Chapter 9, Problem 43QAP

Consider the equation: $2\text{A}+\text{B}\to \text{5C}$. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant determined? Choose the best answer and explain.

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Choose the reactant with the smallest coefficient in the balanced chemical equation. So in this case, the limiting reactant is B.

Choose the reactant with the smallest mass given. So in this case, the limiting reactant is

The mass of each reactant must be converted to moles and then compared to the ratios in the balanced chemical equation. So in this case, the limiting reactant cannot be determined without the molar masses of A and B.

The mass of each reactant must he converted to moles first. The reactant with the fewest moles present is the limiting reactant. So in this case, the limiting reactant cannot be determined without the molar masses of A and B.

The mass of each reactant must be divided by their coefficients in the balanced chemical equation, and the smallest number present is the limiting reactant. So in this case, there is no limiting reactant because A and B arc used up perfectly.