In a certain experiment 7.50 mile of NH3 was placed in an empty 1.0 liter flask at 900C. After equilibrium was reached, 0.50 mile of N2 was found to be in the flask (along with other gases). Calculate the [NH3] and [H2] at equilibrium and the numerical value of Kc. 2NH3 (g) = N2(g) + 3H2(g)
In a certain experiment 7.50 mile of NH3 was placed in an empty 1.0 liter flask at 900C. After equilibrium was reached, 0.50 mile of N2 was found to be in the flask (along with other gases). Calculate the [NH3] and [H2] at equilibrium and the numerical value of Kc. 2NH3 (g) = N2(g) + 3H2(g)
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does...
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In a certain experiment 7.50 mile of NH3 was placed in an empty 1.0 liter flask at 900C. After equilibrium was reached, 0.50 mile of N2 was found to be in the flask (along with other gases). Calculate the [NH3] and [H2] at equilibrium and the numerical value of Kc.
2NH3 (g) = N2(g) + 3H2(g)
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