The value of K for a following reaction at standard condition is 2.1 x 1013. Cu2*(aq) + 4 NH3(aq) = Cu(NH3)42*(aq) What can you conclude from this? A. The rate constant of the forward reaction always is greater than the rate constant of the reverse reaction. B. The free energy of the reaction is approximately 76.0 kJ/mol. C. At equilibrium, the concentration of products will be much greater than the concentration of reactants. Gas constant is R = 8.3144598 J. mol-1. K1. B only. Both B and C. C only. Both A and . A only. Both A and B. All A, B, and C.

The value of K for a following reaction at standard condition is 2.1 x 1013. Cu2(aq) + 4 NH3(aq) = Cu(NH3)42(aq) What can you conclude from this? A. The rate constant of the forward reaction always is greater than the rate constant of the reverse reaction. B. The free energy of the reaction is approximately 76.0 kJ/mol. C. At equilibrium, the concentration of products will be much greater than the concentration of reactants. Gas constant is R = 8.3144598 J. mol-1. K1. B only. Both B and C. C only. Both A and . A only. Both A and B. All A, B, and C.

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

For the Haber process, Kc = 9.5 at 300C. Calculate Kp for this reaction at this temperature. N2(g) + 3 H2(g) → 2 NH3 (g)
Express the equilibrium constant for the following reaction. RbBrO3 (s) = RbBrO(s) + O2(g) ок [O2] [RbBrO]*[02]? [RbBrO3]? O K 2 [RbBrOg]3 [RbBrO]° [02]° O K O K [O2]-1 [RbBrO][O2] [RbBrO3] O K =
In the gas phase, formic acid forms a dimer, 2HCOOH(g) (HCOOH)2(g). For this reaction, AH = -60.1 kJ/mol and AG = -13.9 kJ/mol at 25°C. Find the equilibrium constant (Kp) for this reaction at 75 °C.
A(aq) + B(aq) = C(aq) has a standard free-energy change of –5.11 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] = [C] = M
Consider the following reaction: Ni(s) + 4CO(g) <-->Ni(CO)4(g) At 1397o C, the standard free energy change of the reaction is -40.0 kJ/mol. If the partial pressure of CO is 2 atm and that of Ni(CO)4(g) is 3 atm, calculate the free energy change of the reaction at 1397oC. Group of answer choices -63.2 kJ/mol -23.2 kJ/mol 23.2 kJ/mol -16.8 kJ/mol
ΔG° for the reaction shown is equal to -419.6 (kJ/mol). Use the information given in the table to determine the standard free energy of formation vales, Gf° (kJ/mol) for the substance D. 1 A(s) + 1 B(g) → 1 C(s) + 1 D(g) Substance Gf°(kJ/mol) A(s) -684.3 B(g) -223.7 C(s) 187.7
2. Which of the following reactions will occur spontaneously at standard-state conditions and25°C? a. Mg2+ + Ca → Mg + Ca²+ b. Au +3K+ → Au³+ + 3K c. 2Al³+ + 3Fe → 2Al + 3Fe²+ d. Cu + 2H+ → Cu²+ + H₂
1. If a reaction mixture initially contains a CO concentration of 0.1510 M and a Cl2 concentration of 0.179 M at 1000 K. What is the equilibrium concentration of CO at 1000 K? 2. What is the equilibrium concentration of Cl2 at 1000 K? 3. What is the equilibrium concentration of COCl2 at 1000 K? Thank you so much! These three questions bothered me for so long.
The standard reaction free energy AG=-1181. kJ for this reaction: 4 H,O2) + PbS(s)→ PBSO (s) + 4H,O(1) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction AG 8H,0, () + 2PBS(s) - 2 PbSo,(s) + 8H,0(1) kJ PbSO,(6) + 4H,0 (1) - 4H,0,(1) + PbS(s) 1 POSO,() + 2H,0(1) → 2H,0,(1) + ; PbS(s)
The difference in standard free energy between reactant R and product P is + 7.5 kJ/mol. What’s the ratio of P to R at equilibrium? P to R ratio =
Refer to the attached photo. Thank you!
→ At 355 K, AG = -1.3 kJ/mol for the reaction A (g) 2 B (g). If the partial pressures of A and B are 2.71 atm and 0.110 atm respectively, what is the standard free energy for this reaction at this temperature? AG = 82.5 kJ/mol for the reaction 3 A (g) + B (g) 2 C (g). At 1250 K, the partial pressures of A, B, and C are 10.8 atm, 9.90 atm, and 0.950 atm respectively. What is the free energy for this reaction?