객관식
Determine the standard cell potential, E^ext{°}_{ext{cell}}, for the reaction: Al(s) + 3 Ag^+(aq) → 3 Ag(s) + Al^{3+}(aq). Given: E^ext{°}_{ext{Al}^{3+}/ext{Al}} = -1.66 ext{ V}, E^ext{°}_{ext{Ag}^+/ext{Ag}} = +0.80 ext{ V}.
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6. Chemical Quantities & Aqueous Reactions
Redox Reactions
Multiple Choice
Which of the following balanced equations represents a redox (oxidation-reduction) reaction?
A
CaCO_3 ightarrow CaO + CO_2
B
2Na + Cl_2 ightarrow 2NaCl
C
AgNO_3 + NaCl ightarrow AgCl + NaNO_3
D
HCl + NaOH ightarrow NaCl + H_2O
검증된 단계별 안내1
Step 1: Understand what a redox reaction is. A redox (oxidation-reduction) reaction involves the transfer of electrons between species, resulting in changes in oxidation states of elements.
Step 2: Examine each equation and identify if there is a change in oxidation states of any element from reactants to products.
Step 3: For the equation \(\mathrm{CaCO_3 \rightarrow CaO + CO_2}\), check the oxidation states of calcium, carbon, and oxygen on both sides to see if any element is oxidized or reduced.
Step 4: For the equation \(\mathrm{2Na + Cl_2 \rightarrow 2NaCl}\), determine the oxidation states of sodium and chlorine before and after the reaction to see if electron transfer occurs.
Step 5: For the other equations, \(\mathrm{AgNO_3 + NaCl \rightarrow AgCl + NaNO_3}\) and \(\mathrm{HCl + NaOH \rightarrow NaCl + H_2O}\), analyze if any oxidation state changes occur, indicating redox, or if they are simply double displacement or acid-base neutralization reactions.
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