(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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part c?
Transcribed Image Text:15-
2 NO(g) + O2(g) +2 NO2(g)
For the reaction above, the rate constant at 380°C for the forward reaction is 2.6×10³
liter/mole?-sec and this reaction is first order in O2 and second order in NO. The rate constant
for 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 and
calculate 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 0.0060
mole/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 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.
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