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In an experiment, potassium chlorate decomposed according to the following chemical equation.
KCIO3 -- KCI + O2
(Molar mass of KClO3 = 122.5 g/mol; KCl = 74.55 g/mol; O2 = 31.998 g/mol)
If the mass of potassium chlorate was 240 grams, which of the following calculations can be used to determine the mass of oxygen gas formed

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Related questions

The decomposition of potassium chlorate can be used to produce oxygen gas in the laboratory: 2KClO3(s) ----> 2KCl(s) + 3O2(g)

What volume of gas, measured under STP conditions, can be produced by the decomposition of 12.7 g of KClO3(s)? (The molar mass of KClO3 is 122.5 g/mol)

A. 4.65L
B. 3.48L
C. 1.55L
D. 2.32L
E. 6.97L

What volume of oxygen, measured at STP, can be produced by the decomposition of potassium chlorate if 20.0 g of the salt (KClO3) is completely decomposed into potassium chloride and oxygen gas?

2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)

A- 2.44L B- 2.14L C- 3.66L D- 1.83L E- 5.48L

Determine the volume of O2 (at STP) formed when 50.0 g of KClO3 decomposes according to the following reaction. The molar mass for KClO3 is 122.55 g/mol. Please show all work.

2 KClO3(s) → 2 KCl(s) + 3 O2(g)

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