Question

In: Chemistry

Consider the system: A (aq) → B (aq) at 283 K where ΔGoform A = -11.5...

Consider the system: A (aq) → B (aq) at 283 K where ΔGoform A = -11.5 kJ/mol and ΔGoform B = -13.3 kJ/mol. Calculate the concentration of A at equilibrium when 2.01 mol of A and 1.39 mol of B are mixed in water to form exactly one liter of solution.

Expert Solution

A (aq) → B (aq)

ΔG⁰ = ΔG⁰f products - ΔG⁰f reactans

=-13.3-(-11.5) = -1.8Kj/mole = -1800J/mole

ΔG⁰ = -RTlnk

-1800 = -8.314*298*2.303logK

-1800 = -5705.84logK

logK = -1800/-5705.84

logK = 0.315

K = 10^0.315

K = 2.0654

concentration of A [A] = no of moles/volume in L

= 2.01/1 = 2.01M

concentration of B [B] = no of moles/volume in L

= 1.39/1 = 1.39M

A (aq) → B (aq)

I 2.01 1.39

C -x +x

E 2.01-x 1.39+x

Kc = [B]/[A]

2.0654 = 1.39+x/2.01-x

2.0654*(2.01-x) = 1.39+x

x = 0.9

[A] = 2.01-x = 2.01-0.9 = 1.11M

the concentration of A at equilibrium = 1.11M

queen_honey_blossom answered 1 year ago

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