Consider the balanced reaction: 2Cr3+(aq)+3PbO2(s)+6H2O(l)→2CrO42-(aq)+3Pb2+(aq)+4H3O+ (aq) a.Which species is the oxidizing agent b.What is the oxidation state of the O in CrO42- c.What is the oxidation state of the Pb in PbO2? d.How many valence electrons are in the CrO42- ion? e. How many moles of electrons, ne, are transferred per mole of this reaction? f. At a certain point the measured free energy is ∆?. Adding more PbO2 will cause the free energy change of the reaction, ∆G, to choose...(Increase, Stay the same, Decrease) g. At a certain point the measured ∆G is –5 kJ/mol. Lowering the pH will cause the free energy change of the reaction, ∆?, to choose... (become less negative, stay the same, become more negative) h. The reaction is used to set up an electrochemical cell. What is true about the cell if the measured voltage is negative? Choose ? < ?, ? = ?, ? > ?, Need more info I. At 298.2 K, this reaction has an equilibrium constant K = 1.6 × 1013 . What is the standard molar free energy of reaction, ΔG° (in kJ/mol), for this reaction at 298.2 K?
Consider the balanced reaction:
2Cr3+(aq)+3PbO2(s)+6H2O(l)→2CrO42-(aq)+3Pb2+(aq)+4H3O+ (aq)
a.Which species is the oxidizing agent
b.What is the oxidation state of the O in CrO42-
c.What is the oxidation state of the Pb in PbO2?
d.How many valence electrons are in the CrO42- ion?
e. How many moles of electrons, ne, are transferred per mole of this reaction?
f. At a certain point the measured free energy is ∆?. Adding more PbO2 will cause the free energy change of the reaction, ∆G, to choose...(Increase, Stay the same, Decrease)
g. At a certain point the measured ∆G is –5 kJ/mol. Lowering the pH will cause the free energy change of the reaction, ∆?, to choose...
(become less negative, stay the same, become more negative)
h. The reaction is used to set up an
? < ?, ? = ?, ? > ?, Need more info
I. At 298.2 K, this reaction has an equilibrium constant K = 1.6 × 1013 . What is the standard molar free energy of reaction, ΔG° (in kJ/mol), for this reaction at 298.2 K?
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