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. H2(g) + F2(g) = 2 HF(g) 1 2 NEXT > 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.. Ke 2.1 x 103 5 RESET [0] [0.0021] 2[0.0021] [x] [2x] [x]P [2x]? [0.0011] 2[0.0011] [0.0011P II
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. H2(g) + F2(g) = 2 HF(g) 1 2 NEXT > 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.. Ke 2.1 x 103 5 RESET [0] [0.0021] 2[0.0021] [x] [2x] [x]P [2x]? [0.0011] 2[0.0011] [0.0011P II
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 39A
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![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.
H:(g) + F2(g) = 2 HF(g)
1
2
NEXT
>
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..
Ko
= 2.1 x 103
RESET
[0]
[0.0021]
2[0.0021]
[x]
[2x]
[2x}
[0.0011]
2[0.0011]
[0.0011P](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb7903d6c-428f-42dd-80a7-2bce49306e6c%2F5e17d32d-7967-4d1b-9999-a692a9b10024%2F8rsgzeb_processed.png&w=3840&q=75)
Transcribed Image Text: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.
H:(g) + F2(g) = 2 HF(g)
1
2
NEXT
>
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..
Ko
= 2.1 x 103
RESET
[0]
[0.0021]
2[0.0021]
[x]
[2x]
[2x}
[0.0011]
2[0.0011]
[0.0011P
![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.
H2(g) + F2(g) = 2 HF(g)
PREV
1
2
Based on your expression for Kc, solve for the equilibrium concentration of HF.
[HF]eq
M
5 RESET
0.0093
0.096
4.4
4.58 x 10-5
2.1 x 10-9
1.0 x 106](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb7903d6c-428f-42dd-80a7-2bce49306e6c%2F5e17d32d-7967-4d1b-9999-a692a9b10024%2F4znhhp_processed.png&w=3840&q=75)
Transcribed Image Text: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.
H2(g) + F2(g) = 2 HF(g)
PREV
1
2
Based on your expression for Kc, solve for the equilibrium concentration of HF.
[HF]eq
M
5 RESET
0.0093
0.096
4.4
4.58 x 10-5
2.1 x 10-9
1.0 x 106
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