50cm\(^{3}\) of sulphur (IV) oxide were produced at s.t.p. when some quantity of powdered sulphur were burnt in excess oxygen (a) Write the equation for the...
Question 1 Report
50cm\(^{3}\) of sulphur (IV) oxide were produced at s.t.p. when some quantity of powdered sulphur were burnt in excess oxygen
(a) Write the equation for the reaction
(b) Calculate the volume of oxygen used up during the reaction
(c) Which of the gas laws is applicable? State the law.
Answer Details
(a) Equation for the reaction
S(s) + O2(g) → SO2(g)
(b) Volume of oxygen used up
From the equation, the mole ratio of O2 to SO2 is 1 : 1. By Gay-Lussac's law of combining volumes, gases combine in volume ratios equal to their mole ratios (at the same temperature and pressure). Therefore:
1 volume of O2 produces 1 volume of SO2
Since 50 cm3 of SO2 is produced, the volume of oxygen used up = 50 cm3.
(c) Gas law applicable
Gay-Lussac's law of combining volumes. It states that when gases react, they do so in volumes which bear a simple whole number ratio to one another and to the volumes of the gaseous products, provided the temperature and pressure remain constant.
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