Question

1. consider the following reaction to answer the questions below: 8zn(s) + s₈(s) → 8zns(s).

a. identify the limiting reactant if you start with 5.00 mol of zn and 2.50 mol of s₈.

Explanation:

Step1: Determine mole - ratio from the balanced equation

The balanced equation is \(8Zn(s)+S_8(s)
ightarrow8ZnS(s)\). The mole - ratio of \(Zn\) to \(S_8\) is \(n_{Zn}:n_{S_8}=8:1\).

Step2: Calculate the moles of \(S_8\) required to react with the given \(Zn\)

Given \(n_{Zn} = 5.00\ mol\). Using the mole - ratio, the moles of \(S_8\) required to react completely with \(Zn\) is \(n_{S_8\ required}=\frac{5.00\ mol\ Zn}{8}=0.625\ mol\).

Step3: Compare the required and given moles of \(S_8\)

We are given \(n_{S_8\ given}=2.50\ mol\). Since \(0.625\ mol<2.50\ mol\), \(Zn\) will be completely consumed first.

Answer:

The limiting reactant is \(Zn\).