Answer :
Sure, let's analyze each reaction step-by-step to determine which one is a redox reaction (one that involves a change in oxidation states due to the transfer of electrons).
### A. [tex]\( AgNO_3 + LiCl \rightarrow AgCl + LiNO_3 \)[/tex]
1. Identify the oxidation states:
- [tex]\(AgNO_3\)[/tex]:
- [tex]\(Ag\)[/tex] is +1
- [tex]\(NO_3^-\)[/tex]: [tex]\(N\)[/tex] is +5, [tex]\(O\)[/tex] is -2
- [tex]\(LiCl\)[/tex]:
- [tex]\(Li\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(AgCl\)[/tex]:
- [tex]\(Ag\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(LiNO_3\)[/tex]:
- [tex]\(Li\)[/tex] is +1
- [tex]\(NO_3^-\)[/tex]: [tex]\(N\)[/tex] is +5, [tex]\(O\)[/tex] is -2
2. Check for changes in oxidation states:
- All elements maintain their oxidation states before and after the reaction.
- [tex]\(Ag\)[/tex] remains +1, [tex]\(Li\)[/tex] remains +1, [tex]\(Cl\)[/tex] remains -1, [tex]\(N\)[/tex] remains +5, [tex]\(O\)[/tex] remains -2.
Since there are no changes in oxidation states, this is not a redox reaction.
### B. [tex]\( HCl + LiOH \rightarrow LiCl + H_2O \)[/tex]
1. Identify the oxidation states:
- [tex]\(HCl\)[/tex]:
- [tex]\(H\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(LiOH\)[/tex]:
- [tex]\(Li\)[/tex] is +1
- [tex]\(OH^-\)[/tex]: [tex]\(O\)[/tex] is -2, [tex]\(H\)[/tex] is +1
- [tex]\(LiCl\)[/tex]:
- [tex]\(Li\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(H_2O\)[/tex]:
- [tex]\(H\)[/tex] is +1
- [tex]\(O\)[/tex] is -2
2. Check for changes in oxidation states:
- All elements maintain their oxidation states before and after the reaction.
- [tex]\(H\)[/tex] remains +1, [tex]\(Li\)[/tex] remains +1, [tex]\(Cl\)[/tex] remains -1, [tex]\(O\)[/tex] remains -2.
Since there are no changes in oxidation states, this is not a redox reaction.
### C. [tex]\( 2 NaBr + Cl_2 \rightarrow 2 NaCl + Br_2 \)[/tex]
1. Identify the oxidation states:
- [tex]\(NaBr\)[/tex]:
- [tex]\(Na\)[/tex] is +1
- [tex]\(Br\)[/tex] is -1
- [tex]\(Cl_2\)[/tex]:
- [tex]\(Cl\)[/tex] is 0
- [tex]\(NaCl\)[/tex]:
- [tex]\(Na\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(Br_2\)[/tex]:
- [tex]\(Br\)[/tex] is 0
2. Check for changes in oxidation states:
- The bromine ([tex]\(Br\)[/tex]) in [tex]\(NaBr\)[/tex] changes from -1 to 0.
- The chlorine ([tex]\(Cl\)[/tex]) in [tex]\(Cl_2\)[/tex] changes from 0 to -1.
Since there are changes in oxidation states ([tex]\(Br\)[/tex] from -1 to 0 and [tex]\(Cl\)[/tex] from 0 to -1), this reaction involves the transfer of electrons and is indeed a redox reaction.
### D. [tex]\( HNO_3 + KOH \rightarrow KCl + H_2O \)[/tex]
1. Identify the oxidation states:
- [tex]\(HNO_3\)[/tex]:
- [tex]\(H\)[/tex] is +1
- [tex]\(N\)[/tex] is +5
- [tex]\(O\)[/tex] is -2
- [tex]\(KOH\)[/tex]:
- [tex]\(K\)[/tex] is +1
- [tex]\(OH^-\)[/tex]: [tex]\(O\)[/tex] is -2, [tex]\(H\)[/tex] is +1
- [tex]\(KCl\)[/tex]:
- [tex]\(K\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(H_2O\)[/tex]:
- [tex]\(H\)[/tex] is +1
- [tex]\(O\)[/tex] is -2
2. Check for changes in oxidation states:
- All elements maintain their oxidation states before and after the reaction.
- [tex]\(H\)[/tex] remains +1, [tex]\(K\)[/tex] remains +1, [tex]\(Cl\)[/tex] remains -1, [tex]\(N\)[/tex] remains +5, [tex]\(O\)[/tex] remains -2.
Since there are no changes in oxidation states, this is not a redox reaction.
