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# Answer to Question #171372 in Inorganic Chemistry for thibhashini segeran

Question #171372

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

2

KClO3               2 KCl + 3 O2

i.        If 1.50 mol of KClO3 decomposes, what is the mass of O2 that will be produced?

1
2021-03-15T09:29:11-0400

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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