Atoms And Molecules Class 9th Physics & Chemistry AP Board Solution

Class 9th Physics & Chemistry AP Board Solution
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  1. Draw the diagram to show the experimental setup for the law of conservation of mass.…
  2. Explain the process and precautions in verifying law of conservation of mass.…
  3. 15.9g. of copper sulphate and 10.6g of sodium carbonate react together to give 14.2g of…
  4. Carbon dioxide is added to 112g of calcium oxide. The product formed is 200g of calcium…
  5. 0.24g sample of compound of oxygen and boron was found by analysis to contain 0.144g of…
  6. In a class, a teacher asked to write the molecular formula of oxygen Shamita wrote the…
  7. Imagine what would happen if we do not have standard symbols for elements?…
  8. Mohith said "H2 differs from 2H". Justify.
  9. Lakshmi gives a statement "CO and Co both represents element". Is it correct? State…
  10. The formula of the water molecule is H2O. What information you get from this formula.…
  11. How would you write 2 molecules of oxygen and 5 molecules of Nitrogen.…
  12. The formula of a metal oxide is MO. Then write the formula of its chloride.…
  13. Formula of calcium hydroxide is Ca (OH)2 and zinc phosphate is Zn3(PO4)2. Then write the…
  14. Find out the chemical names and formulae for the following common household substances. a)…
  15. 0.5 mole of N2 gas. Calculate the mass of the following
  16. 0.5 mole of N atoms. Calculate the mass of the following
  17. 3.011 × 10^23 number of N atoms. Calculate the mass of the following…
  18. 6.022 × 10^23 number of N2 molecules. Calculate the mass of the following…
  19. 46g of Na Calculate the number of particles in each of the following…
  20. 8g of O2 Calculate the number of particles in each of the following…
  21. 0.1 mole of hydrogen Calculate the number of particles in each of the following…
  22. 12g of O2 gas. Convert into mole
  23. 20g of water. Convert into mole
  24. 22g of carbon dioxide. Convert into mole
  25. Write the valencies of Fe in FeCl2 and FeCl3
  26. Calculate the molar mass of Sulphuric acid (H2SO4) and glucose (C6H12O6)…
  27. Which has more number of atoms - 100g of sodium or 100g of iron? Justify your answer.…
  28. Complete the following table.
  29. Fill the following table

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Question 1.

Draw the diagram to show the experimental setup for the law of conservation of mass.


Answer:

Step 1: Take a flask and take a mixture of sodium hydroxide solution and copper sulphate solution.


Step 2: Weight the flask and note it.


Step 3: Now mix the whole mixture thoroughly.


Step 4: Now, weight the flask.



We will observe that after mixing there is no change in the mass. This explains the law of conservation of mass.



Question 2.

Explain the process and precautions in verifying law of conservation of mass.


Answer:

Law of conservation of mass states that “Matter is neither created nor destroys in a chemical reaction. More simply, the mass of products is equal to the mass of reactants in a chemical reaction.



Question 3.

15.9g. of copper sulphate and 10.6g of sodium carbonate react together to give 14.2g of sodium sulphate and 12.3g of copper carbonate. Which law of chemical combination is obeyed? How?


Answer:

Law of conservation of mass is obeyed.


Explanation:



Total mass of reactants = 15.9g + 10.6g = 26.5g


Total mass of products = 14.2g + 12.3g = 26.5g


As there is no change in the mass of reactants and products, hence law of conservation is obeyed.



Question 4.

Carbon dioxide is added to 112g of calcium oxide. The product formed is 200g of calcium carbonate. Calculate the mass carbon dioxide used. Which law of chemical combination will govern your answer.


Answer:

The reaction taking place is:



Let the mass of CO2 is xg.


According to the law of conservation of mass, the mass of reactants is equal to the mass of products.


Therefore,


⇒ x + 112g = 220g


⇒ x = 220g – 112g


⇒ x = 108g


Thus, the mass of carbon dioxide is 108g.



Question 5.

0.24g sample of compound of oxygen and boron was found by analysis to contain 0.144g of oxygen and 0.096g of boron. Calculate the percentage composition of the compound by weight.


Answer:

Given: Mass of compound = 0.24g


Mass of oxygen = 0.144g


Mass of boron = 0.096g


To calculate the percent of the composition of oxygen, we apply the formula:



⇒ 


⇒ % composition of oxygen = 0.6g × 100


⇒ % composition of oxygen = 60%


To calculate the percent of the composition of boron, we apply the formula:



⇒ 


⇒ % composition of boron = 0.4g × 100


⇒ % composition of boron = 40%


Total percentage composition of compound is 60% + 40% = 100%



Question 6.

