The table below gives concentrations of reactants and productsas a function of t

Question

The table below gives concentrations of reactants and productsas a function of time for the following reaction at 55°C:
2 N2O5 (g) 4 NO2 (g) +O2 (g) Use this Rate constant =-0.001697033
Time(s) Concentration(M)
[N2O5]
0 0.0200
100 0.0169
200 0.0142
300 0.0120
400 0.0101
500 0.0086
600 0.0072
700 0.0061
a) Estimate the half life for the decomposition of gaseousN2O5 at 55 degrees C based on the[N2O5] vs. Time data. b) Use this Rateconstant = -0.001697033 Calculate the half-life from the rate constant givenabove. c) If the initial concentration of N2O5is 0.020M, what is the concentration of N2O5after 5 half-lives? d) How long will it take for N2O5concentration to fall to 12.5 % of its initial value?
The table below gives concentrations of reactants and productsas a function of time for the following reaction at 55°C:
2 N2O5 (g) 4 NO2 (g) +O2 (g) Time(s) Concentration(M)
[N2O5]
0 0.0200
100 0.0169
200 0.0142
300 0.0120
400 0.0101
500 0.0086
600 0.0072
700 0.0061
a) Estimate the half life for the decomposition of gaseousN2O5 at 55 degrees C based on the[N2O5] vs. Time data. b) Use this Rateconstant = -0.001697033 Calculate the half-life from the rate constant givenabove. c) If the initial concentration of N2O5is 0.020M, what is the concentration of N2O5after 5 half-lives? d) How long will it take for N2O5concentration to fall to 12.5 % of its initial value? Calculate the half-life from the rate constant givenabove. c) If the initial concentration of N2O5is 0.020M, what is the concentration of N2O5after 5 half-lives? d) How long will it take for N2O5concentration to fall to 12.5 % of its initial value?
Time(s) Concentration(M)
[N2O5]
0 0.0200
100 0.0169
200 0.0142
300 0.0120
400 0.0101
500 0.0086
600 0.0072
700 0.0061

Explanation / Answer

We Know that :       The given Reaction is:
          2N2O5 (g) 4 NO2 (g) +O2 (g)           From the data provided it is clear that thedecomposition of N2 O5 follows First - order Kinetics.              We Know that :                    T1/2 = 0.693 / K                             = 0.693 / 0.001697033 s-1                              = 408.359 s.            [N2 O5 ]   =   1/ 25   x intial concentrationof N2O5                              = 1 / 32 x 0.020 M                               = 0.000625 M             t = 2.303 / K log [ 0.020 M ] / [ 0.0025 M ]                 = 2.303 / 0.0016970 s -1 log [ 0.020 M] / [ 0.0025 M ]                = 1225.8 sec.                                 = 1 / 32 x 0.020 M                               = 0.000625 M             t = 2.303 / K log [ 0.020 M ] / [ 0.0025 M ]                 = 2.303 / 0.0016970 s -1 log [ 0.020 M] / [ 0.0025 M ]                = 1225.8 sec.                     

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.