Sulphur burns in air to form sulphur dioxide: #S + O_2 -> SO_2#. What is the mass of sulphur that must be burned to produce 64g of sulphur dioxide?

1 Answer
anor277
Jan 26, 2017

About #32*g#.

Explanation:

This problem uses your understanding of equivalent mass. The combustion of sulfur may be represented by the following equation:

#underbrace(S(s) + O_2(g) rarr SO_2(g))_"64 g of reactant gives 64 g of product"#

And given molar masses, the reaction EXPLICITLY states that #32*g# of sulfur is oxidized by #32*g# to give #64*g# of sulfur dioxide - these are all the equivalent masses of the reactants and products, which contain stoichiometric quantities of reactant and product.

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