Q1.) The following equilibrium exists at 552 K. (a) If there are 2.31 mol SO 2 ,

Question

Q1.) The following equilibrium exists at 552 K.

(a) If there are 2.31 mol SO2, 2.25107 mol O2, and 8.54 mol SO3 at equilibrium in a 12.9 L container, what is Kc for this reaction? (HINT: moles and volume are given - calculation molarities first! )


(b) Does this reaction favor the reactants or the product?

reactants or products   

Q2.) Consider the following equilibrium reaction at 250.°C.

If the equilibrium constant in terms of concentrations (Kc) is 3.4102, calculate the equilibrium constant in terms of partial pressures (Kp).

Q3.) Write the equilibrium constant expression for the following reaction in terms of concentrations of the components.

(Use the format: K_{c}=[C]c/[A]a.[B]b where the K_{c}= is required. Remember that exponents of 1's are understood and need not be typed and use a period to separate terms that are multiplied - and no spaces. Check the auto formatting in chemPad.)

Explanation / Answer

1)

a)

[SO2] = mol of SO2 / volume

= 2.31 mol / 12.9 L

= 0.179 M

[O2] = mol of O2 / volume

= 2.25*10^-7 mol / 12.9 L

= 1.74*10^-8 M

[SO3] = mol of SO3 / volume

= 8.54 mol / 12.9 L

= 0.662 M

Kc = [SO3]^2 / [SO2]^2 [O2]

Kc = (0.662)^2 / (0.179)^2 (1.74*10^-8)

Kc = 7.86*10^8

Answer: 7.86*10^8

b)

Since Kc is greater than 1, there will be more product at equilibrium

It will be product favoured

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