A proposed mechanism for a reaction is
Write the rate law expected for this mechanism. What is the overall balanced equation for the reaction? What are the intermediates in the proposed mechanism?
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Chemical Principles
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- When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay: HCOOH(g)CO2(g)+H2(g) The rate of reaction is monitored by measuring the total pressure in the reaction container. Time (s) Pressure (torr) 0 220 50 324 100 379 150 408 200 423 250 431 300 435 Calculate the rate constant and half-life in seconds for the reaction. At the start of the reaction (time = 0), only formic acid is present. (HINT: Find the partial pressure of formic acid using Dalton's law of partial pressure and the reaction stoichiometry to find PHCOOH at each time.)arrow_forwardWhen enzymes are present at very low concentration, their effect on reaction rate can be described by first-order kinetics. Calculate by what factor the rate of an enzyme-catalyzed reaction changes when the enzyme concentration is changed from 1.5 107 M to 4.5 106 M.arrow_forwardFor the reaction the rate law is Rate=k[(CH3)3CBr] Identify each mechanism that is compatible with the rate law. (a) (CH3)3CBr (CH3)3C+ + Br slow (CH3)3C+ + OH (CH3)3COH fast (b) (CH3)3CBr + OH (CH3)3COH + Br (c) (CH3)3CBr + OH (CH3)2(CH2)CBr + H2O fast (CH3)2(CH2)CBr (CH3)2(CH2)C + Br slow (CH3)2(CH2)C + H2O (CH3)3COH fastarrow_forward
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