Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 × 103 at a certain temperature. If the equilibrium concentrations of H2 and F2 are both 0.0021 M, determine the concentration of HF at equilibrium. %3D H2(g) + F2(g) = 2 HF(g) 1 2 If [x] represents the equilibrium concentration of HF, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms..
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 × 103 at a certain temperature. If the equilibrium concentrations of H2 and F2 are both 0.0021 M, determine the concentration of HF at equilibrium. %3D H2(g) + F2(g) = 2 HF(g) 1 2 If [x] represents the equilibrium concentration of HF, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms..
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 14.40QE
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Question 4 of 4
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Consider the equilibrium system described by
the chemical reaction below. For this reaction,
Kc = 2.1 x 10° at a certain temperature. If the
equilibrium concentrations of H2 and F2 are both
0.0021 M, determine the concentration of HF at
equilibrium.
H2(g) + F2(g) = 2 HF(g)
1
2
If [x] represents the equilibrium concentration
of HF, set up the equilibrium expression for Kc
to solve for the concentration. Do not combine
or simplify terms..
Kc =
= 2.1 x 103
2 RESET
[0]
[0.0021]
2[0.0021]
[x]
[2x]
[x]?
[2x]?
[0.0011]
2[0.0011]
[0.0011]?
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Transcribed Image Text:10:26
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Question 4 of 4
Submit
Consider the equilibrium system described by
the chemical reaction below. For this reaction,
Kc = 2.1 x 10° at a certain temperature. If the
equilibrium concentrations of H2 and F2 are both
0.0021 M, determine the concentration of HF at
equilibrium.
H2(g) + F2(g) = 2 HF(g)
1
2
If [x] represents the equilibrium concentration
of HF, set up the equilibrium expression for Kc
to solve for the concentration. Do not combine
or simplify terms..
Kc =
= 2.1 x 103
2 RESET
[0]
[0.0021]
2[0.0021]
[x]
[2x]
[x]?
[2x]?
[0.0011]
2[0.0011]
[0.0011]?
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![10:27
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Question 4 of 4
Submit
Consider the equilibrium system described by
the chemical reaction below. For this reaction,
Kc = 2.1 x 10° at a certain temperature. If the
equilibrium concentrations of H2 and F2 are both
0.0021 M, determine the concentration of HF at
equilibrium.
H2(g) + F2(g) = 2 HF(g)
2
Based on your expression for Kc, solve for the
equilibrium concentration of HF.
[HF]eg
RESET
0.0093
0.096
4.4
4.58 x 10-5
2.1 x 10-9
1.0 x 10-6
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Transcribed Image Text:10:27
ll ?
Question 4 of 4
Submit
Consider the equilibrium system described by
the chemical reaction below. For this reaction,
Kc = 2.1 x 10° at a certain temperature. If the
equilibrium concentrations of H2 and F2 are both
0.0021 M, determine the concentration of HF at
equilibrium.
H2(g) + F2(g) = 2 HF(g)
2
Based on your expression for Kc, solve for the
equilibrium concentration of HF.
[HF]eg
RESET
0.0093
0.096
4.4
4.58 x 10-5
2.1 x 10-9
1.0 x 10-6
Tap here or pull up for additional resources
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