Calculate the rate constant (k) for a reaction where a 0.1 M first order reactant and a 0.3 M second order reactant result in a rate of 4.5 x 10³ M/sec. Report your answer with one significant figure; you do not need to include any units, just the value of k. The molarities given are the initial concentrations for each reactant.

-Ea J R = 8.314 k = A·e RT mol·K Calculate the rate constant (k) for a reaction where a 0.1 M first order reactant and a 0.3 M second order reactant result in a rate of 4.5 x 10³ M/sec. Report your answer with one significant figure; you do not need to include any units, just the value of k. The molarities given are the initial concentrations for each reactant.

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

3
In a kinetic experiment with multiple reactants, the general form of the rate law is Rate = k[A]*[B]" To study the order of each reactant, you add a large excess of one reactant, A, and plot the concentration of the other, B, over time. From the plot, you determine that the rate law is first order with respect to B. You then repeat the experiment with a different concentration of A, resulting in this data table. Trial k from Slope [A], (M) [B], (M) 1 0.16 0.200 0.00200 0.32 0.400 0.00200 What is the order of the rate law with respect to A?
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0076 M-s -1. 2 HI (g) → H₂(g) + 1₂ (8) Suppose a 4.0 L flask is charged under these conditions with 500. mmol of hydrogen iodide. After how much time is there only 250. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 00 X
Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. NO, (g) + CO(g) → NO(g) + CO,(g)
Consider the following reaction: 2NO(g) + 2H₂(g)→N2 (g) + 2H₂O(g). If the rate constant for this reaction at 1000 K is 6.0 × 104 M-2-¹, what is the reaction rate when [NO] = 3.30x10-² M and [H₂] 2.00×10-² M? Express your answer using two significant figures. rate= Submit Part C ΫΠ ΑΣΦ rate = Request Answer ? What is the reaction rate at 1000 K when the concentration of NO is increased to 0.12 M while the concentration of H₂ is 2.00×10-² M? Express your answer using two significant figures. IVE ΑΣΦ M/S ? M/s =
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0084 M's : 2 HI (g) → H, (g) + I, (g) Suppose a 2.0 L flask is charged under these conditions with 100. mmol of hydrogen iodide. How much is left 1.0 s later? You may assume no other reaction is important. olo Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 18 Ar x10
The rate expression for a particular reaction is rate = k[A][B]2. If the initial concentration of B is increased from 0.1 M to 0.3 M, the initial rate will increase by which of the following factors?
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0032 M's ¹: → 3H2(g) → 2 NH3 (g) N2(g) +3H₂ (g) Suppose a 450. mL flask is charged under these conditions with 350. mmol of ammonia. How much is left 60. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0025 M.s¹: 2 HI(g) → H₂(g) +1₂ (8) Suppose a 500. mL flask is charged under these conditions with 450. mmol of hydrogen iodide. How much is left 90. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. 0 X x10
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0076 M•s *: 2 NH, (g) → N2 (g) + 3 H, (g) Suppose a 5.0 L flask is charged under these conditions with 500. mmol of ammonia. How much is left 3.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10
Please answer the question
Chlorine dioxide, CIO₂, is a reddish-yellow gas that is soluble in water. In basic solution it gives CIO3 and ClO₂ ions. 2 CIO₂(aq) + 2 OH(aq) → CIO3(aq) + ClO₂ (aq) + H₂O(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO₂ was determined. Use the data here to determine the order of the reaction for CIO₂ and OH, and the value of the rate constant. [CIO2]init [OH Jinit Initial Rate, mol/(Los) Exp. 1 0.030 Exp. 2 0.060 Exp. 3 0.030 Order for CIO₂: Order for OH": Rate constant = 0.030 0.030 0.060 0.0062 0.0248 0.0124