Calcium metal (Ca) can be produced by passing an electric current through molten calcium chloride (#CaCl_2#). Chlorine gas (#Cl_2#) is also formed. What is the balanced equation for this reaction?

Question

Henry Antrim · Accepted Answer

#CaCl_2(l) +Deltararr Ca(l) + Cl_2(g)#

Tick. Is the mass and charge balanced? Tick.

If either quantity was unbalanced, we could not accept the equation as a legitimate representation of reality. What does the #Delta# symbol represent? Is this a redox reaction?

HIX Tutor · Answer

undefined To write the balanced equation for the reaction of molten calcium chloride (CaCl₂) to produce calcium metal (Ca) and chlorine gas (Cl₂), follow these steps:

1. **Write the unbalanced equation**:
   $$
   \text{CaCl}_2 \rightarrow \text{Ca} + \text{Cl}_2
   $$

2. **Count the atoms on each side**:
   - Left side: 1 calcium (Ca) and 2 chlorine (Cl)
   - Right side: 1 calcium (Ca) and 2 chlorine (Cl in Cl₂)

3. **Balance the chlorine atoms**:
   The chlorine is already balanced because there are 2 Cl on the left and 2 Cl in Cl₂ on the right.

4. **Confirm calcium is balanced**:
   There is 1 calcium on both sides.

5. **Final balanced equation**:
   $$
   \text{CaCl}_2 \rightarrow \text{Ca} + \text{Cl}_2
   $$

So, the final balanced equation is:
$$
\text{CaCl}_2 \rightarrow \text{Ca} + \text{Cl}_2
$$
Great job!

Cooper Anderson · Answer

undefined $$ \text{CaCl}_2 (\text{molten}) \rightarrow \text{Ca} (\text{s}) + \text{Cl}_2 (\text{g}) $$