Consider the metals in the following reactions.

2 Mg + O2 → 2 MgO
CuO + H2 → Cu + H2O
Ag+ + Cl− → AgCl

Which of the following is true?

1. Magnesium is oxidized, copper is reduced,
and silver is neither oxidized nor reduced.

2. Magnesium is oxidized; copper and silver
are reduced.

3. Magnesium is reduced; copper and silver
are neither oxidized nor reduced.

4. Magnesium and silver are oxidized; copper
is reduced.
1. Magnesium is oxidized, copper is reduced,
and silver is neither oxidized nor reduced.

The answer to your question is  the first option

Explanation:

Reactions

                            2 Mg + O₂ → 2 MgO

                            CuO + H₂ → Cu + H₂O

                            Ag+ + Cl− → AgCl

Process

1.- Determine the oxidation number of the elements

                            2 Mg⁰ + O₂⁰ → 2 Mg⁺²O

⁻²

                            Cu⁺²O⁻² + H₂⁰ → Cu⁰ + H₂⁺¹O

⁻²

                            Ag+ + Cl− → Ag⁺¹Cl⁻¹

2.- Determine if the metals were oxidized or reduced

Magnesium changed from 0 to +2                     oxidized

Copper changed from +2 to 0                            reduced

Silver changed from +1 to +1                                it did not change.

b. th3 n4zc4 pl4t3 15 c0nv3rg1ng w1th the s0uth 4m3ric4n pl4t3.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: