Question

A sample of metal weighing 2.51 g is combined with oxygen; the metal oxide weighs 3.01 g. The mass percent of oxygen in the compounds is __

[A] 16.6%
[B] Cannot be determined from the given information
[C] 19.9%
[D] 83.4%
[E] 50.0%

Answer 1

The Answer Is A
Hope this will help!

Answer 2

The mass percent of oxygen in the compound is 16.6%. The correct option is [A] 16.6%

From the question,

We are to determine the mass percent of oxygen in the compound

The mass percent of oxygen in the compound can be calculated from

$Mass\ percent\ of\ oxygen = \frac{Mass\ of\ oxygen\ in\ the\ compound}{Mass\ of\ the\ compound } \times 100\%$

First, we will determine the mass of oxygen in the compound

Mass of oxygen in the compound = Mass of the compound - Mass of the metal before it combined with oxygen

From the question

Mass of the compound = 3.01 g

Mass of the metal before it combined with oxygen = 2.51 g

∴ Mass of oxygen in the compound = 3.01g - 2.51g

Mass of oxygen in the compound = 0.5 g

Now,

For the mass percent of oxygen in the compound

$Mass\ percent\ of\ oxygen = \frac{Mass\ of\ oxygen\ in\ the\ compound}{Mass\ of\ the\ compound } \times 100\%$

∴ $Mass\ percent\ of\ oxygen = \frac{0.5}{3.01} \times 100\%$

$Mass\ percent\ of\ oxygen = \frac{50}{3.01} \%$

Mass percent of oxygen = 16.611%

Mass percent of oxygen ≅ 16.6%

Hence, the mass percent of oxygen in the compound is 16.6%. The correct option is [A] 16.6%

Learn more here: https://brainly.com/question/14139062