The scene below represents a mixture of A2 and B2 before they react to form $\mathrm{AB}_{3}$
(a) What is the limiting reactant?
(b) How many molecules of product can form?

Percent yields are generally calculated from masses. Would the result be the same if amounts (mol) were used instead? Why?

Reactants $A$ and $B$ form product $C .$ Draw a road map and write a Plan to find the mass (g) of $C$ when 25 g of A reacts with excess $B$

Reactants D and E form product F. Draw a road map and write a Plan to find the mass (g) of F when 27 g of D reacts with 31 g of E.

Chlorine gas can be made in the laboratory by the reaction of hydrochloric acid and manganese(IV) oxide:
$$
4 \mathrm{HCl}(a q)+\mathrm{MnO}_{2}(s) \longrightarrow \mathrm{MnCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{Cl}_{2}(g)
$$
When 1.82 mol of $\mathrm{HCl}$ reacts with excess $\mathrm{MnO}_{2},$ how many (a) moles of $\mathrm{Cl}_{2}$ and (b) grams of $\mathrm{Cl}_{2}$ form?