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In 17.5% w/w HCl, the complex ion Ru(NH3)63+ decomposes to a variety of products.  The reaction is first order in [Ru(NH3)63+] and has a half-life of 14 h at 25°C. (a)What is the rate constant for this reaction? (b)Under these conditions, how long will it take for the [Ru(NH3)63+] to decrease to 6.25% of its initial value? What is the rate constant in s-1 for a first order reaction with an initial concentration of a 0.600 mol/L if, after 142 s, the concentration is 0.444 mol/L? What is the half-life in seconds for a second order reaction with the rate constant k = 2.74 x 10-1 L/mole∙s if the initial reactant concentration is 0.500 mol/L?

In 17.5% w/w HCl, the complex ion Ru(NH3)63+ decomposes to a variety of products.  The reaction is first order in [Ru(NH3)63+] and has a half-life of 14 h at 25°C. (a)What is the rate constant for this reaction? (b)Under these conditions, how long will it take for the [Ru(NH3)63+] to decrease to 6.25% of its initial value? What is the rate constant in s-1 for a first order reaction with an initial concentration of a 0.600 mol/L if, after 142 s, the concentration is 0.444 mol/L? What is the half-life in seconds for a second order reaction with the rate constant k = 2.74 x 10-1 L/mole∙s if the initial reactant concentration is 0.500 mol/L?

Chemistry
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...
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    1. In 17.5% w/w HCl, the complex ion Ru(NH3)63+ decomposes to a variety of products.  The reaction is first order in [Ru(NH3)63+] and has a half-life of 14 h at 25°C.
    2. (a)What is the rate constant for this reaction?
    3. (b)Under these conditions, how long will it take for the [Ru(NH3)63+] to decrease to 6.25% of its initial value?

    1. What is the rate constant in s-1 for a first order reaction with an initial concentration of a 0.600 mol/L if, after 142 s, the concentration is 0.444 mol/L?

    1. What is the half-life in seconds for a second order reaction with the rate constant k = 2.74 x 10-1 L/mole∙s if the initial reactant concentration is 0.500 mol/L?
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