### Conclusion
After analyzing each equation, we can determine that the equation representing a redox reaction is:
C. [tex]\(2 NaBr + Cl_2 \rightarrow 2 NaCl + Br_2\)[/tex]
### A. [tex]\( AgNO_3 + LiCl \rightarrow AgCl + LiNO_3 \)[/tex]
1. Identify the oxidation states:
- [tex]\(AgNO_3\)[/tex]:
- [tex]\(Ag\)[/tex] is +1
- [tex]\(NO_3^-\)[/tex]: [tex]\(N\)[/tex] is +5, [tex]\(O\)[/tex] is -2
- [tex]\(LiCl\)[/tex]:
- [tex]\(Li\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(AgCl\)[/tex]:
- [tex]\(Ag\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(LiNO_3\)[/tex]:
- [tex]\(Li\)[/tex] is +1
- [tex]\(NO_3^-\)[/tex]: [tex]\(N\)[/tex] is +5, [tex]\(O\)[/tex] is -2
2. Check for changes in oxidation states:
- All elements maintain their oxidation states before and after the reaction.
- [tex]\(Ag\)[/tex] remains +1, [tex]\(Li\)[/tex] remains +1, [tex]\(Cl\)[/tex] remains -1, [tex]\(N\)[/tex] remains +5, [tex]\(O\)[/tex] remains -2.
Since there are no changes in oxidation states, this is not a redox reaction.
### B. [tex]\( HCl + LiOH \rightarrow LiCl + H_2O \)[/tex]
1. Identify the oxidation states:
- [tex]\(HCl\)[/tex]:
- [tex]\(H\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(LiOH\)[/tex]:
- [tex]\(Li\)[/tex] is +1
- [tex]\(OH^-\)[/tex]: [tex]\(O\)[/tex] is -2, [tex]\(H\)[/tex] is +1
- [tex]\(LiCl\)[/tex]:
- [tex]\(Li\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(H_2O\)[/tex]:
- [tex]\(H\)[/tex] is +1
- [tex]\(O\)[/tex] is -2
2. Check for changes in oxidation states:
- All elements maintain their oxidation states before and after the reaction.
- [tex]\(H\)[/tex] remains +1, [tex]\(Li\)[/tex] remains +1, [tex]\(Cl\)[/tex] remains -1, [tex]\(O\)[/tex] remains -2.
Since there are no changes in oxidation states, this is not a redox reaction.
### C. [tex]\( 2 NaBr + Cl_2 \rightarrow 2 NaCl + Br_2 \)[/tex]
1. Identify the oxidation states:
- [tex]\(NaBr\)[/tex]:
- [tex]\(Na\)[/tex] is +1
- [tex]\(Br\)[/tex] is -1
- [tex]\(Cl_2\)[/tex]:
- [tex]\(Cl\)[/tex] is 0
- [tex]\(NaCl\)[/tex]:
- [tex]\(Na\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(Br_2\)[/tex]:
- [tex]\(Br\)[/tex] is 0
2. Check for changes in oxidation states:
- The bromine ([tex]\(Br\)[/tex]) in [tex]\(NaBr\)[/tex] changes from -1 to 0.
- The chlorine ([tex]\(Cl\)[/tex]) in [tex]\(Cl_2\)[/tex] changes from 0 to -1.
Since there are changes in oxidation states ([tex]\(Br\)[/tex] from -1 to 0 and [tex]\(Cl\)[/tex] from 0 to -1), this reaction involves the transfer of electrons and is indeed a redox reaction.
### D. [tex]\( HNO_3 + KOH \rightarrow KCl + H_2O \)[/tex]
1. Identify the oxidation states:
- [tex]\(HNO_3\)[/tex]:
- [tex]\(H\)[/tex] is +1
- [tex]\(N\)[/tex] is +5
- [tex]\(O\)[/tex] is -2
- [tex]\(KOH\)[/tex]:
- [tex]\(K\)[/tex] is +1
- [tex]\(OH^-\)[/tex]: [tex]\(O\)[/tex] is -2, [tex]\(H\)[/tex] is +1
- [tex]\(KCl\)[/tex]:
- [tex]\(K\)[/tex] is +1
- [tex]\(Cl\)[/tex] is -1
- [tex]\(H_2O\)[/tex]:
- [tex]\(H\)[/tex] is +1
- [tex]\(O\)[/tex] is -2
2. Check for changes in oxidation states:
- All elements maintain their oxidation states before and after the reaction.
- [tex]\(H\)[/tex] remains +1, [tex]\(K\)[/tex] remains +1, [tex]\(Cl\)[/tex] remains -1, [tex]\(N\)[/tex] remains +5, [tex]\(O\)[/tex] remains -2.
Since there are no changes in oxidation states, this is not a redox reaction.
### Conclusion
After analyzing each equation, we can determine that the equation representing a redox reaction is:
C. [tex]\(2 NaBr + Cl_2 \rightarrow 2 NaCl + Br_2\)[/tex]
