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?

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queen_honey_blossom answered 2 years ago

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 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.

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 reaction and the initial concentration and initial rate data below. BrO3-(aq) + 5 Br-...

Consider the reaction and the initial concentration and initial rate data below. BrO3-(aq) + 5 Br- (aq) + 6 H+(aq) ® 3 Br2 (aq) + 3 H2O (l) Experiment [BrO3-], (M) [Br-],(M) [H+],(M) Initial Rate (M/sec) 1 0.10 0.10 0.10 1.2 x 10-3 2 0.20 0.10 0.10 2.4 x 10-3 3 0.10 0.30 0.10 3.5 x 10-3 4 0.20 0.10 0.15 5.4 x 10-3 a)Determine the rate law for this reaction b)What is the overall order of the rate law?...

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...

he reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) has the following equilibrium constant: K=[C][D][A][B]=2.4 What is the final concentration...

he reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) has the following equilibrium constant: K=[C][D][A][B]=2.4 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 ?

Consider the reaction A → products at 311 K. The concentration of A was monitored over...

Consider the reaction A → products at 311 K. The concentration of A was monitored over time and the data was analyzed by plotting. It was found that a plot of 1/[A] vs time gave a straight line relationship. It was also observed that it took 24.5 s for the concentration of A to decrease from 0.757 M to 0.107 M. What is the half life for this reaction when [A]o = 0.757 M?

Consider the reaction A → products at 282 K. The concentration of A was monitored over...

Consider the reaction A → products at 282 K. The concentration of A was monitored over time and the data was analyzed by plotting. It was found that a plot of ln[A] vs time gave a straight line relationship. It was also observed that it took 20.7 s for the concentration of A to decrease from 0.689 M to 0.235 M. What is the half life for this reaction when [A]o = 0.689 M? t1/2 (in seconds)

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