Question

1.) Consider the reaction of peroxydisulfate ion (S2O2−8) with iodide ion (I−) in aqueous solution:

S2O2−8(aq)+3I−(aq)→2SO2−4(aq)+I−3(aq).
What is the rate of disappearance of I− when [S2O2−8]= 3.5×10⁻² M and [I−]= 5.5×10⁻² M ?

2.) Consider the reaction

2H3PO4→P2O5+3H2O

Using the information in the following table, calculate the average rate of formation of P2O5 between 10.0 and 40.0 s.

Time (s)010.0, 20.0, 30.0, 40.0, 50.0[P2O5] (M)02.20×10^−3, 5.20×10^−3, 7.00×10^−3, 8.20×10^−3, 8.80×10⁻³

3.) The reactant concentration in a second-order reaction was 0.470 M after 190 s and 8.20×10⁻²M after 825 s . What is the rate constant for this reaction?

4.) A certain reaction with an activation energy of 115 kJ/mol was run at 555 K and again at 575 K . What is the ratio of f at the higher temperature to f at the lower temperature?

Answer 1