A reaction A(aq) + B(aq) --> C(aq) has a standard free-energy change of –3.23 kJ/mol at...

A reaction
A(aq) + B(aq) --> C(aq)
has a standard free-energy change of –3.23 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively?

Solutions

Expert Solution

Using the standard free energy change formula, we can find the equilibrium constant for the reaction

Initial 0.3M 0.4M 0

Final (0.3-x)M (0.4-x)M xM

The value of 0.826 is not possible since otherwise the conc of A and B will be negative hence the correct answer is 0.145M

Concentration of C = 0.145M

Concentation of B = (0.4 - 0.145) = 0.255M

Concentation of A = (0.3 - 0.145) = 0.155M

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A reaction A + B <==> C has a standard free-energy change of -3.27 kJ/mol at...

A reaction A + B <==> C has a standard free-energy change of -3.27 kJ/mol at 25oC What are the concentrations of A, B, and C at equilibrium if at the beginning of the reaction their concentrations are 0.30M, 0.40M and 0M respectively?

A reaction: A (aq) + B (aq) <-----> C (aq) has a standard free energy change...

A reaction: A (aq) + B (aq) <-----> C (aq) has a standard free energy change of -3.05 kJ/mol at 25 C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? A = ? M B= ? M C= ? M How would your answer above change if the reaction had a standard free energy change of +3.05 kJ/mol? A.)...

For the reaction A(aq) ---> B(aq) the change in the standard free enthalpy is 2.59 kJ...

For the reaction A(aq) ---> B(aq) the change in the standard free enthalpy is 2.59 kJ at 25 oC and 4.73 kJ at 45 oC. Calculate the value of this reaction's equilibrium constant at 75 oC.

has a standard free-energy change of –3.82 kJ/mol at 25 °C. What are the concentrations of...

has a standard free-energy change of –3.82 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively

a) For the reaction: A(aq) ---> B(aq) the change in the standard free enthalpy is 2.83...

a) For the reaction: A(aq) ---> B(aq) the change in the standard free enthalpy is 2.83 kJ at 25 oC and 4.61 kJ at 45 oC. Calculate the value of this reaction's equilibrium constant at 75 oC. b) A container encloses 31.1 g of CO2(g). The partial pressure of CO2 is 2.66 atm and the volume of the container is 25.9 L. What is the average, or root mean square, speed (in m/s) of the CO2 molecules in this container?

The standard free energy of activation of a reaction A is 75.1 kJ mol–1 (17.9 kcal...

The standard free energy of activation of a reaction A is 75.1 kJ mol–1 (17.9 kcal mol–1) at 298 K. Reaction B is one million times faster than reaction A at the same temperature. The products of each reaction are 10.0 kJ mol–1 (2.39 kcal mol–1) more stable than the reactants. (a) What is the standard free energy of activation of reaction B?

Consider the reaction NH4Cl(aq)NH3(g) + HCl(aq) The standard free energy change for this reaction is 62.8...

Consider the reaction NH4Cl(aq)NH3(g) + HCl(aq) The standard free energy change for this reaction is 62.8 kJ. The free energy change when 1.72 moles of NH4Cl(aq) react at standard condition is____ kJ. What is the maximum amount of useful work that the reaction of 1.72 moles of NH4Cl(aq) is capable of producing in the surroundings under standard conditions?_______ If no work can be done, enter none. kJ

What is the standard free energy of the reaction, in kJ, at 298K for: 1 A...

What is the standard free energy of the reaction, in kJ, at 298K for: 1 A (aq) + 1 B (aq) <--> 2 C (aq) + 2 D (aq) if ΔH° (A)= -3.4134 kJ/mol , ΔH° (B) = 93.8823 kJ/mol, ΔH° (C) = -26.8495 kJ/mol, and ΔH° (D) = -39.4984 kJ/mol ΔS° (A)= 33.3845 J/(mol K) , ΔS° (B) = 92.5722 J/(mol K) , ΔS° (C) = -59.1781 J/(mol K) , and ΔS° (D) = -12.7602 J/(mol K)

A) The activation energy of a certain reaction is 48.0 kJ/mol . At 27 ∘C ,...

A) The activation energy of a certain reaction is 48.0 kJ/mol . At 27 ∘C , the rate constant is 0.0120s−1. At what temperature in degrees Celsius would this reaction go twice as fast? B) Given that the initial rate constant is 0.0120s−1 at an initial temperature of 27 ∘C , what would the rate constant be at a temperature of 170. ∘C for the same reaction described in Part A?

a) The activation energy of a certain reaction is 47.0 kJ/mol . At 24 ∘C ,...

a) The activation energy of a certain reaction is 47.0 kJ/mol . At 24 ∘C , the rate constant is 0.0190s−1. At what temperature in degrees Celsius would this reaction go twice as fast? b)Given that the initial rate constant is 0.0190s−1 at an initial temperature of 24 ∘C , what would the rate constant be at a temperature of 100. ∘C for the same reaction described in Part A?

Subjects