of 201819691 STOM ads In a sealed flask at 400°C the equilibrium constant of the following reaction see below is 0.50. The concentrations at equilibrium of the N2 was 0.125 M and the concentration of NH3 was 0.53 M calculate the equilibrium concentration of the H2. N2(g) + 3H2(g) = 2NH3(g) arlo Hq B HOqarted iw lw HOO oiloa

World of Chemistry, 3rd edition
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ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
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Chapter17: Equilibrium
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Problem 38A
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In a sealed flask at 400°C the equilibrium constant of the following reaction see below
is 0.50. The concentrations at equilibrium of the N2 was 0.125 M and the concentration of NH3
was 0.53 M calculate the equilibrium concentration of the H2.
N2(g) + 3H2(g) = 2NH3(g)
arlo Hq B HOqarted iw lw HOO oiloa
Transcribed Image Text:of 201819691 STOM ads In a sealed flask at 400°C the equilibrium constant of the following reaction see below is 0.50. The concentrations at equilibrium of the N2 was 0.125 M and the concentration of NH3 was 0.53 M calculate the equilibrium concentration of the H2. N2(g) + 3H2(g) = 2NH3(g) arlo Hq B HOqarted iw lw HOO oiloa
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