The percentage of nitrogen in urea is about
- 63
- 70
- 28
- 47
The Correct Option is D
Approach Solution - 1
The correct answer is Option D) 47
Urea is \((NH_4)_2CO\) 2N = Urea 28 g = 60 g
\(\therefore\) Percentage of nitrogen = \(\frac{28}{60} \times 100\) = 46.66%
Read more from the chapter: Some Basic Concepts of Chemistry
Approach Solution -2
The correct answer is Option D) 47
Real Life Applications
- Urea is highly used in agriculture. Therefore the percentage of nitrogen is important.
- Urea is a source of nitrogen for plants. Urea will provide a source of nitrogen to fish. They help in the growth and reproduction of fish.
- Urea has many industrial applications.
Question can also be asked as
- What is the percentage of nitrogen in urea?
- How can you calculate the percentage of nitrogen in urea?
- What is the significance of the percentage of nitrogen in urea?
Approach Solution -3
The correct answer is Option D) 47
The percentage composition is the number of individual elements that are present in the compound multiplied by 100. It tells the contribution of each element in a compound. It can be used for stoichiometric calculations.
The formula for composition formula
% composition = grams of element/grams of compound *100
Properties
- The percentage composition will remain constant for a particular chemical compound.
- It is the ratio of each element that forms a compound.
- It can be used to make the molecular formula of the given compound.
- The ratio of each element can be obtained from the molecular mass and the percentage composition.
Read more:
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Notes on Mole concept and Molar Masses
Concepts Used:
Mole Concept
In the field of chemistry, a mole is defined as the amount of a substance that contains exactly 6.02214076 * 1023 ‘elementary entities’ of the given substance.
The number 6.02214076*1023 is popularly known as the Avogadro constant and is often denoted by the symbol ‘NA’. The elementary entities that can be represented in moles can be atoms, molecules, monoatomic/polyatomic ions, and other particles (such as electrons).
For example, one mole of a pure carbon-12 (12C) sample will have a mass of exactly 12 grams and will contain 6.02214076*1023 (NA) number of 12C atoms. The number of moles of a substance in a given pure sample can be represented by the following formula:
n = N/NA
Where n is the number of moles of the substance (or elementary entity), N is the total number of elementary entities in the sample, and NA is the Avogadro constant.
The word “mole” was introduced around the year 1896 by the German chemist Wilhelm Ostwald, who derived the term from the Latin word moles meaning a ‘heap’ or ‘pile.
The mole concept refers to the atomic mass of a mole that is measured in grams. The gram atomic mass of an element is known as a mole. The mole concept combines the mass of a single atom or molecule in a.m.u. to the mass of a large group of comparable molecules in grams. Atomic mass is the mass of a single atom, whereas molecular mass is the mass of a group of atoms.
The Formula of Mole Concept
The number of units that make up a mole has been calculated to be 6.022 ×10²³. The fundamental constant is also known as Avogadro's number (NA) or Avogadro constant. This constant is appropriately represented in chemistry using an explicit unit termed per mole.
Number of Moles = (Mass of the Sample)/(Molar Mass)
Read More: Mole Fraction