We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
please help answer QUESTION 2 Calculate the value of the equilibrium constant for the following reaction...
Determine the value of the equilibrium constant for the reaction below if an equilibrium mixture contains 0.0497 g PbCl2, and is 0.0165 M in C ions and is 0.0392 M in Pb2+ ions. PbCl2 (s) = Pb2+ (aq) + 2 CF(aq) Answer:
13. Calculate the value for the equilibrium constant, Ksp for the following reaction. Ca(OH)2 (s) - > Cat? (aq) + 2OH(aq) assume that a 20.00 mL sample of saturated Ca(OH)2 was titrated with a 0.050 M standard HCI solution to the equivalence point. Assume that 8.1 mL of standard HCl was needed to get to the equivalence point
please help me answer this question........ thanks Use the appropriate standard reduction potentials in the appendix of your book to determine the equilibrium constant at 205.00 K for the following reaction under acidic conditions. 4H^+(aq)+MnO_2(s)+2Fe^2+(aq) rightarrow Mn^2+(aq)+2Fe^3+(aq)+2H_2O(I) k = 6.19 times 10^53 The equation that relates equilibrium constants with cell potentials is: log k = nFE^0_cell/2.303RT Use this formula, along with the information in the appendix of your book to solve for K.
13. Calculate the value for the equilibrium constant, Ksp for the following reaction. Ca(OH)2 (s) Ca+2 (aq) + 2 OH- ⇆ (aq) assume that a 20.00 mL sample of saturated Ca(OH)2 was titrated with a 0.050 M standard HCl solution to the equivalence point. Assume that 8.1 mL of standard HCl was needed to get to the equivalence point. (I am having trouble with this one. Let me know if there is additional information needed)
Question 9 of 27 > Calculate the equilibrium constant for the chemical reaction, given the equilibrium concentrations of the reactants and products in the table. Substance . Equilibrium concentration AB 1.48 M CD 2.00 M AD 2.51 M BD 2.04 M 4.85 M 2 AB(aq) + 4 CD(aq) = 2 AD(aq) + 2 BD(aq) + 4C(aq)
The value of the equilibrium constant for the following chemical equation is Kc = 5.2 ×103 AgCl (s) + 2S2O32-<-->[Ag(S2O3)2]3- (aq) + Cl– (aq) Calculate the solubility of AgCl (s) in an aqueous solution whose equilibrium concentration of S2O32- is 0.015 M. Ksp = 1.8 × 10-10 M2 for AgCl
calculate equilibrium constant and free energy change please Calculate the cell potential, the equilibrium constant, and the free-energy change for Ca(s) + M12+ (aq)(1M) = Cap+ (aq)(1M) + Mn(3) given the following E' values: Ca2+ (aq) + 2e + Ca(8) E° = -1.50 V Mn2+ (aq) + 2e - →Mn(s) E° = -0.58 V Part A Calculate the cell potential 0.920 V Previou Correct Part B Calculate the equilibrium constant I ALCO ? Submit Previous Answers Request Answer X Incorrect;...
< Question 7 of 10 > Substance Calculate the equilibrium constant for the chemical reaction, given the equilibrium concentrations of the reactants and products in the table. Equilibrium concentration 4.01 M AB CD 3.60 M 4.82 M 2 AB(aq) + 4CD(aq) = 2 AD(aq) + 2 BD(aq) + 4C(aq) 2.22 M 3.66 M
selected answer is incorrect please solve Question 8 0 / 1 point Calculate the equilibrium constant, K, for the spontaneous galvanic cell between Pb2+/Pb and Cr3+/Cr2+ conducted at standard conditions. 7.9 x102 1.7 x1014 3.1 x109 5.6 x104
(Set 2) Practice Problems in Equilibrium All weak acids use this generic equation: HA(aq)+ H2O() A (aq) + H30*(aq) And all weak bases use this one: B(aq)+ H2O(I) = BH*(aq)+ OH'(aq) Part A: Finding K, or Kb 3.012? What is the value of Ka for a weak acid if a 1.44 M solution has a pH 1. 2. A weak acid is 0.00987 M, but is found to be 25.5 % ionized. What is the pH? 3. The pH for...