Question

Trace amounts of sulfur (S) in coal are burned in the presence of diatomic oxygen (O2) to form sulfur dioxide (SO2). Determine the minimum mass of oxygen required in the reactants and the mass of sulfur dioxide in the products when 2 kg of sulfur is burned.

Answer 1

Answer: Thus 2 kg of oxygen is required in the reactants and 4 kg of sulfur dioxide in the products when 2 kg of sulfur is burned.

Step-by-step explanation:

The balanced chemical equation is:

`S+O_2\rightarrow SO_2`

To calculate the moles :

`\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}`

`\text{Moles of sulphur}=(2* 1000g)/(32)=62.5moles`

According to stoichiometry :

a) 1 mole of sulphur require = 1 mole of
`O_2`

Thus 62.5 moles of sulphur will require=
`(1)/(1)* 62.5=62.5moles` of
`O_2`

Mass of
`O_2=moles* {\text {Molar mass}}=62.5moles* 32g/mol=2000g=2kg`

b) As 1 moles of sulphur give = 1 mole of
`SO_2`

Thus 62.5 moles of sulphur give =
`(1)/(1)* 62.5=62.5moles` of
`SO_2`

Mass of
`SO_2=moles* {\text {Molar mass}}=62.5moles* 64g/mol=4000g=4kg`

Thus 2 kg of oxygen is required in the reactants and 4 kg of sulfur dioxide in the products when 2 kg of sulfur is burned.