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 In acidic solution, BiO3-(aq) is reduced to Bi3+(aq) by Al(s) which in turn is oxidised to Al2O3(s)

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 In acidic solution, BiO3-(aq) is reduced to Bi3+(aq) by Al(s) which in turn is oxidised to Al2O3(s). Write balanced equation that describes this process. 
Q2. The decomposition reaction of hydrogen peroxide (H2O2(aq)) into water and oxygen is a first order reaction with a rate constant, k = 4.0 x 10-8 L mol-1 s-1 at 0°C. Answer the following questions:
a) What is the half life for the decomposition of hydrogen peroxide at 0°C? (1 mark)
b) What percentage of the original hydrogen peroxide would be left after 1.0 x 108 seconds has elapsed at 0ºC? (1.5 marks)
-c) How long will it take for the concentration of hydrogen peroxide to decrease from 1.0 mol / L to 0.25 mol / L? (1 mark
Q3. Use the Nernst equation to calculate the cell potential, E, for the following Galvanic cell at 25ºC,
Zn Ι Zn2+(aq) ΙΙ Cu2+(aq) Ι Cu
where the [Zn2+(aq)] = 2.00 mol / L and [Cu2+(aq)] = 0.00100 mol / L. For this reaction, the standard cell potential, E0 = +1.10 V
Q4. A Galvanic cell was constructed based on the following two half reactions:
O2(g) + 4H+(aq) + 4e- → 2H2O(l)   E0red = +1.23 V
      Cr3+(aq) + 3e- → Cr(s)     E0red = -0.74 V
Answer the following questions:
a) Write balanced equation that describes the cell, ensuring that E0cell > 0 V. 
(3 marks)
b) Calculate E0cell for this reaction. (1 mark)
Q5. Use the Nernst equation to calculate the equilibrium constant, Kc, for the following reaction at 25ºC:
Fe2+(aq) + Ag+(aq) → Fe3+(aq) + Ag(s)   E0 = 0.030 V
Q6. Magnetic measurements of the complex ion [Mo(CN)6]4- show that it has 2 unpaired electrons, whole magnetic measurements of the [Mo(H2O)6]2+ complex ion show that it has 4 unpaired electrons. Answer the following questions concerning these experimental observations.
a) What is the oxidation state of the Mo in each complex? How many d valence electrons does each complex possess? (1 mark)
b) Complete crystal field diagram for each complex using the supplied template. (3 marks)
c) Which of the two complex ions, [Mo(CN)6]4- or [Mo(H2O)6]2+ would absorb visible light at the lower energy? Explain your answer. (1 mark)
d) Based on you previous answers, how many unpaired electrons would you expect the [Mo(NO2)6]4- complex ion to have and what complex would it have the most similar colour to [Mo(CN)6]4- or [Mo(H2O)6]2+ ? Explain your reasoning. 
PLEASE HELP ME TO SOLVE THESE QUESTIONS HAVE ONLY 40 MINUTES TO ANSWER THESE QUESTIONS.