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Stoichiometry

Students perf...

Question

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 ( $M g O$ ) of the compound produced in the reaction.
$M g (s) + O_{2} (g) \to 2 M g O (s)$
$I$ . 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 $1 : 1$ ratio.

Statement

I

is true, Statement

I I

is true

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Statement

I

is true, Statement

I I

is false

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Statement

I

is false, Statement

I I

is true

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Statement

I

is false, Statement

I I

is false

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Statement

I

is true, Statement

I I

is true and is a correct explanation of the phenomena described in

I

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Solution

The correct option is A Statement $I$ is true, Statement $I I$ is true
Here,The reaction performed according to law of conservation of mass .the magnesium and oxygen should react in $1 : 1$ .
So, $0.24$ g of magnesium will react with $0.24$ of oxygen.

Suggest Corrections

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The correct option is A Statement I is true, Statement II is trueHere,The reaction performed according to law of conservation of mass .the magnesium and oxygen should react in 1:1.So, 0.24g of magnesium will react with 0.24 of oxygen.

The correct option is A Statement $I$ is true, Statement $I I$ is true
Here,The reaction performed according to law of conservation of mass .the magnesium and oxygen should react in $1 : 1$ .
So, $0.24$ g of magnesium will react with $0.24$ of oxygen.