Respuesta :
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.
Explanation:
The balanced chemical equation is:
[tex]S+O_2\rightarrow SO_2[/tex]
To calculate the moles :
[tex]\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}[/tex]
[tex]\text{Moles of sulphur}=\frac{2\times 1000g}{32}=62.5moles[/tex]
According to stoichiometry :
a) 1 mole of sulphur require = 1 mole of [tex]O_2[/tex]
Thus 62.5 moles of sulphur will require=[tex]\frac{1}{1}\times 62.5=62.5moles[/tex] of [tex]O_2[/tex]
Mass of [tex]O_2=moles\times {\text {Molar mass}}=62.5moles\times 32g/mol=2000g=2kg[/tex]
b) As 1 moles of sulphur give = 1 mole of [tex]SO_2[/tex]
Thus 62.5 moles of sulphur give =[tex]\frac{1}{1}\times 62.5=62.5moles[/tex] of [tex]SO_2[/tex]
Mass of [tex]SO_2=moles\times {\text {Molar mass}}=62.5moles\times 64g/mol=4000g=4kg[/tex]
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.
