  # At a certain temperature, 0.5011 mol of N2 and 1.781 mol of H2 are placed in a 4.00-L containerN2(g)+3H2 (g)<---->2NH3At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Kc.

Question

At a certain temperature, 0.5011 mol of N2 and 1.781 mol of H2 are placed in a 4.00-L container

N2(g)+3H2 (g)<---->2NH3

At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Kc.

check_circleExpert Solution
Step 1

The given equilibrium reaction is

Step 2

Since 0.1401 mol N2 is present at equilibrium, mol of N2 that reacts = 0.5011 - 0.1401 = 0.361 mol N2

Using stoichiometry, calculate mol of H2 that reacts with 0.361 mol N2.

Step 3

How much NH3 is produced from N2 and H2? Convert mol of each reactant that "reacts" to mol NH3. The reactant...

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