Consider the following equilibrium: 2NOCl(g) 2NO(g) + Cl2(g) with K = 1.6 × 10–5. 1.00 mole of pure NOCl and 0.958 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of NO(g). a 5.78 × 10–3 M b 9.58 × 10–1 M c 2.04 × 10–3 M d 4.09 × 10–3 M e 1.04 M
Consider the following equilibrium: 2NOCl(g) 2NO(g) + Cl2(g) with K = 1.6 × 10–5. 1.00 mole of pure NOCl and 0.958 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of NO(g). a 5.78 × 10–3 M b 9.58 × 10–1 M c 2.04 × 10–3 M d 4.09 × 10–3 M e 1.04 M
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.56QE
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Consider the following equilibrium:
2NOCl(g) 2NO(g) + Cl2(g)
with K = 1.6 × 10–5. 1.00 mole of pure NOCl and 0.958 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of NO(g).
a
|
5.78 × 10–3 M |
b
|
9.58 × 10–1 M |
c
|
2.04 × 10–3 M |
d
|
4.09 × 10–3 M |
e
|
1.04 M
|
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