It is determined that the equilibriumconcentrations of Fe3+, SCN and [F eSCN2*] are 5.30 × 10-4 M (5.30 times 10 tothe minus 4th power M), 8.30 x 10-4 M(8.30 times 10 to the minus 4th power M)and 2.60 x 104 M (2.60 times 10 to theminus 4th power M) respectively. What isthe value of K,? No units, please.XYour Answer:Answer

Given data Equilibrium concentration are Fe3+=5.30×10-4 M SCN-=8.30×10-4 M FeSCN2+=2.60×10-4 M

Answered: It is determined that the equilibrium…

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...

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A student determines [FeSCN2+] is 0.00016 M at equilibrium. If the initial concentration of Fe3+ was 0.00080 M and the initial SCN- concentration was 0.0012 M, what is the measured value of Kc?
At a certain temperature, the equilibrium constant for the chemical reaction shown is 3.86×10−33.86×10−3. At equilibrium, the concentration of AB is 2.6252.625 M, the concentration of BC is 2.8252.825 M, and the concentration of AC is 0.1300.130 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq)
Calculate K for the reaction between the general reactants A and B. The equilibrium concentrations are as follows: [A] = 0.596 M; [B] = 0.536 M; [AB] = %3D 0.543 M. 2 A3 +3 B2 = 6 AB
A student prepares an FeSCN2+ experimental sample by mixing:4.0 mL of 0.0025 M Fe(NO 3) 32.0 mL of 0.0025 M KSCN8.0 mL of 0.10 M HNO 3Based on a standard curve, it was determined that the concentration of FeSCN 2+ present in thesample at equilibrium was 2.52 × 10 -5 M. Based on this data, calculate the equilibrium constant forthe reaction of Fe 3+ with SCN– .
4 Calculate the equilibrium constant, K, for the following: A + 2 B 3C +D when the equilibrium concentrations of each species were determined: [A] = 0.010 M, [B] = 0.15 M, [C] = 0.20 M, and [D] = 0.25 M.
In the fictitious reaction below, the equilibrium concentration of A is 0.7140 M, B is 0.1133 M, and A 2B 3 is 0.5984 M. What is the value of the equilbrium constant k for this reaction? 2 A (ag) + 3 В (aq) А 2B з 0.001239 128.1 8.778 7.397 807.1
A student ran the following reaction in the laboratory at 642 K: 2HI=H2+I2 When she introduced 0.368 moles of HI into a 1.00 liter container, she found the equilibrium concentration of I2 to be .0363 M Calculate the equilibrium constant, KC, she obtained for this reaction.
At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The resulting equilibrium solution has a pH of 10.18. What is the Kp of the salt at 22 °C? -12 1.4 x10 Ksp = Incorrect
Fe3+ + SCN- <---> FeNCS2+ Given that Keq= 299, the initial concentration of Fe3+ is 0.04 M, and the initial concentration of SCN- is 0.001 M, calculate the final concentrations of each species in the reaction at equilibrium.
Calculate the concentration of Ag+ present in solution at equilibrium when concentrated ammonia is added to a 0.010 M solutionof AgNO3 to give an equilibrium concentration of [NH3] = 0.20 M. Neglect the small volume change that occurs when NH3 isadded.
9. For the reaction Hg²+ (aq) + 4 I- (aq) → [HgI4]²+ (aq) the value of Kc = 1.0 × 1030. If the initial concentration of I- is 0.78 M and Hg2+ is 0.010 M, what will be the equilibrium concentrations of Hg²+?
calc . the equilibruim concebtration if k = 1.2 x 10^-5

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