Need help with 1 and 2 please! Rate law, order, and decomposition rate For the f

Question

Need help with 1 and 2 please! Rate law, order, and decomposition rate For the following reaction, a series of four experiments were performed. From calculate (a) the complete rate law, (b) ORDER of the reaction , (c) individual 1. H2O2 +31. +2H+ = 13. + 2H20 Experiment H202] Initial rate, Mis 0.010 2 3 0.010 0.00050 1.15 x 106 0.00050 2.30x10-6 0.020 0.010 0.010 0.010 0.02022 0.00050 2.30 x 106 0.010 0.00100 1.15x 10* 4 2. Calculate the average rate of decomposition of N20s 2N2Os = 4NO2 + O2 Time, s [N205] 600 1.24 x 102 0.93 x 102 1200

Explanation / Answer

2) The given reaction is---

2N2O5 ---> 4NO2 + O2

Decrease in concentration of N2O5 in 600 s = 1.24 x 10-2 - 0.93 x 10-2 = (1.24 -0.93 ) x 10-2 = 0.31 x 10-2 M

The average rate of decomposition will be---

= moles decomposed/ time taken

=( 0.31 x 10-2 /600) Ms-1

= 5.167 x 10-6 Ms-1

Related Questions

Navigate

• Browse (All)
• Browse N
• Subjects

---