Calculate K for the reaction A + 2B ↔ 3C if [A] = 0.3 M, [B] = 1.5 M, and [C] = 2.8 M. What is the value?

To calculate the equilibrium constant ( K ) for the reaction ( A + 2B \leftrightarrow 3C ), you can use the formula:

[

K = \frac{[C]^3}{[A][B]^2}

]

In this scenario, you have the concentrations of the reactants and products as follows:

• ([A] = 0.3 , \text{M})

• ([B] = 1.5 , \text{M})

• ([C] = 2.8 , \text{M})

Plugging these values into the formula, we first calculate ([C]^3):

[

[C]^3 = (2.8)^3 = 21.952

]

Next, calculate ([A][B]^2):

[

[B]^2 = (1.5)^2 = 2.25

]

Now, ( [A][B]^2 ) is:

[

[A][B]^2 = (0.3)(2.25) = 0.675

]

Now substituting these calculations back into the equilibrium constant expression:

[

K