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Chap14_Part2 - 1 Concentra)onandRate NH4(aq NO2(aq)N2(g...

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Concentra)on and Rate: NH 4 + ( aq ) + NO 2 ( aq ) N 2 (g) + 2 H 2 O( l ) (a) These data are ini7al rates. (b) For constant NO 2 , the rate is propor7onal to the NH 4 + concentra7on. (c) For constant NH 4 + , the rate is propor7onal to the NO 2 concentra7on. Rate = k [ NH 4 + ][ NO 2 ] k = propor7onality constant 2
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Rate = k [ NH 4 + ][ NO 2 ] From the table, Ini7al rate = 5.4 X 10 ‐7 M/s [NH4] + = 0.0100 M [NO2] = 0.200 M 5.4X10 ‐7 M/s "What frac7on of the molecules in the origina7ng compartment is travelling via this process per unit 7me”‐ Rate constant [0.01 M] [0.20M] = 2.7 X 10 ‐4 M ‐1 s ‐1 k = Once we have both rate law and rate constant for a reac7on, we can calculate the rate of a reac7on fro any set of concentra7ons. 3
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Using the table 14.2, determine the rate law, rate constant and rate of the reac7on when the concentra7ons of both reactants raised to [0.1M] Rate = k [ NH 4 + ][ NO 2 ] k = 2.7X10 ‐4 M ‐1 s ‐1 (See previous slide) 4
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Using the table 14.2, determine the rate law, rate constant and rate of the reac7on when the concentra7ons of both reactants raised to [0.1M] Rate = k [ NH 4 + ][ NO 2 ] k = 2.7X10 ‐4 M ‐1 s ‐1 Rate = [2.7 X 10 ‐4 M ‐1 s ‐1 ][0.10M] [0.10M] = 2.7 X 10 ‐6 M/s 5
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(a) The rate law is (b) The rate depends only on the reactant concentra7ons. (c) The propor7onality constant k is called the rate constant . (d) The values of m and n are usually small integers . Rate Laws Consider a general reac7on with two reactants and two products: dD cC bB aA + + Rate = k [ A ] m [ B ] n 6
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Exponents in the Rate Laws Rate = k [ A ] m [ B ] n [ C ] p ... The exponents are called reac7on orders . This reac7on is mth order in [A] nth order in [B] pth order in [C] The overall reac7on order is m + n + p + … The reac7on orders must be determined experimentally.
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