The equilibrium constant for the following reaction is 6.30 at 723K. 2NH3 <=> N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 10.2 L container at 723 K contains 0.221 mol of NH3(g) and 0.315 mol of N2(g), the equilibrium concentration of H2 is M. (Enter numbers as numbers, no units. For example, 300 minutes would be 300. For letters, enter A, B, or C. Enter numbers in scientific notation using e# format. For example 1.43×10-4 would be 1.43e-4.)

The equilibrium concentration of H2 is 0.4579 M

Explanation:

Step 1: Data given

The equilibrium constant for the following reaction is 6.30 at 723K

Volume = 10.2 L

Number of moles NH3 = 0.221 moles

Number of moles N2 = 0.315 moles

Step 2: The balanced equation

2NH3 <=> N2(g) + 3H2(g)

Step 3: Calculate concentration

Concentration = moles / volume

Concentration NH3= 0.221 moles / 10.2 L

Concentration NH3 = 0.0217 M

Concentration N2 = 0.315 moles / 10.2 L

Concentration N2 = 0.0309 M

Step 4: Define Kc

Kc = [H2]³[N2] / [NH3]²

6.30 = [H2]³ * (0.0309) / (0.0217)²

[H2]³ = 0.09601 M

[H2] = 0.4579 M

The equilibrium concentration of H2 is 0.4579 M

beta decay is the answer

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