Chem solubility problem?

4. In a 500 mL flask, we put 6 mol of A, 6 mol of B, 4 moles of C and 9 mol of D. The value of K is 17.3.

Is the system in equilibrium? If not, in which direction will the reaction proceed to attain equilibrium?

A(g) + 2B(g)<---->2C(g) +D(g)

2 Answers

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  • 9 years ago
    Best Answer

    K = {[C]^2*[D]} / {[A][B]^2}

    K = {[4/0.5]^2*[9/0.5]} / {[6/0.5][4/0.5]^2}

    Efffectively the volumes cancel down and so can be written

    K = {16*9} / {6 * 16}

    K = 144 / 96

    K = 1.5

    The system is NOT in equilibrium .

    Since K needs to be larger 1.5 < 17.3 , the concentrations of the products 'C' & 'D' need to be larger and the concentrations of 'A' & 'B' need to be smaller.

    So the reaction will proceed to create more product, that is from left to right.

  • 9 years ago

    shift R as the constant is positive.

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