Part a Rate of reaction with respect to N2O5 -r N2O5 = - d[N2O5] / dt = k [N2O5]

Question

Part a

Rate of reaction with respect to N2O5

-rN2O5 = - d[N2O5] / dt = k [N2O5]2

Negative Sign shows the decomposition of N2O5

Rate of reaction with respect to NO2

rNO2 = d[NO2] / dt = k [N2O5]2

Rate of reaction with respect to O2

rO2 = d[O2] / dt = k [O2]2

Relation between rate of reaction of products and reactants

-rN2O5 / 2 = rNO2 / 4 = rO2 / 1

-rN2O5 = 0.50 rNO2 = 2 rO2

k [N2O5]2 = 0.50 k [N2O5]2 = 2k [N2O5]2

Part b

i) decomposition rate of N2O5 at 200 s

= (0.0142 - 0.02)M/(200 - 0)s

= - 2.9*10-5 M/s

decomposition rate of N2O5 between 300s and 500 s

= (0.0086 - 0.012)M/(500 - 300)s

= - 1.7*10-5 M/s

ii) formation rate of NO2

= (0.0256 - 0.0160)M / (600 - 300)s

= 3.2*105 M/s

iii) formation rate of O2

= (0.0057 - 0)M / (500 - 0)s

= 1.14*105 M/s

Explanation / Answer

Consider the decomposition of No, to give NO, and O, 2N205(g) 4NO2(g) + 02(g) The concentration of each gas is given as: Time Concentration (M) NO NO2 100 200 300 400 500 600 700 0.0200 0.0169 0.0142 0.0120 0.0101 0.0086 0.0072 0.0061 0.0063 0.0115 0.0160 0.0197 0.0229 0.0256 00278 00016 : 0.0029 0:0040 0.0049 00057 0.0064 0.0070

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