part c? 15-2 NO(g) + O2(g) +2 NO2(g)For the reaction above, the rate constant at 380°C for the forward reaction is 2.6×10³liter/mole?-sec and this reaction is first order in O2 and second order in NO. The rate constantfor the reverse reaction at 380°C is 4.1 liter/mole-sec and this reaction is second order in NO2.(a) Write the equilibrium expression for the reaction as indicated by the equation above andcalculate the numerical value for the equilibrium constant at 380°C.(b) What is the rate of the production of NO2 at 380°C if the concentration of NO is 0.0060mole/liter and the concentration of O2 is 0.29 mole/liter?(c) The system above is studied at another temperature. A 0.20 mole sample of NO2 is placedin a 5.0 liter container and allowed to come to equilibrium. When equilibrium is reached,15% of the original NO2 has decomposed to NO and O2. Calculate the value for theequilibrium constant at the second temperature.

Equilibrium constant(Kc) is the ratio of concentration of products to the reactants at equilibrium…

(c) The system above is studied at another temperature. A 0.20 mole sample of NO2 is placed in a 5.0 liter container and allowed to come to equilibrium. When equilibrium is reached, 15% of the original NO2 has decomposed to NO and O2. Calculate the value for the equilibrium constant at the second temperature.

(c) The system above is studied at another temperature. A 0.20 mole sample of NO2 is placed in a 5.0 liter container and allowed to come to equilibrium. When equilibrium is reached, 15% of the original NO2 has decomposed to NO and O2. Calculate the value for the equilibrium constant at the second temperature.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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