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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter19: Transitition Metals, Coordination Chemistry And Metallurgy
Section: Chapter Questions
Problem 19.69QE
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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?
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