Consider the following net ionic reaction in aqueous in medium under standard st

Question

Consider the following net ionic reaction in aqueous in medium under standard state: MnO_4^- + H_2 O_2 ____ Mn^2- + O_2 + 1.20 kJ/mol What is the entropy change of this redox reaction if the free energy change is 1.80 kJ/mol? A. 0.01067 J/k B. 0.00201 kJ/k C. -10.06 J/k D. 0.00207 kJ/k E. 10.06 kJ/k Consider the reaction: C_ H_ (g) + 5 O_2 (g) ____ 3 CO_2 (g) + 4 H_2 O (l) + 1.30 kJ The entropy change for the reaction is - 12.0 J/k. At what temperature(s) would you expect the reaction to be spontaneous? A. T > 192 k B. T > 150 k C. T

Explanation / Answer

10)

pKa = -log Ka = -log (3.10 x 10^-6)

pKa = 5.509

millimoles of HNO2 = 25 x 0.1 = 2.5

At equivalence point :

millimoles of acid = millimoles of base

2.5 = 0.125 x V

V = 20 mL

here salt only remains.

salt concentration = millimoles / total volume

                              = 2.5 / 20 + 25 = 0.056 M

pH = 7 + 1/2 (pKa + log C)

    = 7 + 1/2 (5.508 + log 0.056)

    = 9.13

pH = 9.13

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