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Ch.14 - Chemical Kinetics

Chapter 14, Problem 33a

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl- + I- → OI- + Cl- . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4

(a) Write the rate law for this reaction.

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everyone to wear the reaction below. And were given the following data were asked about the right law for the reaction in the term of the units. For the rate constant. Here we're gonna use our right lot equation, which is going to be right people is the rate constant times concentration of a power of X. And X. Is ordered with respect to A times concentration of B. The power of why and why is order with respect to be. We need to first determine the order with respect to A. And B. And to find the right order for A. We're gonna use our 1st and 2nd experiments. 5.0. I'm sensing Megan to smaller per second. Go to the right constant times 0.3 smaller the power of X. Time 0.15 smaller the power of Y. We have 2.5 symptoms of two molar per second equals the right constant $0.15. The power of x times 0.15 Mahler. The power of why. And I'm just gonna cancel out this cancels out as well. Two equals two to the power of X. X equals one A first order and then to find the right order for B. 1st and 3rd experiments, 7.5 Substance and negative to Mueller per second. He goes the rate constant times 0.15 smaller tuatara eggs From 0.45 smaller the power of Y. Then we have 2.5 times two Mueller per second. It was the right concert $0.15. The power of x times 0.15 moller the power of why? So now this cancels out and this as well. Three equals three to the power of Y. Y equals one. The B is also first order R right. Gonna be the rate constant construction of a construction of B in our rate constant into our rate right by the concentration of a last construction update. If we rearrange the equation and for the unit. All right. Is in units of Mueller per second, frustration at A. In consideration of B is in units of Mueller of the right concept. You have more per second. What about muller? I'm smaller to get Baller two megawatt power on second two megawatt power. Thanks for watching my video. And I hope it was up for
Related Practice
Textbook Question

Consider the following reaction: 2 NO1g2 + 2 H21g2¡N21g2 + 2 H2O1g2 (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and 3H24 is increased to 0.030 M?

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Textbook Question

The react ion between ethyl bromide 1C2H5Br2 and hydroxide ion in ethyl alcohol at 330 K, C2H5Br1alc2 + OH- 1alc2¡ C2H5OH1l2 + Br - 1alc2, is first order each in ethyl bromide and hydroxide ion. When 3C2H5Br4 is 0.0477 M and 3OH- 4 is 0.100 M, the rate of disappearance of ethyl bromide is 1.7 * 10-7 M>s. (a) What is the value of the rate constant?

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Textbook Question

The react ion between ethyl bromide 1C2H5Br2 and hydroxide ion in ethyl alcohol at 330 K, C2H5Br1alc2 + OH- 1alc2¡ C2H5OH1l2 + Br - 1alc2, is first order each in ethyl bromide and hydroxide ion. When 3C2H5Br4 is 0.0477 M and 3OH- 4 is 0.100 M, the rate of disappearance of ethyl bromide is 1.7 * 10-7 M>s. (c) How would the rate of disappearance of ethyl bromide change if the solution were diluted by adding an equal volume of pure ethyl alcohol to the solution?

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Textbook Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl - + I - ¡OI - + Cl - . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4

(b) Calculate the rate constant with proper units.

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Textbook Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl- + I- → OI- + Cl- . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4 (c) Calculate the rate when [OCl-] = 2.0 * 10-3 M and [I-] = 5.0 * 10 - 4 M.

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Textbook Question

The following data were measured for the reaction 

(b) What is the overall order of the reaction?

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