Solved worksheet Some Basic Concepts of Chemistry

Solved worksheet Some Basic Concepts of Chemistry is all about subjective and objective knowledge.

Q1. How many significant figures are there in (i) 3.070 and (ii) 0.0025?     
Ans 1. (i) 4                  (ii) 2

Q 2. How many significant figures are present in the answer of the following calculation:  .0125 + 0.8250 + 0.025
Ans 2.  0.86

Q 3. The density of vanadium is 5.96 g cm3. Express this in SI unit.
Ans3. 5960 kg m³

Q 4. The body temperature of a normal healthy person is 37⁰C. Calculate its value in ⁰F.
Ans 4. We know
⁰F = 9/5(⁰C) + 32
⁰F = 9/5(37) + 32
⁰F = 9 × 7.4 + 32 = 98.6 ⁰F

Q5. At what temperature will both the Celsius and Fahrenheit scales read the same value?
Ans. Let x be the common reading.
Then, C = F = x
We knoe the relation between ⁰C and ⁰F
⁰C=5/9 (⁰F-32), and substituting x for ⁰C and ⁰F, we get
x =5/9 (x-32)
x =5/9x – 5/9×32
x – 5/9x = 5×32/9
4/9x = – 5×32/9
x = – 5×32/4 = -40
So, -40C = -40F
Hence, at -40 degrees, the readings on the Celsius scale and the Fahrenheit scales are the same.

Q6. Express the following in the scientific notation: (i) 0.0048 (ii) 234,000
Ans 6. i). 4.8 × 10^-4                 ii) 2.34 × 10⁵

Q7. Given the numbers: 161 cm, 0.161 cm, O.OI61 cm. Write The number of significant figures for these three numbers.
Ans 7. 3,3,3

Q8. Read the following and choose the incorrect statements.
(i) Both weight and mass are the same quantities used for measurement of the amount of matter present in a substance
(ii) Mass and weight of a substance vary from one place to another due to a change in gravity.
(iii) ST unit of mass is kilogram and while the SI unit of weight is the gram.
(a) (i) and (iii)                                     (b) (ii) and (iii)
(c) (i) and (ii)                                      (d) All of these
Ans 8. (d) All of these

Q9. A student performs a titration with different burettes and finds titre values of 25.2 mL, 25.25 mL, and 25.0 mL the number of significant figures in the average titre value is  
a) 1                       b) 3 
c) 2                       d) 4
Ans 9. (b)  Calculate the average value of different titre values.
Then use the rule to determine the significant figures for mathematical calculation.
Average value =  25.2  +  25.25  +  25.0/3  =   75.45/3
= 25.15  = 25.2 mL  The number of significant figure is 3

Solved worksheet Some Basic Concepts of Chemistry

Q10. What will be the answer of 77.32-6.3? 
a) 71.02                                       b) 71.0           
c) 71.2                                         d) 71.1
Ans 10. (b)  The answer is to be reported up to the same number of decimal places as that of the term with the least number of decimal places. This after rounding off 71.02 becomes 71.0.

Que 11. What is the unit factor method? Express the following in SI units – 93 million miles (distance between earth and sun)
Ans 11. The method to convert units from one system to another is called the unit factor method.
93 million miles = 93 × 10⁶ miles
1 mile = 1.60934 km = 1.60934 × 10³ m

Que 12. What do mean by gram atomic mass. one million silver atoms weigh 1.79 x 10¹⁶ g. Calculate the gram atomic mass of silver.
Ans 12. The atomic mass of an element expressed in grams is the gram atomic mass
Number of silver atoms = 1 million = 1 × 10⁶
Mass of one million Ag atoms = 1.79 × 10¹⁶g
Mass of 6.023 x 10²³ atoms of Silver = 1.79 × 10¹⁶g x 6.023× 10²³/1 × 10⁶
= 107.8 g

Que 13. Copper oxide obtained by heating copper carbonate or copper nitrate contains copper and oxygen in the same ratio by mass. Which law is illustrated by this observation? State the law.
Ans 13. Law of Definite Proportions: According to this law a chemical compound
always consists of the same elements combined together in the same ratio,
irrespective of the method of preparation or the source from where it is taken.

