2. consider the following reaction to answer the questions below: 8zn(s) + s₈(s) → 8zns(s).\n a. identify…

2. consider the following reaction to answer the questions below: 8zn(s) + s₈(s) → 8zns(s).\n a. identify the limiting reactant if you start with 5.00 mol of zn and 2.50 mol of s₈.

2. consider the following reaction to answer the questions below: 8zn(s) + s₈(s) → 8zns(s).\n a. identify the limiting reactant if you start with 5.00 mol of zn and 2.50 mol of s₈.

Answer

Explanation:

Step1: Determine mole - ratio from the balanced equation

The balanced equation is (8Zn(s)+S_8(s)\rightarrow8ZnS(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).