Part A. Based on the following information, Br 2 (l) + 2 e - 2 Br - ( aq ) E ° =

Question

Part A. Based on the following information,
Br 2(l) + 2 e- 2 Br -(aq) E° = +1.09 V
Mg 2+(aq) + 2 e- 2 Mg(s) E° = -2.37 V
which of the following chemical species is the strongest reducing agent?

Part B. Consider the following standard reduction potentials,
Pb 2+(aq) + 2 e- Pb(s) E° = -0.13 V
I2(s) + 2 e- 2 I-(aq) E° = +0.54 V
Under standard conditions,

Part C. A redox reaction has an equilibrium constant of K=1.2×103. Which statement is true regarding Grxn and Ecell for this reaction? Which statement is true regarding and for this reaction?

Part D. A redox reaction has an E°cell = 0.58 V. What can you conclude about the equilibrium constant(K) for the reaction?

Part E. What element is being reduced in the following redox reaction?
MnO4-(aq) + H2C2O4(aq) Mn2+(aq) + CO2(g)

Explanation / Answer

A)

reducing agent --> The one oxidizing, i..e the one with the lowest potential

choose Mg(s)

B)

the order or reduciton potential

I- > Pb > Pb+2 > I2

then for the reducing agent, invert order i..e I2 is the strongest and so on

C)

if K> 1, this is favoured forward, then E°cell > 0 and G < 0

D)

if Ecell > 0, then Grxn > 0, K < 1

E

Mn goes from +7 to +´2, it gains 5 electrons, then Mn

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