Question

For the following reaction, determine the limiting reactant for each of the initial amounts of reactants: 2Na(s) + Br2(g) → 2NaBr(s)

Option a) Na(s)
Option b) Br2(g)
Option c) NaBr(s)
Option d) Both Na(s) and Br2(g)

Answer 1

To determine the limiting reactant, compare the amounts of each reactant and their stoichiometric coefficients in the balanced equation. If the amount of a reactant is less than or equal to half its stoichiometric coefficient, it is the limiting reactant. Otherwise, it is in excess. In this reaction, either Na(s) or Br2(g) could be the limiting reactant depending on their initial amounts.

Step-by-step explanation:

In order to determine the limiting reactant in a chemical reaction, you need to compare the amounts of each reactant and their stoichiometric coefficients in the balanced equation.

For the reaction 2Na(s) + Br2(g) → 2NaBr(s), we need to compare the amounts of Na(s) and Br2(g) with their stoichiometric coefficients of 2.

Let's consider the initial amounts of Na(s) and Br2(g) separately:

1. For Na(s), if the amount is less than or equal to half the stoichiometric coefficient (2/2 = 1), Na(s) is the limiting reactant. Otherwise, if the amount is greater than half the stoichiometric coefficient, it is in excess.
2. For Br2(g), if the amount is less than or equal to half the stoichiometric coefficient (2/2 = 1), Br2(g) is the limiting reactant. Otherwise, if the amount is greater than half the stoichiometric coefficient, it is in excess.

Based on this analysis, the limiting reactant will be Na(s) if the initial amount of Na(s) is less than or equal to 1, and Br2(g) if the initial amount of Br2(g) is less than or equal to 1. If both initial amounts are greater than 1, then both Na(s) and Br2(g) are in excess.