Question

2. For the following reaction, calculate how many moles of each product are formed when 0.356

moles of Pbs completely react. Assume there is an excess of oxygen.
2PbS(s) + 302(g) → 2Pb0(s) + 2802(9)

Answer 1

`\large \boxed{\text{0.356 mol each of PbO and SO}_(2)}}`

Step-by-step explanation:

2PbS + 3O₂ ⟶ 2PbO + 2SO₂

n/mol: 0.356

1. Moles of PbO

2 mol of PbO are formed from 2 mol of PbS

`\text{Moles of PbO} = \text{0.356 mol PbS} * \frac{\text{2 mol PbO}}{\text{2 mol PbS}} = \textbf{0.356 mol PbO}`

2. Moles of SO₂

2 mol of SO₂ are formed from 2 mol of PbS

`\text{Moles of SO}_(2) = \text{0.356 mol PbS} * \frac{\text{2 mol SO}_(2)}{\text{2 mol PbS}} = \textbf{0.356 mol SO}_(2)\\\\\text{The reaction produces } \large\boxed{\textbf{0.356 mol of PbO and 0.356 mol of SO}_(2)}`