Que 14. Write the empirical formula of the following:
(a) N₂O₄ (b) C₆H₁₂O₆ (c) H₂O (d) H₂O₂
Ans 14. (a) NO₂ (b) CH₂O (c) H₂O (d) HO

Que 15. Chlorine has two isotopes of atomic mass units 34.97 and 36.97. The relative abundance of the isotopes is 0.755 and 0.245 respectively. Find the average atomic mass of chlorine.
Ans 15. Average atomic mass = 34.97 × 0.755 + 36.97 × 0.245 = 35.46 u

Solved worksheet Some Basic Concepts of Chemistry

Que 16. How are 0.50 mol Na₂CO₃ and 0.50 M Na₂CO₃ different?
Ans 16. Molar mass of Na₂CO₃ = 2 × 23 +12 + 3 × 16 = 106 g / mol
0.50 mol Na₂CO₃ means 0.50 × 106 = 53 g
0.50 M Na₂CO₃ means 0.50 mol i.e. 53 g of Na₂CO₃ are present in I L of the
solution.

Solved worksheet Some Basic Concepts of Chemistry is all about subjective and objective knowledge

Que 17. What is the percentage of carbon, hydrogen, and oxygen in ethanol?
Ans 17. Molecular formula of ethanol is: C₂H₅OH
Molar mass of ethanol is: (212.01 + 61.008 + 16.00) g = 46.068 g
Mass per cent of carbon = (24.02g / 46.068g) ×100 = 52.14%
Mass per cent of hydrogen = (6.048g / 46.068g) × 100 = 13.13%
Mass per cent of oxygen = (16.00 g / 46.068g) ×100 = 34.73%

Que 18. What do mean by molarity? Calculate the molarity of NaOH in the solution
prepared by dissolving its 4 g in enough water to form 250 mL of the solution.
Ans 18. The number of moles of solute dissolved per litre (dm³) of the solution is called molarity.
Since molarity (M) = No. of moles of solute /Volume of solution in litres
= (Mass of NaOH / Molar Mass of NaOH) /0.250 L
= (4 g / 40 g 0.1 mol) / 0.250L = 0.1 mol / 0.250 L
= 0.4 mol L^-1  = 0.4 M

Que 19. Express the following in the scientific notation with 2 significant figures-
(a) 0.0048                         (b) 234,000                       (c) 200.0
Ans 19. (a) 4.8 × 10^-3                       (b) 2.3 × 10⁵                      (c) 2.0 × 10²

Que 20. Calculate the number of atoms in each of the following:
(i) 52 moles of Ar   (ii) 52 u of He         (iii) 52 g of He
Ans 20. (i) 1 mole of Ar = 6.022 × 1023 atoms of Ar
52 mol of Ar = 52 × 6.022 × 10²³ atoms of Ar
= 3.131 × 10²⁵ atoms of Ar
(ii) 1 atom of He = 4 u of He
Or
4 u of He = 1 atom of He
1 u of He = 1/4 atom of He
52 u of He = 52/4 atom of He
= 13 atoms of He
(iii) Molar mass of He = 4 g/mol
4 g of He contains = 6.022 × 10²³ atoms of He
52 g of He contains = 6.022 × 10²³ x 52/4 = 78.286 x 10²³ atoms of He

Que 21. What is the difference between empirical and molecular formulas? A compound contains 4.07 % hydrogen, 24.27 % carbon, and 71.65 % chlorine. Its molar mass is 98.96 g. What are its empirical and molecular formulas?
Ans 11. An empirical formula represents the simplest whole-number ratio of various atoms present in a compound whereas the molecular formula shows the exact number of different types of atoms present in a molecule of a compound.

The empirical formula of the above compound is CH₂Cl.
empirical formula mass is 12 + (1 x 2) + 35.5 = 49.5
n= Molecular Mass / Empirical Formula Mass = 98.96 / 49.5 = 2
Hence molecular formula is C₂H₄Cl₂

Solved worksheet Some Basic Concepts of Chemistry