Acompound weighing 115g contains 68.3g of carbon, 13.2g of hydrogen,15.9g of nitrogen, and some amount of oxygen. what is the mass percent of oxygen in the compound?

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Acompound weighing 115g contains 68.3g of carbon, 13.2g of hydrogen,15.9g of nitrogen, and some amount of oxygen. what is the mass percent of oxygen in the compound?

20.82% is the mass percent of oxygen in the compound.

Explanation:

Total mass of the compound = 143.1 g

Mass of carbon = 53.4 g

Mass of hydrogen = 16.9 g

Mass of nitrogen= 43 g

Mass of oxygen= x

143.1 g = x + 53.4 g + 16.9 g + 43 g

x = 143.1 g - 53.4 g - 16.9 g - 43 g = 29.8 g

Percentage of oxygen in the compound:

[tex]\%=\frac{\text{Mass of oxygen}}{\text{Mass of compound}}\times 100[/tex]

[tex]\%=\frac{29.8 g}{143.1 g}\times 100=20.82\%[/tex]

20.82% is the mass percent of oxygen in the compound.

80.5%- The total mass of the compound is 18g (14.5 + 3.5) then divide the mass of magnesium by the total. easy way to remember is- (part/whole) x 100

The answer is 69.048%.

Mass of potassium dichromate (K₂Cr₂O₇) is 294 g, which is a 100%.

Given mass of chromium is 52 g. So, the mass percent of chromium in the compound is 17.687%:

52 g : x% = 294 g : 100%

x = 52 ÷ 294 × 100 %

x = 17.687%

Given mass of potassium is 39 g. So, the mass percent of potassium in the compound is 13.265%:

39 g : x% = 294 g : 100%

x = 39 ÷ 294 × 100 %

x = 13.265%

Therefore, the mass percent of oxygen in the compound is 69.048%:

100% - 17.687% - 13.265% = 69.048%.

The mass percentage of oxygen in the given compound is 15.30 %.

Explanation:

We are given:

Mass of carbon in given compound = 68.3 g

Mass of Nitrogen in given compound = 15.9 g

Mass of Hydrogen in given compound = 13.2 g

Mass of the given compound = 115 g

Mass of Oxygen in compound = [tex]115-(68.3+15.9+13.2)=17.6g[/tex]

To calculate the mass percent of an element in a compound, we use the equation:

[tex]\text{Mass percent of oxygen}=\frac{\text{Mass of oxygen in compound}}{\text{Mass of the compound}}\times 100[/tex]

Putting values in above equation, we get:

[tex]\text{Mass percent of oxygen}=\frac{17.6g}{115g}\times 100=15.30\%[/tex]

Hence, the mass percentage of oxygen in the given compound is 15.30 %.

69.047% is the answer to this question

Hello helpful problems c

im not completely sure if this is correct, but this is what I did. and how I got my answer.

(3.5 g) / (14.5 + 3.5) g = 0.19 = 19% O by mass

From the question, we can get that there is only carbon, hydrogen, nitrogen and oxygen in this compound. So if we use the total amount minus weight of carbon, hydrogen and nitrogen, we can get the weight of oxygen. The mass percent equals the mass of oxygen divided by compound mass multiply 100%. The answer is 15.3%

mass of oxygen = 143,1g - (53,4g + 16,9g + 43g) = 29,8g

If 143,1g is 100%

so

29,8g is %O

%O = (29,8g*100%) / 143,1g = 20,82%

The mass percent of oxygen in given compound is 15.30%.

Explanation:

We are given:

Mass of nitrogen in compound = 31.8 g

Mass of hydrogen in compound = 26.4 g

Mass of carbon in compound = 136.6 g

Total mass of compound = 230 g

So, mass of oxygen will be = [tex]230-(136.6+26.4+31.8)=35.2g[/tex]

To calculate the percentage composition of element in a compound, we use the following equation:

[tex]\% \text{composition}=\frac{\text{Mass of the element}}{\text{Mass of the compound}}\times 100[/tex]

Putting values in above equation, we get:

[tex]\% \text{composition of oxygen}=\frac{35.2g}{230g}\times 100=15.30\%[/tex]

Hence, the mass percent of oxygen in given compound is 15.30%.