Suppose a 500. mL flask is filled with 0.40 mol of N, and 0.10 mol of 0,. The followingreaction becomes possible:N, (g) + 0,(g) – 2NO(g)The equilibrium constant K for this reaction is 5.29 at the temperature of theflask.Calculate the equilibrium molarity of N,. Round your answer to two decimalplaces.OM

The equilibrium reaction given is, Given: Initial moles of N2 taken = 0.40 mol. Initial moles of O2…

Answered: Suppose a 500. mL flask is filled with…

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

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Suppose a 500. mL flask is filled with 0.40 mol of N, and 0.10 mol of 0,. The following
reaction becomes possible:
N, (g) + 0,(g) – 2NO(g)
The equilibrium constant K for this reaction is 5.29 at the temperature of the
flask.
Calculate the equilibrium molarity of N,. Round your answer to two decimal
places.
OM

Expert Solution

Step 1

The equilibrium reaction given is,

Given: Initial moles of N₂ taken = 0.40 mol.

Initial moles of O₂ taken = 0.10 mol.

Volume of vessel = 0.500 L = 500 mL (Since 1 L = 1000 mL)

And the equilibrium constant of the reaction is 5.29.

$S i n c e c o n c e n t r a t i o n = \frac{M o l e s}{V o l u m e o f s o l u t i o n i n L} = > I n i t i a l c o n c e n t r a t i o n o f N_{2} = \frac{0.40}{0.50} = 0.80 M A n d i n i t i a l c o n c e n t r a t i o n o f O_{2} = \frac{0.10}{0.50} = 0.20 M$

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