Question

Question 2 1 pts You will need to generate a set of graphs to answer this question. Concentration vs time data for the following decomposition reaction was collected at 300 K. The data is shown in the table below What is the rate constant for the reaction at this temperature (in units of min )? H2O2(aq) ? H2O(l) + 1/2?2(g) H202lmol/L time (min) 0.0200 0.0118 0.00693 0.00408 0.00240 2000 0.00141 0 500 1000 1500 2500 Question 3 1 pts Sulfuryl chloride, SO2Cl2g) decomposes at high temperature to form SO2(3) and Cl2g). The rate constant at a certain temperature is 4.68 x 10-5s-1. What is the order of the reaction? Enter a number: 0 (for 0 order), 1 for first order), 2, etc.

Answer 1

Answer:

(1) Given reaction H2O2(aq) -----> H2O(i) + 1/2O2(g)

The calculations are shown below,

Time(min)	[H2O2](mol/L)	ln(H2O2)	1/[H2O2](M-1)
0	0.02	-3.91202301	50
500	0.0118	-4.43965575	84.74576271
1000	0.00693	-4.97189547	144.3001443
1500	0.00408	-5.50165829	245.0980392
2000	0.0024	-6.03228654	416.6666667
2500	0.00141	-6.56416557	709.2198582

The plots are shown below

null

From the above plots, ln[H2O2] vs time gave straight line with R2=1.

So the order of reaction is first order and the rate law is

ln[H2O2]= -kt+ln[H2O2]0

the plot ln[H2O2] vs t give slope=rate constant

From the plot, slope=-k=-0.00106 min-1

Therefore rate constant k=1.06x10^-3 min^-1.

(3) Given reaction is SO2Cl2(g) -------> SO2(g) + Cl2(g)

rate constant k=4.68x10^-5 s^-1.

From the unit, we conclude that rate constant is independent of concentration.

so the order of reaction is first order=1.

Thanks and I hope you like it. Please let me know if you have any doubt.