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.

Related questions
See all questions in Atomic Mass
Impact of this question
27560 views around the world
You can reuse this answer
Creative Commons License