2. Hydrogen peroxide, H202 decomposes according the following reaction: 2 H2O2(a

Question

2. Hydrogen peroxide, H202 decomposes according the following reaction: 2 H2O2(aq) 2 H2O(g) O2(g) > + The following were collected during a study of its decomposition at a certain temperature: time (sec) 0.100 0.088 0.0700 0.051 0.025 0.006 120 300 uest 600 1200 2400 Graph the concentration and time data to determine the order of the reaction with respect to hydrogen peroxide. Explain your reasoning and work. Nhen graphing the deta, yon get dine. By Write a rate law for this reaction, assuming that the products do not affect the rate of the reaction, and determine a rate constant with appropriate units a. a, yon get curved line. Buunewetn take h b. Wrte arate law for this reacion, ássuming that the products do not affect the rate b. Caculate ine half-life of the reaction C. d. Predict the concentration of hydrogen peroxide at a time of 8 mins

Explanation / Answer

The analysis can be done by integral method of analysis by assuming an order. To begin with Zero order, does not fit since the rate depends on time ( for zero order reaction rate is independent of concentration)

for a first order reaction lnC= lnCo-Kt

where Co = initial concentration and C= Concentration at any time T

so a plot of lnC vs time gives a straight line whose slope is -K and initial concentration is intercept. The plot is show below.

The slope is -K= -0.001sec-1 , K= 0.001/sec and lnCo= -2.292, Co =0.10. So it is first order.

B)Rate law -r= 0.001[H2O2]

C) For first oder reaction, half life= 0.693/K =0.693/0.001=693 sec

d) after 8 minutes, 480 sec lnC= ln(0.1)-0.001*480, C=0.062M

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