Identify the oxidation-reduction reactions among the following:
1. Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
2. 2Na(s) + Cl2(aq) → 2NaCl(s)
3. 2Mg(s) + O2(g) → 2MgO
1 and 2 only
2 and 3 only
1 and 3 only
All of 1, 2, and 3
None of 1, 2, and 3
Good Morning DrBob222, My answer is all of 1,2,and 3. Please let me know if I am on the right track.
2) 2na=2na+2e (oxidation)
Cl2+2e-=2Cl- (reduction)
3) 2Mg=Mg2+ +4e (oxidation)
O2+4e-=2O2 (oxidation)
Oxidation is the loss of electrons. Reduction is the gain of e.electrons.
For 1.
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
Zn on left has oxidation state (OS) of 0. Zn on right has(OS) of +2. So that's a loss of 2e which makes Zn to Zn^2+ oxidation.
Cu^2+ on the left has OS of 2+. On the right it is zero. That's a gain of 2e which makes Cu^2+ reduced.
So check out 2 and 3 and you can answer the question.
All of the reactions mentioned (1, 2, and 3) are oxidation-reduction (redox) reactions. So the correct answer is "All of 1, 2, and 3."
But hey, even though they're redox reactions, they're not exactly "redox-tacular." Maybe they should consider adding some pyrotechnics to make them more exciting? 😉
To identify the oxidation-reduction reactions among the given equations, you need to determine if there is a transfer of electrons between the reactants.
Let's analyze each equation:
1. Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
In this equation, zinc (Zn) is being oxidized because it loses two electrons to form Zn2+. Copper (Cu2+) is being reduced because it gains two electrons to form Cu. Therefore, equation 1 represents an oxidation-reduction reaction.
2. 2Na(s) + Cl2(aq) → 2NaCl(s)
In this equation, sodium (Na) is being oxidized because it loses one electron to form Na+. Chlorine (Cl2) is being reduced because it gains two electrons to form 2Cl-. Therefore, equation 2 represents an oxidation-reduction reaction.
3. 2Mg(s) + O2(g) → 2MgO
In this equation, magnesium (Mg) is being oxidized because it loses two electrons to form Mg2+. Oxygen (O2) is not being reduced because it does not gain any electrons. Therefore, equation 3 does not represent an oxidation-reduction reaction.
Based on the analysis, equations 1 and 2 represent oxidation-reduction reactions, while equation 3 does not. Therefore, the correct answer is:
1 and 2 only