A solution contains 0.097 M Ce3+, 1.55x10-3 M Ce4+, 1.55x10-3 M Mn2+, 0.097 M MnO4-, and 1.00 M HClO4 (F= 9.649 x 104 C/mol). a) Write a balanced net reaction that can occur between species in this solution. b) Calculate deltaG0 and K for the reaction. c) Calculate E and deltaG for the conditions given. Ce4+ + e- = Ce3+  E0= 1.70 V MnO4- + 8H+ + 5e- = Mn2+ + 4H2O   E0= 1.507 V

Given the equilibrium constants for the following reactions: 4Cu(s) + O2(g) = 2Cu,O(s), K1 2CuO(s) = Cu20(s) +02(g), K2 n what is K for the system 2Cu(s) + O2(g) = 2CuO(s) equivalent to? Select one: O a. [(K2) / (K1)] O b. (K)(K» O . (K)(K) O d. (K)/ (K O e. [(K)/ (K2)] re to search F10 %24 G M

Potassium Ferrioxalate is mixed with in 50 mL of 1 M H2SO4 In a beaker , it is then placed one-half of this solution in another beaker in the sun and the other half in a cabinet in the dark. the color of both solutions after 0, 5, 15, and 30 minutes are : In the sun it stayed clear the whole 30 min and the sample in the darkness of the cabinet turned light green, Briefly explain your observations in terms of the photochemical properties of ferrioxalate.

When 1.40 moles of Br2 are put in a 0.960−L flask, 1.10 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Kc for the reaction.

6. Please don't write on a paper. I can't understand handwritten.

What happens when too much NaSCN is prepared in solution of mixtures of standard solutions of Fe(NO3)3 and NaSCN, so that [SCN^-] is higher than expected? What does this do to the measured Keq?

2. The popular antacid, Milk of Magnesia, is a suspension of magnesium hydroxide, Mg(OH)2. In water, Mg(OH)2 undergoes the reaction shown in Equation 9. Mg(OH),(s, white) = Mg²+(aq) +20H¯(aq) (Eq. 9) (1) What would you observe if you added an acid to an equilibrium mixture containing MgtOH)2 H water? (2) Write a chemical equation that accounts for the effect of the added acid. (3) Briefly explain how your answer to (1) is consistent with Le Châtelier's principle.

Given that Ksp for AgCl is 1.6E-10 and Kf for Ag(CN)2- is 5.6E8, calculate the concentration of Ag+ when 0.15 M AgNO3 is reacted with 0.25 M KCN.

1. Calculate the concentration of ions in the following saturated solutions: (a) [1'] in Agl solution with [Ag'] = 9.1 x 10° M; Ksp= 8.3 x 107 (b) [A*] in Al(OH); solution with [OH] = 2.9 x 10° M; Ksp = 1.8 x 10 33 2. 2.4414 g sample containing KCI, K;SO4 and inert materials was dissolved in sufficient water to give 250 mL of solution. A Mohr titration of a 50 ml aliquot required 41.36 ml of 0.05818 M AGNO3. A second 50mL aliquot was treated with 40 ml of 0.1083M NaB(CsHs)4. The reaction is NaB(CsHs)a + + KB(CsHs)4s) + Na*. The solid was filtered, redissolved in acetone, and titrated with K* 49.98mL of the AgNO: solution according to the reaction KB(C,H;). + Ag* + AgB(CsHs)46) + K*. Calculate the percentage of KCl and K:SO, in the sample. a. As a food chemist for a major potato chip company, you are responsible for determining the salt content of new potato chip products for the packaging label. The potato chips are seasoned with table salt, NaCl. You weigh out a handful of the chips…

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