± Introduction to Reaction Rates Learning Goal: To calculate average and relativ

Question

± Introduction to Reaction Rates Learning Goal: To calculate average and relative reaction rates. You can measure the rate of a reaction, just like you can measure the speed a jogger runs. While a jogger would be reported to run a specific number of miles in an hour, miles/hour, a reaction is reported to form product or consume reagent in molar concentration per second, M/s. Reaction rate can be defined either as the increase in the concentration of a product per unit time or as the decrease of the concentration of a reactant per unit time. By definition, reaction rate is a positive quantity. In the reaction X2Y, for example, Y is being produced twice as fast as X is consumed and thus rate of X=12(rate of Y) Each rate can be expressed as the change in concentration over the change in time, t: [X]t=12([Y]t)

Part A

Consider the reaction

2H3PO4P2O5+3H2O

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

Express your answer with the appropriate units.

Explanation / Answer

we know that

the average rate is given by

average rate = d[P205] / dt

now

between 10 and 40 s

d[P205] = ( 7.7 x 10-3) - ( 1.7 x 10-3) = 6 x 10-3

dt = 40-10 = 30

so

average rate = 6 x 10-3 / 30

average rate = 2 x 10-4

so

the average rate of formation of P205 between 10 and 40 s is 2 x 10-4 M / s

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