Question #171372

**b) Answer the following stoichiometry questions by referring to the equation below: **

**2 **

**KClO**_{3}** 2 KCl + 3 O**_{2}** **

**i. If 1.50 mol of KClO**_{3}** decomposes, what is the mass of O**_{2}** that will be produced? **

Expert's answer

This is a problem of determining mole ratios in the stoichiometric equations.

(i) Mass of O2

We have moles of KClO3 = 1.50mol

Mole ratios of KClO3 : O2 = 2:3

Thus moles of O2

= 2.25mol of O2

Moles

Therefore Mass of O2 = Moles x MM

= 2.25mol x 32g/mol

= 72g

(ii) Moles of KClO3

Moles of O2

Mole ratios of O2:KClO3 = 3:2

Moles of KClO3

(ii)Mass of KClO3

We are given moles of KCl = 2.75mol

Mole ratios of KCl : KClO3 = 2:2

Thus moles of KClO3

Mass = Moles x MM

= 2.75mol x 122.55g/mol

= 337.013g

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