By convention, the rate of the reaction is always positive and should be the same regardless of the chemical species monitored. For the H2O2 decomposition reaction, the rate of the reaction is therefore defined as
Rate of the reaction = -1/2 (?[H2O2]/?t) = ?[O2]/?t (in units of solution molarity).
Suppose you carried out the decomposition reaction using 25.0 mL reaction solution (i.e. 15.0 mL of a 6.0% hydrogen peroxide and 10.0 mL of there reactants or solvent) and obtained the following results: a pressure change of 0.050 atm was observed over a period of 12 seconds, and the temperature was constant at 23.1° C.
A. How many moles of oxygen gas are produced in 12 seconds? (You will want to use your conversion factor from question #1.)
B. What would be the concentration of oxygen if the gas had remained in the solution?
C. Base on the above data, what is the rate of the reaction (in units of solution molarity per second)?