Oxygen forms a number of compounds with nitrogen, many of which are quite reactive. One such compound is 36.86 % by mass N . Calculate the number of grams of oxygen present in a sample of this compound that contains 44.00 grams of N .

75.37 g

Explanation:

From the question given above, the following data were obtained:

Percentage of nitrogen (N) in the compound = 36.86 %

Mass of nitrogen (N) in the compound = 44 g

Mass of oxygen (O) in the compound =?

Next, we shall determine the total mass of the compound. This can be obtained as follow:

Percentage of nitrogen (N) in the compound = 36.86 %

Mass of nitrogen (N) in the compound = 44 g

Total mass of compound (T) =?

Percentage of N = mass of N/ total mass × 100

36.86 % = 44 / T

36.86 / 100 = 44 / T

Cross multiply

36.86 × T = 100 × 44

36.86 × T = 4400

Divide both side by 36.86

T = 4400 / 36.86

Total mass = 119.37 g

Next, we shall determine the percentage of oxygen in the compound. This can be obtained as follow:

Percentage of N = 36.86 %

Percentage of O =?

Percentage of O = 100 – 36.86 %

Percentage of O = 63.14 %

Finally, we shall determine the mass of oxygen in the compound. This can be obtained as follow:

Percentage of O = 63.14 %

Total mass = 119.37 g

Mass of O =.?

Percentage of O = mass of O / total mass × 100

63.14 % = Mass of O / 119.37

Cross multiply

Mass of O = 63.14 % × 119.37

Mass of O = (63.14 / 100)× 119.37

Mass of O = 75.37 g

Thus, the mass of oxygen in the compound is 75.37 g

it takes on an electronical energy