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Question 1

State Graham‘s law of diffusion

Answer 1

Graham’s Law of diffusion: The rate of diffusion (r) of a gas is inversely propositional to the square root of its density (d)” at constant temperature and pressure.
r  1/ d

Question 2

Daltons law of particle pressure

Answer 2

The total pressure entered by a mixture of chemically non – reacting gases at a given temperature and volume is equal to the sum of partial pressures of the component gases.
P=P1 +P2 +P3 ……

Question 3

Which gas diffuses faster among N2, O2, CH4 gases? Why?

Answer 3

The molecules weights of the given gases are N2 (28), O2 (32) and CH4 (16). The lighter gases diffuse faster than heavier gases. Hence, CH4 diffuses faster.

Question 4

What is Boltzman’s constant? Give its value.

Answer 4

Boltzman’s constant is the gas constant per molecule Boltzman’s Constant K = R/N
= 1.38 x 10-16 erg / K. Molecule

Question 5

How many times methane diffuses faster than sulphur dioxide?

Answer 5

According to graham’s Law of diffusion

Check pdf

Hence methane gas diffuses 2 times faster than S

Question 6

What are Isobars?

Answer 6

The curves (or) graphs that can be drawn at constant pressure are called Isobars. Ex: Graph drawn between Volume and Temperature

Question 7

Why pressure cooker is used for cooking food in hills?

Answer 7

-At hill areas pressure cooker is used for cooking food because low atmospheric pressure is observed at high altitudes. At high altitudes liquids boil at low tempera

Question 8

Give the ratio of R M S average and most probable speed of gas molecule

Answer 8

Check 8

Question 9

How many numbers of moles of glucose are present in 540 Grams of Glucose?

Answer 9

G.M. Weight of (C6H12O6) Glucose = 180.
No. Of Moles = Weight / G.M Weight = 540/180 = 3

Question 10

The empirical formula of a compound is CH2O. Its molecular weight is 90. Calculate the molecular formula of the compoun

Answer 10

Molecular formula = n (Empirical formula)
N =- Moleculas weight / Empirical weight = 90 /30 = 3 Mol. Weight = 90
Empirical weight (CH2O) = 30.
Moleculas formula = 3 (CH2O) = C3H6O3.

Question 11

What is Redox concept? Give an example?

Answer 11

Redox reactions are the reactions in which reduction and oxidation both takes place
______________
Ex Cu + Zn (^-2)—-> Cu(+2) +Zn
^____________________

Question 12

. Calculate the weight of 0.1 mole of Sodium carbonate?

Answer 12

No. of moles = weight / G.Mol. Wt. No. of Moles = 0.1
G.M.W of Na2CO3 = 106 Weight = 106 x 0.1 = 10.6 Gr.

Question 13

State the first law of the thermodynamics

Answer 13

Energy can neither be created nor destroyed, but it can be transformed from one form to another”

Question 14

State third law of thermodynamics

Answer 14

The entropy of a pure crystalline substance is Zero at the absolute Zero of a temperature (-2730C)

Question 15

What are intensive and extensive properties?

Answer 15

Intensive properties : The properties which do not depend upon the quantity of matter are called intensive properties.
Ex: Pressure
Extensive Properties : The properties which depend upon the quantity of matter are called extensive properties
Ex: Mass.

Question 16

16. Write the relation between Kp and Kc

Answer 16

Kp = Kc (RT) Δn
Δn = No. of gaseous products – No. Of gaseous reactants

Question 17

17. Give two chemical equilibrium reactions for which Kp > K

Answer 17

1.
2.
2NH3 (g) N2 (g) + 3H2 (g) Δn=nP –nR =(3+1)–2=2 Δn = 2 (+ve)
Therefore Kp > Kc
2SO3 (g) 2SO2 (g)+O2 (g) Δn=nP –nR =(2+1)–2=1 Δn = 1 (+ve)
Therefore Kp > Kc

Question 18

What is Lewis acid? Give one example?

Answer 18

A substance which can accept an electron pair to form a co-ordinate covalent bond with donor is called Lewis Acid.
Ex: BF3.