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Laws of Mass Conservation

When 0.0976 g...

Question

When 0.0976 g of magnesium was heated in air, 0.1627 g of magnesium oxide $(M g O)$ was produced. What is the mass of oxygen needed to produce 0.1627 g of $M g O$ ?

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Solution

Total mass of reactants = Total mass of products
Mass of $M g$ + Mass of $O$ = Mass of $M g O$
$0.0976 g$ + mass of $O = 0.1627 g$
Mass of $O = 0.1627 - 0.0976 = 0.0651 g$

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Similar questions

Q. When 0.0976 g of magnesium was heated in air, 0.1627 g of magnesium oxide

(M g O)

was produced. What is the mass of oxygen needed to produce 0.1627 g of

M g O

?

M g + O_{2} \to M g O

0.486 g

of magnesium is fully oxidized, what mass of magnesium oxide should be produced?

Q. Students perform an experiment in which the mass of a sample of

M g

is vigorously heated so that it reacts with oxygen to form magnesium oxide. The purpose of the experiment is to verify the formula unit (

M g O

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M g (s) + O_{2} (g) \to 2 M g O (s)

I

. The students find their initial sample of magnesium had a mass of

0.24 g

and the ending mass of the magnesium oxide was

0.48 g

. The students obtained an ending mass of

M g O

which matches perfectly with the ration predicted by the balanced equation.
BECAUSE

I I

. The magnesium and oxygen should react in a

1 : 1

Q. A certain amount of water is dissociated to produce oxygen which was just sufficient to burn magnesium to form 400 g of magnesium oxide. Calculate the amount of water dissociated.

Q. Question 3
Magnesium ribbon on burning in air produces

(a) magnesium oxide, water and light
(b) magnesium oxide and heat
(c) magnesium oxide, heat and light
(d) magnesium oxide, water and heat

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