Multiple Choice
Provide the products from the reaction between 2 moles of antimony with four moles of chlorine.
2 Sb(s) + 4 Cl2 →
23. Chemistry of the Nonmetals
Nitrogen Family Reactions
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Identify the reducing agent in the reaction of hydrazine and hydrogen peroxide to form nitrogen gas and water vapor.
N2H4 (l) + 2 H2O2 (l) → N2 (g) + 4 H2O (g)
A
N2H4
B
H2O2
C
N2
D
H2O
E
cannot be determined
Verified step by step guidance1
Identify the oxidation states of each element in the reactants and products. For hydrazine (N2H4), nitrogen typically has an oxidation state of -2. For hydrogen peroxide (H2O2), oxygen has an oxidation state of -1.
Determine the oxidation states of the elements in the products. In nitrogen gas (N2), nitrogen has an oxidation state of 0. In water (H2O), oxygen has an oxidation state of -2.
Compare the changes in oxidation states from reactants to products. If an element's oxidation state increases, it is oxidized and acts as the reducing agent.
Observe that nitrogen in N2H4 goes from an oxidation state of -2 to 0, indicating it is oxidized. This means N2H4 is the reducing agent.
Conclude that the reducing agent is the species that donates electrons, which in this reaction is N2H4, as it undergoes oxidation by increasing its oxidation state.
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