In a class, a teacher asked to write the molecular formula of oxygen Shamita wrote the formula as O2 and Priyanka as O. which one is correct? State the reason.


Answer:

Shamita wrote the correct formula of oxygen as O2 because:


i. A molecule of oxygen has two atoms.


ii. It is diatomic in nature (atomicity = 2)


iii. Thus, writing oxygen as O2 indicates two separate atoms of oxygen.


Note: Atomicity is the number of atoms constituting a molecule.



Question 7.

Imagine what would happen if we do not have standard symbols for elements?


Answer:

if we do not have standard symbols for elements, then it will take a lot of time to write the full name of the elements and compounds every time to describe a reaction.



Question 8.

Mohith said "H2 differs from 2H". Justify.


Answer:



Question 9.

Lakshmi gives a statement "CO and Co both represents element". Is it correct? State reason.


Answer:

No, CO does not represent element whereas Co represents element because the first letter of the symbol is always the upper case and the second letter is always lower case.


In CO, the second letter is uppercase whereas in Co, the second letter is lowercase. Hence Co represents an element.



Question 10.

The formula of the water molecule is H2O. What information you get from this formula.


Answer:

To get the information, first, we will see the elements present in a molecule of the compound.


Second, we will count the number of atoms of each element of that molecule.


In H2O:


i. 2 atoms of hydrogen and one atom of oxygen are present.


ii. There are total three atoms present in a molecule of water.



Question 11.

How would you write 2 molecules of oxygen and 5 molecules of Nitrogen.


Answer:

For oxygen:


⇒ First, write the symbol of oxygen – 


⇒ Now write 2 as a subscript after O – 


For nitrogen:


⇒ First, write the symbol of nitrogen – 


⇒ Now write 5 as a subscript after N – 



Question 12.

The formula of a metal oxide is MO. Then write the formula of its chloride.


Answer:

The formula of its chloride is MOCl2



Question 13.

Formula of calcium hydroxide is Ca (OH)2 and zinc phosphate is Zn3(PO4)2. Then write the formula to calcium phosphate.


Answer:

Valency of Ca = 2


Valency of PO4 = 3


Now, apply the criss cross method



So the formula will be Ca3(PO4)2



Question 14.

Find out the chemical names and formulae for the following common household substances.

a) common salt

b) baking soda

c) washing soda

d) vinegar


Answer:

a) Common salt


Chemical name – sodium chloride


Chemical formula – NaCl


b) baking soda


Chemical name – sodium bicarbonate


Chemical formula – NaHCO3


c) washing soda


Chemical name – sodium carbonate


Chemical formula – Na2CO3


d) vinegar


Chemical name – acetic acid


Chemical formula – CH3COOH



Question 15.

Calculate the mass of the following

0.5 mole of N2 gas.


Answer:

0.5 mole of N2 gas


First, we apply the formula:



⇒ Mass of N2 = No. of moles × Molar mas of N2


⇒ Mass of N2 = 0.5 mole × 2(atomic mass of nitrogen)


⇒ Mass of N2 = 0.5 × 2 × 14


⇒ Mass of N2 = 14g


Thus, the mass of N2 gas is 14g.



Question 16.

Calculate the mass of the following

0.5 mole of N atoms.


Answer:

0.5 mole of Natoms


First, we apply the formula:



⇒ Mass of Natoms = No. of moles × Molar mass of N


⇒ Mass of Natoms = 0.5 mole × (atomic mass of nitrogen)


⇒ Mass of Natoms = 0.5 × 14


⇒ Mass of N2 = 7g


Thus, the mass of N atoms is 7g.



Question 17.

Calculate the mass of the following

3.011 × 1023 number of N atoms.


Answer:

3.011 X 1023 number of N atoms.


As we know that 1 mole = 6.022 X 1023atoms


⇒ 


⇒ 1/2 mole = 0.5 mole


For 0.5 mole of Natoms


First, we apply the formula:



⇒ Mass of Natoms = No. of moles × Molar mass of N


⇒ Mass of Natoms = 0.5 mole × (atomic mass of nitrogen)


⇒ Mass of Natoms = 0.5 × 14


⇒ Mass of N atoms = 7g


Thus, mass of3.011 × 1023 number of N atoms is 7g



Question 18.

Calculate the mass of the following

6.022 × 1023 number of N2 molecules.


Answer:

6.022 X 1023 number of N2 molecules.


As we know that 1 mole = 6.022 X 1023atoms


For 1 mole of N2molecules:


First, we apply the formula:



⇒ Mass of N2 = No. of moles × Molar mass of N2


⇒ Mass of N2 = 1 mole × 2(atomic mass of nitrogen)


⇒ Mass of N2 = 1mole × 28u


⇒ Mass of N2 = 28g


Thus, mass of6.022 × 1023 number of N2 molecules is 28g.



