A student ran the following reaction in the laboratory at 427 K:PCl5(g) PCl3(g) + Cl2(g)When she introduced 4.21 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of PCl5(g) to be 4.17 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.

PCl5(g) → PCl3(g) + Cl2(g)Initial 4.21 M 0 0 Initial…

Answered: A student ran the following reaction in…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 41QRT: Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) +...

See similar textbooks

Related questions

Question

A student ran the following reaction in the laboratory at 427 K:

PCl₅(g) PCl₃(g) + Cl₂(g)

When she introduced 4.21 moles of PCl₅(g) into a 1.00 liter container, she found the equilibrium concentration of PCl₅(g) to be 4.17 M.

Calculate the equilibrium constant, K_c, she obtained for this reaction.

Expert Solution

Step 1

$P C l_{5} (g) \to P C l_{3} (g) + C l_{2} (g) I n i t i a l 4.21 M 0 0 I n i t i a l c o n c e n t r a t i o n o f a f t e r d i s s o c i a t i o n - x x x P C l_{5} = 4.21 m o l e s / 1 l i t r e a t e q u i l i b r i u m 4.21 x - x x x = 4.21 M G i v e n a t e q u i l i b r i u m [P C l_{5}] = 4.17 M 4.21 - x = 4.17 M x = 4.21 - 4.17 x = 0.04 M [P C l_{3}] = 0.04 M [C l_{2}] = 0.04 M K_{C} = \frac{[P C l_{3}] [C l_{2}]}{[P C l_{5}]} = \frac{0.04 M x 0.04 M}{4.17 M} K_{C} = 3.837 x 10^{- 4} M$

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

A student ran the following reaction in the laboratory at 427 K: PCl5(g) PCl3(g) + Cl2(g) When she introduced 4.21 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of PCl5(g) to be 4.17 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.