To determine the limiting reactant in a synthesis reaction, stoichiometric calculations are essential. These calculations rely on understanding the mole ratios of the reactants involved.
In the reaction given:
[tex]$
A + B \rightarrow C
$[/tex]
we need to identify the key ratio used in stoichiometry. Here are the given options:
1. Mole ratio of A to B: This is the ratio of the number of moles of reactant A required to react with a certain number of moles of reactant B. This ratio is crucial in determining stoichiometric proportions and, accordingly, the limiting reactant.
2. Mole ratio of B to A: While this is mathematically the inverse of the mole ratio of A to B, it serves the same purpose. However, for the context of determining limiting reactants directly, we usually refer to the mole ratio as provided directly from the balanced chemical equation.
3. Starting amount of C in grams: This value does not help in determining the limiting reactant directly as the product's initial quantity typically is zero before the reaction begins. Moreover, the stoichiometric calculations focus on the reactants' quantities to identify the limiting component.
4. Starting amount of A in moles: Knowing the starting amount of A in moles is important but it only gives half the information needed. We also need corresponding information about the amount of B and their respective stoichiometric ratios.
In conclusion, the value used to determine the limiting reactant for the reaction is the mole ratio of A to B. This ratio tells us how much of each reactant is required and enables us to identify the reactant that will be consumed first, thus limiting the extent of the reaction. Therefore, the correct answer is:
1. Mole ratio of A to B
