Upon dissolving InCl(s) in HCl, In+(aq) undergoes a disproportionation reaction according to the following unbalanced equation: In+(aq) = In(s) + In3+(aq) This disproportionation follows first-order kinetics with a half-life of 667 s. What is the concentration of In+(aq) after 1.35 h if the initial solution of In+(aq) was prepared by dissolving 2.38g InCl(s) in dilute HCl to make 5.0x10^2 mL of solution? What mass of In(s) is formed after 1.35 h?
Upon dissolving InCl(s) in HCl, In+(aq) undergoes a disproportionation reaction according to the following unbalanced equation: In+(aq) = In(s) + In3+(aq) This disproportionation follows first-order kinetics with a half-life of 667 s. What is the concentration of In+(aq) after 1.35 h if the initial solution of In+(aq) was prepared by dissolving 2.38g InCl(s) in dilute HCl to make 5.0x10^2 mL of solution? What mass of In(s) is formed after 1.35 h?
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Chapter13: Rates Of Reaction
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Problem 13.66QP: In the presence of excess thiocyanate ion, SCN, the following reaction is first order in iron(III)...
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Upon dissolving InCl(s) in HCl, In+(aq) undergoes a disproportionation reaction according to the following unbalanced equation:
In+(aq) = In(s) + In3+(aq)
This disproportionation follows first-order kinetics with a half-life of 667 s.
What is the concentration of In+(aq) after 1.35 h if the initial solution of In+(aq) was prepared by dissolving 2.38g InCl(s) in dilute HCl to make 5.0x10^2 mL of solution? What mass of In(s) is formed after 1.35 h?
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