Textbook Problem

For each of the following balanced reactions, calculate how many moles of each product would be produced by complete conversion of 0.50 mole of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion.

msp;  $2{\text{H}}_2\text{O}\left(l\right)\to 2{\text{H}}_2\text{O}\left(l\right)+{\text{O}}_2\left(g\right)$

msp;  $2{\text{KClO}}_3\left(s\right)\to 2\text{KCl}\left(s\right)+3{\text{O}}_2\left(g\right)$

msp;  $2\text{Al}\left(s\right)+6\text{HCl}\left(aq\right)\to 2{\text{AlCl}}_3\left(aq\right)+3{\text{H}}_2\left(g\right)$

msp;  ${\text{C}}_3{\text{H}}_8\left(g\right)+5{\text{O}}_2\left(g\right)\to 3{\text{CO}}_2\left(g\right)+4{\text{H}}_2\text{O}\left(g\right)$