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Chapter 2: Problem 3

A 0.406 g sample of magnesium reacts with oxygen, producing \(0.674 \mathrm{g}\) of magnesium oxide as the only product. What mass of oxygen was consumed in the reaction?

Short Answer

Expert verified
The mass of oxygen that was consumed in the reaction is \(0.268 \mathrm{g}\).

Step by step solution

01

Understanding the Conservation of Mass

The law of conservation of mass states that matter cannot be created nor destroyed. Therefore, the sum of the masses of the reactants, magnesium and oxygen, before the reaction must be equal to the sum of the masses of the products, in this case magnesium oxide, after the reaction.
02

Calculate the mass of Oxygen

The problem provides the masses of magnesium (\(0.406 \, \mathrm{g}\)) and of magnesium oxide (\(0.674 \, \mathrm{g}\)) produced. The difference in mass between the magnesium oxide produced and the magnesium used will be the mass of oxygen involved in the reaction. So, subtract the mass of magnesium from the mass of magnesium oxide to find the mass of oxygen: \(0.674 \mathrm{g} - 0.406 \mathrm{g} = 0.268 \mathrm{g}\).
03

Concluding the solution

So, the mass of oxygen consumed in the reaction was \(0.268 \mathrm{g}\). It's important to remember that the law of conservation of mass allows us to make these types of calculations. Regardless of how substances within a closed system interact with one another, or change forms, their total mass will always remain the same.

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Most popular questions from this chapter

Refer to the periodic table inside the front cover and identify (a) the element that is in group 11 and the sixth period (b) an element with atomic number greater than 50 that has properties similar to the element with atomic number 18 (c) the group number of an element \(\mathrm{E}\) that forms an ion \(\mathrm{E}^{2-}\) (d) an element \(M\) that you would expect to form the ion \(\mathrm{M}^{3+}\)

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