Answer
The balanced equation for that reaction is:
$2Cl_2(g) + O_2(g) --\gt 2OCl_2(g)$
Work Step by Step
1. As we have determined in 7.81a, the reactants are: $Cl_2$ and $O_2$, and the product is: $OCl_2$.
- Write the unbalanced equation:
$Cl_2(g) + O_2(g) --\gt OCl_2(g)$
2. Balance the number of oxygen atoms, by putting a "2" as the coefficient of $OCl_2$.
$Cl_2(g) + O_2(g) --\gt 2OCl_2(g)$
3. Balance the number of chlorine atoms, by putting a "2" as the coefficient of $Cl_2$.
$2Cl_2(g) + O_2(g) --\gt 2OCl_2(g)$
- The equation is balanced.
