Sulphur burns in air to form sulphur dioxide: $S + O_{2} \to S O_{2}$ $S + O_2 -> SO_2$ . What is the mass of sulphur that must be burned to produce 64g of sulphur dioxide?

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Sulphur burns in air to form sulphur dioxide: $S + O_{2} \to S O_{2}$ $S + O_2 -> SO_2$ . What is the mass of sulphur that must be burned to produce 64g of sulphur dioxide?

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Answer 1 · 2017-01-26T10:48:16

About $32 \cdot g$ $32*g$ .

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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Sulphur burns in air to form sulphur dioxide: $S + O_{2} \to S O_{2}$ $S + O_2 -> SO_2$ . What is the mass of sulphur that must be burned to produce 64g of sulphur dioxide?

1 Answer

Explanation:

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Sulphur burns in air to form sulphur dioxide: S + O_2 -> SO_2S+O2→SO2S + O_2 -> SO_2. What is the mass of sulphur that must be burned to produce 64g of sulphur dioxide?

1 Answer

Explanation:

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Sulphur burns in air to form sulphur dioxide: $S + O_{2} \to S O_{2}$ $S + O_2 -> SO_2$ . What is the mass of sulphur that must be burned to produce 64g of sulphur dioxide?