A reactionA(aq)+B(aq) = C(aq)has a standard free-energy change of –4.18 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 are0.30 M, 0.40 M, and 0 M, respectively?[A] =M[B] =M[C] =MHow would your answers change if the reaction had a standard free-energy change of +4.18 kJ/mol?There would be no change to the answers.There would be less A and B but more C.All concentrations would be lower.There would be more A and B but less C.All concentrations would be higher.

We have to calculate concentration of all species at equilibrium .

A reaction A(aq)+B(aq) = C(aq) as a standard free-energy change of -4.18 kJ/mol at 25 °C. Vhat are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are .30 M, 0.40 M, and 0 M, respectively? A] = B] = C] = How would your answers change if the reaction had a standard free-energy change of +4.18 kJ/mol? There would be no change to the answers. There would be less A and B but more C. O All concentrations would be lower. There would be more A and B but less C. All concentrations would be higher.

A reaction A(aq)+B(aq) = C(aq) as a standard free-energy change of -4.18 kJ/mol at 25 °C. Vhat are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are .30 M, 0.40 M, and 0 M, respectively? A] = B] = C] = How would your answers change if the reaction had a standard free-energy change of +4.18 kJ/mol? There would be no change to the answers. There would be less A and B but more C. O All concentrations would be lower. There would be more A and B but less C. All concentrations would be higher.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The standard reaction free energy AG°=-–457. kJ for this reaction: 2 H,(g) + O2(g)→2 H,O(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. AG reaction x10 2H,0 (g) - 2H, (g) + 0,(g) kJ 4H, (g) + 20, (g) → 4H,0(g) kJ 8H,0 (g) → 8H, (8) + 40, (g) kJ
Please don't provide handwritten solution ....
The standard reaction free energy AG°= = -910. kJ for this reaction: 6C(a)+ 6H2(g)+ 3O2(g)->C6H12O(s) Use this information to complete the table below. Round each of your answers to the nearest kJ.
reg # 3 [Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH = 108 kJ, and K. = 1.29 × 10-2, at 600 K: COC1₂ (g) CO(g) + Cl₂ (g) E 20 If the temperature on the equilibrium system is suddenly increased: The value of Ke D Oincreases Odecreases O remains the same The value of Qc Ols less than Ke Ois greater than K O is equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of Cl₂ will Oincrease Odecrease Oremain the same Submit Ans Show Hint $ 4 000 000 F4 R F % 5 T ry Entire Group Cengage Learning | Cengage Technical Support G A 6 9 more group attempts remaining MacBook Air Y H & 7 U * 00 8 ( 9 K O -0 ) F10 P 4) F11 Previous + 11 Next> Save and Ex A
The standard reaction free energy AG = 890. kJ for this reaction: ALO3(s) + 3H₂(g) 2 Al(s) + 3H₂O(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction — Al(s) + H₂O(g) → = ALO, (-) – È F¹₂ (3) –Al₂O; (3) + H₂(g) — — Al(s) – H₂O(g) 2Al(s) + 3H₂O(g) → ALO₂ (s) + 3H₂(g) 4 AG 0 OKJ X
1. Consider the reaction: A 2 B, where Keg 1.33 x 10-1. (a) What is the AGº' for this reaction? (b) If the reaction above is initially at standard-state conditions, what are the concentrations of A and B once equilibrium is reached?
A reaction has a standard free-energy change of –13.20 kJ mol-(-3.155 kcal mol-). Calculate the equilibrium constant for the reaction at 25 °C. Keg
I want solutions of all parts... Otherwise I will downvote
At 725 K, AG° = -21.6 kJ/mol for the reaction A (g) + 2 B (g) - 3 C (g). If the partial pressures of A, B, and C are 0.420 atm, 0.110 atm, and 7.20 atm respectively, what is the free energy for this reaction?
Calculate AG°for each of the following reactions from the equilibrium constant at the temperature given. Reaction Temperature (°C) 2000 N₂ (g) + O₂(g) →→→ 2NO (g) H₂ (g) + 12 (g) → 2HI (g) 400 CO₂ (g) + H₂ (9) → CO (g) + H₂O (g) 980 CaCO3 (s) → CaO (s) + CO2 (g) 900 Ko value 4.1 x 10-4 50.0 1.67 1.04
At 560 K, AG° = -26.5 kJ/mol for the reaction A (g) + 2B (g) → 3 C (g). If the partial pressures of A, B, and C are 0.420 atm, 0.110 atm, and 7.20 atm respectively, what is the free energy for this reaction?
The standard reaction free energy AGO= == -910. kJ for this reaction: 6 C(s) + 6H₂(g) + 3O₂(g) →C6H12O6(s) Use this information to complete the table below. Round each of your answers to the nearest kJ. AGⓇ reaction x10 1 C₂H₁2O6 (s) → 2C (s) + 2H₂ (g) + O₂ (g) kJ 3 C6H₁2O6 (s). 6C (s) + 6H₂(g) + 30₂ (g) kJ 12 3 1 3C (s) + 3H₂(g) + - 12/0₂ (8) → — C₂H₁2 06 (8) kJ 6 12 X ?