Answer :
To determine the correct balanced equation for the production of solid cobalt (III) chloride ([tex]\(CoCl_3\)[/tex]) when cobalt reacts with chlorine, we need to analyze each of the given options carefully:
1. Option A:
[tex]\[ 2 Co (s) + 3 Cl_2(s) \rightarrow 2 CoCl_3(s) \][/tex]
2. Option B:
[tex]\[ 2 Co (s) + 3 Cl_2(l) \rightarrow 2 CoCl_3(s) \][/tex]
3. Option C:
[tex]\[ Co (s) + Cl_2(0) \rightarrow CoCl_2(s) \][/tex]
4. Option D:
[tex]\[ Co (s) + 3 Cll (s) \rightarrow CoCl_3(s) \][/tex]
5. Option E:
[tex]\[ Co (s) + Cl_2(g) \rightarrow CoCl_2(s) \][/tex]
Now let's examine each option:
- Option A:
This equation is balanced and indicates the reaction between solid cobalt (s) and chlorine gas (Cl[tex]\(_2\)[/tex] in the solid state), producing solid cobalt (III) chloride (CoCl[tex]\(_3\)[/tex]). However, chlorine is typically in the gaseous state at room temperature.
- Option B:
This equation is similar to Option A but specifies chlorine in the liquid state (Cl[tex]\(_2(l)\)[/tex]), which is unusual for typical conditions, making this less likely.
- Option C:
This equation suggests cobalt reacting with an undefined form of chlorine (Cl[tex]\(_2(0)\)[/tex]), producing cobalt (II) chloride (CoCl[tex]\(_2\)[/tex]). This doesn't yield CoCl[tex]\(_3\)[/tex] as required.
- Option D:
This equation has chlorine represented incorrectly with "Cll." There's no known form of chlorine denoted this way in standard chemistry, making this incorrect.
- Option E:
This equation reacts cobalt with chlorine gas (Cl[tex]\(_2(g)\)[/tex]) to form cobalt (II) chloride (CoCl[tex]\(_2\)[/tex]), not cobalt (III) chloride (CoCl[tex]\(_3\)[/tex]).
The most accurate representation of cobalt reacting with chlorine gas to form solid cobalt (III) chloride is therefore:
[tex]\[ 2 Co (s) + 3 Cl_2(g) \rightarrow 2 CoCl_3(s) \][/tex]
This matches with Option A:
[tex]\[ 2 Co (s) + 3 Cl_2 (s) \rightarrow 2 CoCl_3 (s) \][/tex]
Thus, the correct answer is:
[tex]\[ 1 \][/tex]
This explains that Option A is indeed the correct balanced equation for the reaction to produce cobalt (III) chloride.
1. Option A:
[tex]\[ 2 Co (s) + 3 Cl_2(s) \rightarrow 2 CoCl_3(s) \][/tex]
2. Option B:
[tex]\[ 2 Co (s) + 3 Cl_2(l) \rightarrow 2 CoCl_3(s) \][/tex]
3. Option C:
[tex]\[ Co (s) + Cl_2(0) \rightarrow CoCl_2(s) \][/tex]
4. Option D:
[tex]\[ Co (s) + 3 Cll (s) \rightarrow CoCl_3(s) \][/tex]
5. Option E:
[tex]\[ Co (s) + Cl_2(g) \rightarrow CoCl_2(s) \][/tex]
Now let's examine each option:
- Option A:
This equation is balanced and indicates the reaction between solid cobalt (s) and chlorine gas (Cl[tex]\(_2\)[/tex] in the solid state), producing solid cobalt (III) chloride (CoCl[tex]\(_3\)[/tex]). However, chlorine is typically in the gaseous state at room temperature.
- Option B:
This equation is similar to Option A but specifies chlorine in the liquid state (Cl[tex]\(_2(l)\)[/tex]), which is unusual for typical conditions, making this less likely.
- Option C:
This equation suggests cobalt reacting with an undefined form of chlorine (Cl[tex]\(_2(0)\)[/tex]), producing cobalt (II) chloride (CoCl[tex]\(_2\)[/tex]). This doesn't yield CoCl[tex]\(_3\)[/tex] as required.
- Option D:
This equation has chlorine represented incorrectly with "Cll." There's no known form of chlorine denoted this way in standard chemistry, making this incorrect.
- Option E:
This equation reacts cobalt with chlorine gas (Cl[tex]\(_2(g)\)[/tex]) to form cobalt (II) chloride (CoCl[tex]\(_2\)[/tex]), not cobalt (III) chloride (CoCl[tex]\(_3\)[/tex]).
The most accurate representation of cobalt reacting with chlorine gas to form solid cobalt (III) chloride is therefore:
[tex]\[ 2 Co (s) + 3 Cl_2(g) \rightarrow 2 CoCl_3(s) \][/tex]
This matches with Option A:
[tex]\[ 2 Co (s) + 3 Cl_2 (s) \rightarrow 2 CoCl_3 (s) \][/tex]
Thus, the correct answer is:
[tex]\[ 1 \][/tex]
This explains that Option A is indeed the correct balanced equation for the reaction to produce cobalt (III) chloride.
