1)
Li in reactant has oxidation state of 0
Li in product has oxidation state of +1
So, Li is getting oxidised.
The oxidation reaction is:
Li -> Li+ + e-
2)
H in reactant has oxidation state of 0
H in product has oxidation state of -1
So, H is getting reduced.
The reduction reaction is:
H2 + 2e- -> 2 H-
Be sure to answer all parts. Write the half-reactions for the following redox reaction: 2Li +...
Separate the following redox reactions into half-reactions, and label each half-reaction as oxidation or reduction. Part A Oxidation half-reaction for 2Li(s)+2H+(aq)→2Li+(aq)+H2(g). Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Oxidation half-reaction for 2Ag+(aq)+Be(s)→Be2+(aq)+2Ag(s). Express your answer as a chemical equation. Identify all of the phases in your answer.
Write the half reactions for the following redox reaction: 2Li + H2 ---> 2LiH Which is the oxidizing agent? Which is the reducing agent?
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Answer Write balanced half-reactions for the following redox reaction: reduction: 0 oxidation: Write balanced half-reactions for the following redox reaction: reduction: 0 oxidation:
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