Question

At 40°C, H2O2(aq) will decompose according to the following reaction: 2H2O2(aq) ---> 2H2O(l) + O2(g). The following data were collected for the concentration of H2O2 at various times. Time: H2O2 (mol/L) 0 1.100 2.53 x 10^4 0.488 5.06 x 10^4 0.217 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.53 x 10^4 s. (Use this rate to calculate the average rate of production of O2(g) over the same time period.) b. What are these rates for the time period 2.53 x 10^4 s to 5.06 x 10^4 s? 2. A certain first-order reaction is 54% complete in 85 s. What are the values of the rate constant and the half-life for this process?

          At 40°C, H2O2(aq) will decompose according to the following reaction: 2H2O2(aq) ---> 2H2O(l) + O2(g). The following data were collected for the concentration of H2O2 at various times.

Time:               H2O2 (mol/L) 
0                 1.100
2.53 x 10^4       0.488
5.06 x 10^4       0.217

a. Calculate the average rate of decomposition of H2O2 between 0 and 2.53 x 10^4 s. (Use this rate to calculate the average rate of production of O2(g) over the same time period.)

b. What are these rates for the time period 2.53 x 10^4 s to 5.06 x 10^4 s?

2. A certain first-order reaction is 54% complete in 85 s. What are the values of the rate constant and the half-life for this process?

Added by Brian H.

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