Balance the redox reaction: 10^- _3 ___ When you balance the reaction, the numbe

Question

Balance the redox reaction: 10^- _3 ___ When you balance the reaction, the number of electron in the balanced half reaction is: A. 9 electron in the left B. 5 electron in the right C. 2 electron in the right D. 5 electron in the left E. 10 electron in the left Determine the entropy change for melting 18.0 g ice at the normal melting point. The enthalpy of fusion for water is 6.0 kJ/mol. The solubility of CrF_3 in water is 0.50 g/L at 25 degree C. Determine the solubility product constant for CrF_3. Which of the following is true for Galvanic cell? A. Delta G > 0, K > 1 B. Delta G > 0, E > 0 C. Delta G 1 D. Delta G H > Cu > Ag > Au ... Which is true? A. Na is the weakest oxidizing agent B. Au is the strongest reducing agent C. Na is the strongest oxidizing agent D. Ag will produce H_2 gas with acids E. Fe will reduce Mg How does the entropy changes in each of the following cases? (increase, decrease, no change) a. NaCl crystal is formed from a solution _____ b. solid iodine undergoes sublimation ______ c. N_2 (g) + H_2 (g) ____ NH_3 (g) _____ d. CuSO_4 crystals are dissolved in water e. KClO_3 (s) ___ KCl (s) + O_2 (g) ____ You may use the following information in solving any problem in the exam. Standard reduction potential values: cu^2+ + 2e ____ Cu (s) E degree = 0.342 V Fe^2+ + 2e ____ Fe E degree = - 0.447 V Cr_2 O^2+ _ + 14 H^+ + 6e _____ 2 Cr^3+ 7 H_2 O E degree = 1.33 V Fe^3+ + e ____ Fe^2+ E degree = 0.771 V Sn^4+ + 2 e ____ Sn^2+ E degree = 0.151 V O_2 + 2 H^+ + 2e ____ H_2 O_2 E degree = 0.695 V (Delta H_t values: C_5 H_12 (g) = - 320 kJ/mol; CO_2 (g) = - 390 kJ/mol; H_2 O (l) = - 285 kJ/mol) R = 0.08205 L atm/mol. k: R = 8.314 J/mol.k; F = 96481 C/mol e;

Explanation / Answer

16. Given solubility of CrF3 , S = 0.50 (g/L) x ( 1mol/109g)

= 4.59x10-3 mol/L

CrF3 ----> Cr3+ + 3F-

[Cr3+ ] = S & [F-] = 3S

Solubility product , Ksp = [Cr3+ ][F-] 3

= S x ( 3S)3

= 27 S4

= 1.19x10-8

Therefore Ksp =  1.19x10-8

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