At 40 C H2O2(aq) will decompose according to the followingreaction: 2H2O2 (aq) -
ID: 678199 • Letter: A
Question
At 40 C H2O2(aq) will decompose according to the followingreaction: 2H2O2 (aq) -----> 2H2O (l) + O2 (g)The following data were collected for the concentration ofH2O2 at various times:
Time (s) H2O2 (mol/L) 0 1.000 2.16 x 104 0.500 4.32 x 104 0.250
a) calculate the average rate of decomposition of H2O2 between0 and 2.16 x 104 s. Use this rate to calculate the averagerate of production of O2 (g) over the same time period.
b) what are these rates for the time period 2.16 x 104 s to4.32 x 104 s ?
Show all work please 2H2O2 (aq) -----> 2H2O (l) + O2 (g)
The following data were collected for the concentration ofH2O2 at various times:
Time (s) H2O2 (mol/L) 0 1.000 2.16 x 104 0.500 4.32 x 104 0.250
a) calculate the average rate of decomposition of H2O2 between0 and 2.16 x 104 s. Use this rate to calculate the averagerate of production of O2 (g) over the same time period.
b) what are these rates for the time period 2.16 x 104 s to4.32 x 104 s ?
Show all work please
Explanation / Answer
From the equation , Rate law is -1/2 [H2O2] / t = 1/2 [H2O] /t = [O2] / t . a ) Average rate of decomposition = - ( 0.5 - 1 ) mol / L / 2* 2.16 x 104 s.- 0 s = 0.5 mol / L /2* 2.16 x 104 s = 0.11 * 10 ^ -4 mol / L.s = 1.1 * 10 ^ -5 mol / L.s Average rate of production of O2 (g ) = 2 * Average rate of decomposition ofH2O2 = 2 * 1.1 * 10 ^ -5 mol / L.s = 2.2 * 10 ^ -5 mol /L.s b) Average rate of decomposition = - ( 0.250 - 0.5 ) mol / L / 2( 4.32*10^4- 2.16 x 104 s ) = 0.0578 * 10 ^ -4 mol / L.s = 5.78 * 10 ^ -6 mol / L.s Average rate of production of O2 (g ) = 2 * 5.78 *10 ^ -6 mol / L.s =11.56 * 10 ^ -6 mol / L.sRelated Questions
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