Q. 205.0( 1 Vote )

# The following dat

2 N2O5(g)2 N2O4 + O2(G)

GIVEN,

At t = 0 0. 5 atm 0 atm 0 atm

At time t 0. 5 - 2x atm 2x atm x atm

To find total pressure:

Pt = sum of partial pressures of all reactants and products

Pt = 0. 5 - 2x + 2x + x

x = pt - 0. 5

p = 0. 5 - 2x

= 0. 5 - 2(pt - 0. 5)

= 1. 5 - 2pt

At t = 100 s ;pt = 0. 512 atm

p = 1. 5 - 20. 512 = 0. 476 atm

Formula to find rate constant of a first order reaction

k = log

k = log

k = 0. 0216 = 4. 9810 - 4 s – 1

conclusion

the rate constant for the following reaction is 4. 9810 - 4 s - 1

OR

Given:

Difference between activation energies = 24. 9 kJ/mol

The Arrhenius equation:

take log on both sides, log k = log (Ae-Ea)

log k = log A -

LETS ASSUME,

For reaction 1 log k1 = log A -

For reaction 2 log k2 = log A -

Subtract 1 from 2

Conclusion:

Ratio between rate constants = 2. 198 4

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