Final answer:
This question pertains to various concepts in Chemistry such as chemical equations, percent yield, molarity, and ionic compounds. The responses provided are factually accurate, addressing each statement in the given question.
Step-by-step explanation:
This series of questions falls within the subject of Chemistry, more specifically including topics such as chemical equations, percent yield, molarity, and ionic compounds. Let's break down each one.
k) In a balanced chemical equation, the number of moles of reactants doesn't necessarily equate to the number of moles of products - it's actually the atoms that must balance.
1) True, the percent yield in a chemical reaction can never exceed 100% because you can't get out more than you put in.
m) One mole of sodium chloride and one mole of calcium chloride do not have the same number of chlorine atoms, though one mole of each has the same number of formula units.
n) Not all ionic compounds are soluble in water. Some ionic compounds are insoluble, combining to form precipitates, or insoluble solids, in solution.
o) Correct, Molarity is defined as the number of moles of solute per liter of solution - not solvent.
p) Correct, strong electrolytes drastically ionize or dissociate in aqueous solution, yielding many ions.
q) The limiting reactant in a chemical reaction is not necessarily the reactant with the smallest mass but it's the reactant that is completely consumed when the reaction goes to completion.