Extra Problems on Kinetics

In the Haber process for the production of ammonia, Problem 1 In the Haber process for the production of ammonia, N2(g) + 3H2(g)  2NH3(g) What is the relationship between the rate of production of ammonia and the rate of consumption of hydrogen?

2N2O5(g)  4NO2(g) + O2(g) At a particular instant rate of (N2O5) = 4.2 x 10−7 mol·L−1·s−1 What are the rates of appearance of NO2 and O2 ?

If, in a certain experiment, over a specific time period, Problem 3. Consider the reaction 4PH3(g)  P4(g) + 6H2(g) If, in a certain experiment, over a specific time period, 0.0048 mol PH3 is consumed in a 2.0-L container each second of reaction, what are the rates of production of P4 and H2 in this experiment?

Initial Rate (mol·L-1·s-1) A + B  C Experiment Number [A] (mol·L-1) [B] (mol·L-1) Initial Rate (mol·L-1·s-1) 1 0.100 4.0 x 10-5 2 0.200 3 1.6 x 10-4 Determine the differential rate law Calculate the rate constant Calculate the rate when [A]=0.050 mol·L-1 and [B]=0.100 mol·L-1

Use the data in table 12.5 to determine 1) The orders for all three reactants 2) The overall reaction order 3) The value of the rate constant

Initial Rate (mol·L-1·s-1) 2NO(g) + 2H2(g)  N2(g) + 2H2O(g) Experiment Number [NO] (mol·L-1) [H2] (mol·L-1) Initial Rate (mol·L-1·s-1) 1 0.10 1.23 x 10-3 2 0.20 2.46 x 10-3 3 4.92 x 10-3 Determine the differential rate law Calculate the rate constant Calculate the rate when [NO]=0.050 mol·L-1 and [H2]=0.150 mol·L-1

Consider the general reaction aA + bB cC and the Sample Problem:. Consider the general reaction aA + bB cC and the following average rate data over some time period Δt: Determine a set of possible coefficients to balance this general reaction.

Problem Reaction: A + B  C obeys the rate law: Rate = k[A]2[B]. A. If [A] is doubled (keeping B constant), how will rate change? B. Will rate constant k change? Explain. C. What are the reaction orders for A & B? D. What are the units of the rate constant?