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 2 years ago

Consider the system: A (aq) → B (aq) at 251 K where ΔGoform A = -11.7...

Consider the system: A (aq) → B (aq) at 251 K where ΔGoform A = -11.7 kJ/mol and ΔGoform B = -14.1 kJ/mol. Calculate the concentration of A at equilibrium when 1.71 mol of A and 1.35 mol of B are mixed in water to form exactly one liter of solution.

Consider the following reaction at 283 K: 2A + B → C + D where rate...

Consider the following reaction at 283 K: 2A + B → C + D where rate = k[A][B]2. An experiment was performed where [A]o = 2.67 M and [B]o = 0.00241 M. A plot of 1/[B] vs. time has a slope of 10.01. What will the rate of this reaction be when [A] = [B] = 0.345 M?

Consider the reaction: A (aq) ⇌ B (aq) at 255 K where the initial concentration of...

Consider the reaction: A (aq) ⇌ B (aq) at 255 K where the initial concentration of A = 1.00 M and the initial concentration of B = 0.000 M. At equilibrium it is found that the concentration of B = 0.501 M. What is the maximum amount of work that can be done by this system when the concentration of A = 0.849 M?

Consider the reaction: A (aq) ⇌ B (aq) at 277 K where the initial concentration of...

Consider the reaction: A (aq) ⇌ B (aq) at 277 K where the initial concentration of A = 1.00 M and the initial concentration of B = 0.000 M. At equilibrium it is found that the concentration of B = 0.363 M. What is the maximum amount of work that can be done by this system when the concentration of A = 0.891 M?

1) Consider the reaction: A (aq) ⇌ B (aq) at 253 K where the initial concentration...

1) Consider the reaction: A (aq) ⇌ B (aq) at 253 K where the initial concentration of A = 1.00 M and the initial concentration of B = 0.000 M. At equilibrium it is found that the concentration of B = 0.523 M. What is the maximum amount of work that can be done by this system when the concentration of A = 0.859 M? 2) Consider the following reaction at 257 K: 2 A (aq) + 1 B (aq)...

Consider the following reaction at 321 K: 2 A (aq) + 1 B (aq) → 2...

Consider the following reaction at 321 K: 2 A (aq) + 1 B (aq) → 2 C (aq) + 1 D (aq) An experiment was performed with the following intitial concentrations: [A]i = 1.33 M, [B]i = 2.05 M, [C]i = 0.25 M, [D]i = 0.29 M. The reaction was allowed to proceed until equilibrium was reached at which time it was determined that [A] = 0.51 M. What was the maximum amount of work that could have been performed...

Consider the following reaction at 215 K: 2 A (aq) + 1 B (aq) → 1...

Consider the following reaction at 215 K: 2 A (aq) + 1 B (aq) → 1 C (aq) + 1 D (aq) An experiment was performed with the following intitial concentrations: [A]i = 1.37 M, [B]i = 2.03 M, [C]i = 0.65 M, [D]i = 0.11 M. The reaction was allowed to proceed until equilibrium was reached at which time it was determined that [A] = 0.61 M. What was the maximum amount of work that could have been performed...

Consider the matrix of Hibert H100 and the system HX = b, where b is a...

Consider the matrix of Hibert H100 and the system HX = b, where b is a column vector from 1 to 100. Solve the system in the following three ways --> 1) X = H-1 b 2) Using the factorization H = LU 3) Using the factorization H = QR Premultiplica H for each of the three solution vectors and make the comparison with vector b. What method gives a better solution?

Consider the following dissociation of the weak acid, HCN: HCN(aq) ⇌ CN−(aq) + H+(aq) K =...

Consider the following dissociation of the weak acid, HCN: HCN(aq) ⇌ CN−(aq) + H+(aq) K = 6.2×10-10 A solution is made with an initial concentration of 2.60 M HCN. At equilibrium, what is the concentration of H+ ions in solution? (Hint: You may use the 5% approximation.) ?M

1) The reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) has the following equilibrium constant: K=[C][D][A][B]=5.2 a) Initially, only A...

1) The reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) has the following equilibrium constant: K=[C][D][A][B]=5.2 a) Initially, only A and B are present, each at 2.00 mol L−1. What is the final concentration of A once equilibrium is reached? b) What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 mol L−1 and [B] = 2.00 mol L−1 ?