At 25oC, for the reaction 2 A(aq) ----> B(aq) + C(aq), the equilibrium constant is 1.79 . If the concentration of B(aq) were 0.311 M and the concentration of C(aq) were 0.477 M, what would be the minimum concentration of A(aq) required (in mol/L) to make this reaction spontaneous under these conditions?

At 25oC, for the reaction 2 A(aq) ----> B(aq) + C(aq), the equilibrium constant is 1.89. If the concentration of B(aq) was 0.361 M and the concentration of C(aq) was 0.496 M, what would be the minimum concentration of A(aq) necessary in order (in mol/L) to make this reaction spontaneous under these conditions?

Consider the following reaction at 25 °C: 3 Ni(s) + N2(g) + 3 H₂O(g) → 3 NiO(s) + 2 NH,(9) If AG° = 18.1 kJ/mol, determine the value of the equilibrium constant at 25 °C.

A chemist fills a reaction vessel with 0.960 M lead (II) (Pb²+) aqueous solution, 0.951 M bromide (Br¯) aqueous solution, and 0.643 g lead (II) bromide (PbBr₂) solid at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 2+ Pb²+ (aq) + 2Br¯ (aq) → PbBr₂ (s) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. kJ X

Give correct detailed Solution (don't give Handwritten answer)

Consider the balanced reaction: 2Cr3+(aq)+3PbO2(s)+6H2O(l)→2CrO42-(aq)+3Pb2+(aq)+4H3O+ (aq) i. At 298.2 K, this reaction has an equilibrium constant K = 1.6 × 1013 . What is the standard molar free energy of reaction, ΔG° (in kJ/mol), for this reaction at 298.2 K? g. At a certain point the measured ∆G is –5 kJ/mol. Lowering the pH will cause free energy change of the reaction, ∆G, to..... choose (become less negative, stay the same, become more negative) h.The reaction is used to set up an electrochemical cell. What is true about the cell if the measured voltage is negative?... choose (Q < K,  Q = K,  Q > K, Need more info)

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

For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard Gibbs free enthalpy change is 1.62 kJ at 25oC. The initial concentration of A(aq) is 0.562 M, the initial concentration of B(aq) is 0.335 M, and the initial concentration of C(aq) is 0.202 M. What would be the concentration of A(aq) (in mol/L) once we attain equilibrium (we are still at 25oC)?

For the reaction A(aq) + B(aq) <---> C(aq) + D(aq), the equilibrium constant is 24.8 at 25oC and 37.5 at 50oC. What is the value of the change in the standard Gibbs free enthalpy (in kJ) of this reaction at 75oC?

consider dissolution of calcium fluoride at 25C. what is the ΔG (kj/mol) for the formation of calcium fluoride?