Question

Please help!!
During an investigation a scientist burned 48 g of magnesium strip. After the reaction the total mass of the product formed was found to be 80 g. Does the law of
conservation of mass hold true in this case? Use complete sentences to justify your answer based on numerical calculations.

Answer 1

Answer:

yes, the law of conservation of mass hold true in this case burning magnesium strip is explained by this equation 2 Mg (s) + O2 (g) -> MgO (s)So the lighter magnesium, after reacting with oxygen in air, forms the heavier magnesium oxide. molar mass of magnesium and magnesium oxide are 24g and 40g respectively. So the same ratio 24:40 (i.e. 3:5) is maintained in the given masses of 48g and 80g, which means mass is conserved in the reacion.

Explanation:

Brainiest Please!!!

Answer 2

For the given scenario, the law of conservation of mass does holds true.

Given:

Mass of magnesium = 48 g

Mass of product = 80 g

• The Law of conservation of mass states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form.

• Total mass on both sides of the reaction (reactant side as well as product side) remains the same.

Total mass of the reactants = Total mass of the products

The balanced chemical reaction for the burning of magnesium strip in air follows:

$2Mg+O_2\rightarrow 2MgO$

Mass of the reactants = Mass of Mg + mass of $O_2$

Mass of the products = Mass of MgO

Putting values in the equation:

$48+\text{ Mass of O}_2=80\\\\\text{ Mass of O}_2=80-48\\\\\text{ Mass of O}_2=32\text{ g}$

The hidden mass of the reactant is the mass of oxygen comsumed. Thus, the formation of magnesium oxide by burning of magnesium follows the law.

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