Question 19.

Calculate the number of particles in each of the following

46g of Na


Answer:

The number of particles present in one mole of any substance is has a fixed value of 6.022 × 1023. This number is called Avogadro constant(NA).


Mass of Na = 46g


Molar mass of Na = 23u


Apply the formula given below:


Number of particles = number of moles × 6.022 × 1023


⇒ 


⇒ 


⇒ Number of particles = 2 × 6.022 × 1023


 Number of particles = 12.046 × 1023


Thus, 46g of Na contains 12.046 × 1023 particles.



Question 20.

Calculate the number of particles in each of the following

8g of O2


Answer:

The number of particles present in one mole of any substance is has a fixed value of 6.022 × 1023. This number is called Avogadro constant(NA).


Mass of O2 = 8g


Molar mass of O2 = 32u


Apply the formula given below:


Number of particles = number of moles × 6.022 × 1023


⇒ 


⇒ 


⇒ Number of particles = 0.25 × 6.022 × 1023


 Number of particles = 1.5 × 1023


Thus, 8g of O2 contains 1.5 × 1023 particles.



Question 21.

Calculate the number of particles in each of the following

0.1 mole of hydrogen


Answer:

The number of particles present in one mole of any substance is has a fixed value of 6.022 × 1023. This number is called Avogadro constant(NA).


Number of mole of hydrogen = 0.1 mole


Molar mass of H2 = 2u


Apply the formula given below:


Number of particles = number of moles × 6.022 × 1023


⇒ Number of particles = 0.1 mole × 6.022 × 1023


 Number of particles = 6.022 × 1024


Thus, 0.1 mole of hydrogen contains 6.022 × 1024particles.



Question 22.

Convert into mole

12g of O2 gas.


Answer:

Mass of O2 gas = 12g


Molar mass of O2 = 32u


Apply the formula:



⇒ 


⇒ No. of moles = 0.37


Thus, the 12g of O2 gas is 0.37 mole



Question 23.

Convert into mole

20g of water.


Answer:

Mass of water(H2O) = 20g


Molar mass of H2O = 18u


Apply the formula:



⇒ 


⇒ No. of moles = 1.11


Thus, the 20g of water is 1.11 mole



Question 24.

Convert into mole

22g of carbon dioxide.


Answer:

Mass of CO2 gas = 22g


Molar mass of CO2 = 44u


Apply the formula:



⇒ 


⇒ No. of moles = 0.5


Thus, the 22g of CO2 gas is 0.5 mole



Question 25.

Write the valencies of Fe in FeCl2 and FeCl3


Answer:

In FeCl2, the valency of Fe is + 2


In FeCl3, the valency of Fe is + 3



Question 26.

Calculate the molar mass of Sulphuric acid (H2SO4) and glucose (C6H12O6)


Answer:

Molar mass of sulphuric acid (H2SO4):


⇒ 2(atomic mass of hydrogen) + (atomic mass of Sulphur) + 4(atomic mass of oxygen)


⇒ 2 × 1 + 32 + 4 × 16


⇒ 2 + 32 + 64


⇒ 98 u


Thus, the molar mass of H2SO4 is 98 u.


Molar mass of glucose (C6H12O6):


⇒ 6(atomic mass of carbon) + 12(atomic mass of hydrogen) + 6(atomic mass of oxygen)


⇒ 6 × 12 + 12 × 1 + 6 × 16


⇒ 72 + 12 + 96


⇒ 108 u


Thus, the molar mass of C6H12O6 is 108 u.



Question 27.

Which has more number of atoms - 100g of sodium or 100g of iron? Justify your answer. (atomic mass of sodium = 23u, atomic mass of iron = 56u)


Answer:

For sodium


Given: Mass of sodium = 100g


Molar mass of sodium = 23u


Number of atoms = number of moles × 6.022 × 1023


⇒ 


⇒ 


⇒ Number of atoms = 4.34 × 6.022 × 1023


 Number of atomss = 2.613 × 1024


Thus, 100g of sodium contains 2.613 × 1024 atoms.


For iron


Given: Mass of iron = 100g


Molar mass of iron = 55.8u


Number of atoms = number of moles × 6.022 × 1023


⇒ 


⇒ 


⇒ Number of atoms = 1.79× 6.022 × 1023


 Number of atoms = 1.07× 1024


Thus, 100g of iron contains 1.07× 1024atoms.


Therefore, 100g of sodium has more number of atoms.



Question 28.

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Answer:



Question 29.

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Answer:






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