At a certain temperature, 0.3811 mol of N2 and 1.761 mol of H2 are placed in a 4.50 L container according to the following equation: N2(g) + 3H2(g) ⇔ 2NH3(g) At equilibrium, 0.1001mol of N2 is present. Calculate the equilibrium constant.
At a certain temperature, 0.3811 mol of N2 and 1.761 mol of H2 are placed in a 4.50 L container according to the following equation: N2(g) + 3H2(g) ⇔ 2NH3(g) At equilibrium, 0.1001mol of N2 is present. Calculate the equilibrium constant.
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
Section17.3: Application Of Equilibria
Problem 1RQ
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At a certain temperature, 0.3811 mol of
N2
and 1.761 mol of
H2
are placed in a 4.50 L container according to the following equation:
N2(g) + 3H2(g) ⇔ 2NH3(g)
At equilibrium, 0.1001mol of
N2
is present. Calculate the equilibrium constant.
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