You must sign in Login/Signup

New student? Register here

Image Description

Chemistry Chapters

11th Class Chapter one Chemistry Short Questions

An important facility for 11th class students preparing for short questions chemistry 11th class chapter one of BISE. Get hundreds of questions to prepare and get better marks in 11th chemistry
Generic placeholder image

0

Our database contains a total of 0 questions for chemistry Short Questions. You’ll prepare using this huge databank.

0%

Perparation Level

You have coverd 0% Short Questions of total chemistry Short Questions
Question: 1
What do you mean by molecular ions?
Answer: 1
1-21



Question: 2

Molecular formula is multiple of empirical formula. Give an example.

Answer: 2
2-21
The empirical formula is the simplest whole number ratio of atoms of different elements present in a compound. Molecular formula tells us the actual number of atoms of each element in a molecule. Hence the empirical formula has to be multiplied with a suitable digit to get the molecular formula.
Question: 3

The atomic mass may be in fractions. Why?

Answer: 3
3-21
Most of the elements have isotopes. Isotopes have fractional atomic masses. The average of atomic masses of isotopes will be definitely in fractions. Moreover, the monoisotopic elements have also fractional atomic, masses.
Question: 4
What is atomic mass unit? Give its values in grams.
Answer: 4
4-21
It is a unit of mass used for atoms and molecules and is equal to the 1/12 of the mass of an atom of carbon —12. It is obtained by dividing the unity by Avogadro's number (6.02 x 1023).
Question: 5
Why positively charged ions of isotopes are passed through magnetic field in the mass spectrometer?
Answer: 5
5-21

The positively charged ions bend perpendicular to the joining lines of the two poles, when passed through the magnetic field. In this way, magnetic field gives these ions semicircular path, scatters them on the basis of m/e values and compels them to fall on the electrometer. Electrometer develops the electric current. The strength of the torrent gives the relative of ions of definite m/v value.

Question: 6
Alternate Text
Answer: 6
6-21
Alternate Text
Question: 7
Define Avogadro's number. How does it relate to the masses of chemical substances?
Answer: 7
7-21
It is the number of atoms, molecules or ions in one gram mole of an element, compound and ion. One gram mole of the substance is the atomic mass, molar mass or ionic mass taken in grams. It means that the number of the species is related with the masses of the species.
Question: 8
Define empirical formula and how it is related to molecular formula?
Answer: 8
8-21
Alternate Text
Question: 9
Alternate Text
Answer: 9
9-21
Alternate Text
Question: 10
180 grams of glucose and 342 grams of sucrose have same number of molecules, but different number of atoms present in them. Justify it.
Answer: 10
10-21
180 grams of glucose (C6H12O6) and 342 grams of sucrose (C12H22O11) are one mole of each. One mole of various substances contain equal number of molecules i.e., 6.02 x 1023. One molecule of C5H12O6 has 24 atoms. The total number of atoms of glucose in one mole is 24 x 6.02 x 1023.one molecule of C12H22011 has 45 atoms and the number of atom in 1 mole is 45 x 6.022 x 1023. It means that one mole of both glucose and sucrose will have different number of atoms.
Question: 11

Calculate the mass in grams of 10-2 moles of water.

Answer: 11
11-21
Alternate Text
Question: 12
2 grams of H2 , 16g of CH4 and 44g of CO2 , occupy separately the volumes of 22.414 dm2 at STP although the sizes and masses of molecules of three gases are very different from each other.
Answer: 12
12-21
One mole of an ideal gas at S.T.P. occupies a volume of 22.414 dm3. Sizes and masses of molecules of different gases do not affect the volume. Normally it is known that in the gaseous state, the distance between the molecules is 300 times greater than their diameter. Therefore two grams of H2 , 16g of CH4 and 44g of CO2 (1 mole of each gas) separately occupy a volume of 22.4 dm3. This is called molar volume (Vm).
Question: 13
What the experimental yield is mostly less than the theoretical yield?
Answer: 13
13-21

. Experimental yield is mostly less than theoretical yield due to the following reasons.

(1) Mechanical loss of products due to:

(a) . Filtration

(b) Separation by distillation

(c) Separating by separating funnel

(d) Washing

(e) Drying

(f) Crystallization

(2)Side reaction.

(3)Reversibility of reaction.
Question: 14
N2 and CO have same number of electrons, protons and neutrons. Justify.
Answer: 14
14-21

No. of electrons in N2 = 7 + 7 = 14, number of protons in N2 = 7 + 7 = 14 and number of neutrons (14 - 7) = 7 + 7 = 14.

In CO, number of electrons in C = 6

Number of electrons in 0 = 8

Total number of electrons = 6 + 8 = 14

Number of neutrons in C = 6

Number of protons in 0 = 8

Total number of protons = 6 + 8 = 14

Question: 15
Alternate Text
Answer: 15
15-21
Alternate Text
Question: 16
Prove that one mole of each 142, CO2 and H2 contain equal number of molecules.
Answer: 16
16-21
This is according to Avogadro's law that one mole of a substance has 6.02 1023 molecules in it. So, 28 g of N2 , 44g of CO2 and 2 g of H2 have 6.02 1023 molecules in each.
Question: 17
How can the efficiency of a chemical reaction be expressed?
Answer: 17
17-21
Alternate Text
Question: 18
What is limiting reactant? How it helps to control the reaction?
Answer: 18
18-21
A limiting reactants is that one which is in lesser quantity and it is consumed earlier. Whenever, it is consumed then the further formation of the product stops, although the excess reagent is lying in the vessel. If the limiting reagent is not available to the excess quantity then product cannot be formed further.
Question: 19
Distinguish between actual and theoretical yield.
Answer: 19
19-21
Alternate Text
Question: 20
What is limiting reactant? How it helps to control the reaction?
Answer: 20
20-21
A limiting reactants is that one which is in lesser quantity and it is consumed earlier. Whenever, it is consumed then the further formation of the product stops, although the excess reagent is lying in the vessel. If the limiting reagent is not available to the excess quantity then product cannot be formed further.
Question: 21
Define Solubility product and write down its application?
Answer: 21
21-21
Solubility product: The product of molar concentration of oppositely charged ions , in equilibrium with its solid salt in its saturated solution at a given temperature is called solubility product. Its is denoted by KSP
Application of KSp:
  • Determination of KSP From solubility.
  • Effect of common ion on solubility.

11th Class Chemistry Chapters Short Questions