Homework 1.1

Homework 1.1 - 2 O 5 What will be the pressure initially...

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HOMEWORK 1.1 22.2b   The rate of consumption of B in the reaction A + 3 B   C + 2 D is 1.0 mol dm −3  s −1 . State the  reaction rate, and the rates of formation or consumption of A, C, and D. 22.4b   The rate law for the reaction in Exercise 22.2b was reported as d[C]/d t = k [A][B][C] −1 . Express  the rate law in terms of the reaction rate; what are the units for  k  in each case? 22.5b   At 400 K, the rate of decomposition of a gaseous compound initially at a pressure of 12.6  kPa, was 9.71 Pa s −1  when 10.0 per cent had reacted and 7.67 Pa s −1  when 20.0 per cent had  reacted. Determine the order of the reaction. 22.7a   The rate constant for the first-order decomposition of N 2 O 5  in the reaction 2 N 2 O 5 (g)   4  NO 2 (g) + O 2 (g) is  k  = 3.38 × 10 −5  s −1  at 25°C. What is the half-life of N
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Unformatted text preview: 2 O 5 ? What will be the pressure, initially 500 Torr, at (a) 10 s, (b) 10 min after initiation of the reaction? 22.8a A second-order reaction of the type A + B → P was carried out in a solution that was initially 0.050 mol dm −3 in A and 0.080 mol dm −3 in B. After 1.0 h the concentration of A had fallen to 0.020 mol dm −3 . (a) Calculate the rate constant. (b) What is the half-life of the reactants? 22.1 The data below apply to the formation of urea from ammonium cyanate, NH 4 CNO → NH 2 CONH 2 . Initially 22.9 g of ammonium cyanate was dissolved in enough water to prepare 1.00 dm 3 of solution. Determine the order of the reaction, the rate constant, and the mass of ammonium cyanate left after 300 min....
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This note was uploaded on 05/01/2011 for the course CHEM 345 taught by Professor Cardelino during the Fall '09 term at Spelman.

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