Answer
Balanced equation:
$2Sb(s) + 3Cl_2(g) --\gt 2SbCl_3(s)$
Reaction type: Combination.
Work Step by Step
1. Count the atoms of each element in both sides of the reaction.
$Sb(s) + Cl_2(g) --\gt SbCl_3(s)$
Reactants: $Sb = 1$ and $Cl = 2$
Products: $Sb = 1$ and $Cl = 3$
2. Balance the number of chlorines, by putting a "3" in front of $Cl_2$, and a "2" as the coefficient of $SbCl_3$.
$Sb(s) + 3Cl_2(g) --\gt 2SbCl_3(s)$
3. Balance the number of antimony atoms, by putting a "2" in front of $Sb$
$2Sb(s) + 3Cl_2(g) --\gt 2SbCl_3(s)$
4. Classify the reaction.
That reaction follows the pattern of a combination reaction (A + B $--\gt$ AB). Where two compounds/elements combine to form a single product.
