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5 October, 16:51

At a certain temperature, 0.4011 mol of N2 and 1.621 mol of H2 are placed in a 3.50 L container. N2 (g) + 3H2 (g) ↽--⇀2NH3 (g) At equilibrium, 0.1001 mol of N2 is present. Calculate the equilibrium constant, Kc.

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  1. 5 October, 16:56
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    The equilibrium constant ≈120.07

    Explanation:

    Step 1: The balanced equation

    N2 (g) + 3H2 (g) ↽--⇀2NH3 (g)

    This means that for 1 mole of N2 consumed, there is needed 3 moles of H2 to produce 2 moles of NH3

    Step 2: Calculate initial moles

    Reactants:

    ⇒N2: 0.4011 mol es

    ⇒H2: 1.621 mol es

    Products

    ⇒NH3: 0 mol

    Step 3: Calculate number of moles that changed

    N2: 0.4011 mol - 0.1001 mol = 0.3010 mol

    H2: 3 * 0.3010 mol = 0.9030 mol

    NH3: 2 * 0.3010 mol = 0.6020 mol

    Step 4: Calculate moles at the equilibrium

    N2: 0.1001 moles

    ⇒[N2] = 0.1001moles / 3.5L = 0.0286 M

    H2: 1.621 moles - 0.9030 moles = 0.718 moles

    ⇒[H2] = 0.718 moles / 3.5L : 0.205 M

    NH3: 0.6020 mol es

    ⇒[NH3] = 0.6020 / 3.5 = 0.172M

    Step 5: Calculate Kc

    Kc = [NH3]² / ([N2] [H2]³)

    Kc = 0.172² / (0.0286*0.205³)

    Kc = 0.029584‬ / (0.0286 * 0.008615125‬)

    Kc ≈120.07

    The Kcis a high value, this shows the position of the equilibrium is to the right.

    The equilibrium constant ≈120.07
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