Oxidation Reduction

What is the oxidation number of Cl in HCl?

What is the oxidation number of Al in AlCl₃?

What is the oxidation number of Cl in Cl₂?

What is the oxidation number of Cl in HClO?

What is the oxidation number of Na in NaOH?

What is the oxidation number of Fe in Fe(OH)₂?

What is the oxidation number of Fe in FeO^–?

What is the oxidation number of carbon in CH₄?

What is the oxidation number of Cr in CaCr₂O₇?

In the following reaction what happens to the oxidation state of iron (Fe)?

 Fe₂O₃ + 3CO → 2Fe + 3CO₂

In the following reaction what happens to the oxidation state of oxygen during the decomposition of hydrogen peroxide?

 2H₂O₂ → 2H₂O + O₂

The net reaction for glycolysis is shown below: 

Glucose + 2 NAD⁺ + 2 ADP + 2 P_i → 2 Pyruvate + 2 NADH + 2H⁺ + 2 ATP

What is reduced in the following reaction?

CH₃OH is reacted with KMnO₄ to yield COOH. Which of the following was oxidized?

In the pentose phosphate pathway, Glucose-6-Phosphate is converted to Gluconate-6-Phosphate and NADP is converted to NADPH. Which reactant is oxidized and which is reduced?

The E_red of Fe/Fe²⁺ is -0.44 V and the E_red of Ag/Ag⁺ is +0.80 V. Which of the following is most likely to be reduced?

Which of the following is most likely to be reduced given the following reduction values?

Cu/Cu²⁺ = +0.34 V
Pb/Pb²⁺ = -0.13 V
Al/Al²⁺ = -1.66 V
Li/Li⁺ = -3.05 V

Which of the following is most likely to be oxidized given the following reduction potentials?

Cd/Cd²⁺ = -0.41 V
Pb/Pb ²⁺ = -0.13 V
Zn/Zn²⁺ = -0.76 V
Au/Au³⁺ = +1.69 V

Which of the following reactions would take place if Zn²⁺_(aq), Zn_(s), Fe_(s), and Fe³⁺_(aq) were added to a container? (Note: E_red of Fe/Fe³⁺ = -0.06 V and E_red of Zn/Zn²⁺ = -0.44 V)

If Pb²⁺_(aq), Pb_(s), Zn²⁺_(aq), and Zn_(s) were placed into a beaker. Which of the following reactions would occur? (Note: E_red Pb/Pb²⁺ = -0.13 V and E_red Zn/Zn²⁺ = -0.44 V)

Given the following reduction potentials which of the following would be the best oxidizing agent?

Cd/Cd²⁺ = -0.41 V
Pb/Pb²⁺ = -0.13 V
Zn/Zn²⁺ = -0.76 V
Au/Au³⁺ = +1.69 V

Given the following reduction potentials which of the following would be the strongest reducing agent?

Cu/Cu²⁺ = +0.34 V
Pb/Pb²⁺ = -0.13 V
Al/Al²⁺ = -1.66 V
Li/Li⁺ = -3.05 V

If the oxidation number of an atom goes from 0 to -3 then this element acted as a?

If the oxidation number of an atom goes from 0 to +1 then this element acted as a:

Which of the following is the oxidizing agent for the given reaction below?

Zn_(s) + H⁺_(aq) → Zn²⁺_(aq) + H_2(g)