problem solving

Rate Laws / Integrated Rate Laws

K4Fe(CN)6 + H2SO4 + H2O --> K2SO4 + FeSO4 + (NH4)2SO4 + CO

 1.       In the reaction above, the [H2SO4] drops from 1.00M to 0.750M in the first 10 seconds. 

a.       Calculate the average rate of this reaction in this time period. (Balance the equation first)

b.       Calculate the rate of change of [K4Fe(CN)6 ] during this time.

2.       Determine the rate law of the reaction with the following data. Include a value for k. 

2A + B --> C

[A] M       [B] M    Rate

0.10      0.05     0.070

0.20     0.10     0.56

0.10     0.10     0.28

3.       The reaction B --> Products has a rate constant of 0.055 (units left off intentionally). If the reaction mixture is initially 0.75M in B, what is the [B] after 140 seconds if the reaction is: 

a.       First order

b.       Second order

Arrhenius Equations

1.       If a reaction has an activation energy of 45.6 kJ/mole and is initially at a temperature of 25.0C with a rate constant of 0.011 1/s at that temperature, what is the new rate constant if the reaction is warmed to 50.0C? 

2.       If a reaction has a rate constant value of 0.0119 1/s at a temperature of 300K and a rate constant of 0.884 1/s at a temperature of 375K, what is the activation energy?