Atoms and Molecules Test

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Atoms and Molecules Test - 53

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Weekly Quiz Competition

Question 1
1 / -0

Calculate the number of atoms of sulphur present in $0.5$ moles of ${ Na }_{ 2 }{ S }_{ 2 }{ O }_{ 3 }$ :

A
$62.02\times { 10 }^{ 23 }$ atoms

B
$622\times { 10 }^{ 23 }$ atoms

C
$6.023\times { 10 }^{ 23 }$ atoms

D
$6.02\times { 10 }^{ -23 }$ atoms

Solution

$1$ mole of $Na_2S_2O_3$ contains Avogadro's number of molecules which is $\displaystyle 6.023 \times 10^{23}$ molecules.

$0.5$ mole of $Na_2S_2O_3$ will contain $\displaystyle 0.5 \times 6.023 \times 10^{23}=3.0115 \times 10^{23}$ molecules.

One molecule of $Na_2S_2O_3$ contains $2\ S$ atoms.

$\displaystyle 3.0115 \times 10^{23}$ molecules of $Na_2S_2O_3$ will contain $\displaystyle 2 \times 3.0115 \times 10^{23}=6.023 \times 10^{23}$ $S$ atoms.
Hence, option $C$ is correct.
Question 2
1 / -0

What weight of calcium contains the same number of atoms as those in $3 g$ of carbon?

A
$10 g$

B
$20 g$

C
$30 g$

D
$40 g$

Solution

Atomic weights of $C$ and $Ca$ are 12 g/mol and 40 g/mol respectively.
3 g $C \displaystyle = \dfrac {3 \ g}{12 \ g/mol}= 0.25 \ mol C$ .
Number of moles of $Ca \displaystyle =$ number of moles of $C \displaystyle =$ 0.25.
Weight of $Ca \displaystyle = 3 \ mol \times 40 \ g/mol = 10 \ g$ .
Note: Since $C$ and $Ca$ samples have same number of atoms, they will have same number of moles.
Question 3
1 / -0

What is the approximate molecular mass of dry air containing 78% $N_2$ and 22% $O_2$ ?

A
28.88

B
27

C
30

D
34

Solution

The molecular mass of dry air is given by-

$\displaystyle = \dfrac { [ \text { Molecular mass of }N_2 \times \text { Percentage of }N_2 ] + [ \text { Molecular mass of }O_2 \times \text { Percentage of }O_2 ] } { \text { Percentage of }N_2 + \text { Percentage of }O_2 }$

$\displaystyle = \dfrac { [ \text { 28 } \times \text { 78 } ] + [ \text { 32 } \times \text { 22 } ] } { \text { 78 } + \text {22 } }$

$\displaystyle = \text {28.88 g/mol}$

Hence, option $A$ is correct.
Question 4
1 / -0

Identify the pair of substances having the same formula unit mass.

A
Calcium chloride, potassium carbonate

B
Calcium oxide, hydrochloric acid

C
Carbon monoxide, ammonia

D
Carbon dioxide, nitrous oxide

Solution

Carbon dioxide and nitrous oxide have the same formula unit mass.
Formula unit mass for carbon dioxide $\displaystyle CO_2 = 12 +2(16)=12+32=44\ u$
Formula unit mass for nitrous oxide $\displaystyle N_2O = 2(14)+16=28+16=44\ u$

Let's look at the formula unit mass of the other given compounds:
Formula unit mass for calcium chloride $\displaystyle CaCl_2 = 40+2(35.5)=40+71=111\ u$
Formula unit mass for potassium carbonate $\displaystyle K_2CO_3 = 2(39)+12+3(16)=78+12+48=138\ u$
Formula unit mass for calcium oxide $\displaystyle CaO = 40+16=56\ u$
Formula unit mass for hydrochloric acid $\displaystyle HCl = 1+35.5=36.5\ u$
Formula unit mass for carbon monoxide $\displaystyle CO = 12+16=28\ u$
Formula unit mass for ammonia $\displaystyle NH_3 = 14+3(1)=17\ u$
Question 5
1 / -0

The heaviest among the following is:

A
$50\ g$ of $Fe$

B
$5\ moles$ of $N_2$

C
$0.1\ g \ atom$ of $Ag$

D
$0.1\ g$ of $Ca$

Solution

(A) $50$ g of $\displaystyle Fe$

(B) 5 moles of $\displaystyle N_2 = 5 \: mol \times 28 \: g/mol = 140$ g.

(C) 0.1 g atom of $Ag$ $\displaystyle = 0.1 \: g \: atom \times 108 \: g/ \: atom = 10.8$ g

(D) $0.1$ g $\displaystyle Ca$

Hence, 5 moles of $\displaystyle N_2$ are heaviest.
Question 6
1 / -0

What is the mass of one molecule of oxygen?

A
$5.31\times { 10 }^{ -23 }g$

B
$5.33\times { 10 }^{ 23 }g$

C
$5.25\times { 10 }^{ 23 }g$

D
$5.02\times { 10 }^{ -23 }g$

Solution

Explanation:
The molecular mass of oxygen ( $O_2$ ) is $32\ grams$ .

$\therefore$ $6.023 \times 10^{23}$ molecules of oxygen ( $O_2$ ) have mass $=32\ grams$ .

$\therefore$ One molecule of oxygen ( $O_2$ ) will have mass $=\dfrac{32}{6.023\times 10^{23}}=5.31\times 10^{-23}\ grams$ .

Final Answer: One molecule of oxygen ( $O_2$ ) have mass $=5.31\times 10^{-23}\ grams$ . Hence option $A$ is correct.
Question 7
1 / -0

Calculate the number of atoms present in $71 g$ of ${ Cl }_{ 2 }$ .

A
$1.205\times { 10 }^{ -24 }$ atoms

B
$1.205\times { 10 }^{ 23 }$ atoms

C
$1.205\times { 10 }^{ 24 }$ atoms

D
$1.205\times { 10 }^{ -23 }$ atoms

Solution

Weight of $\displaystyle Cl_2 = 71$ g

Molecular weight of $\displaystyle Cl_2$ $\displaystyle =71$ g/mol

Number of moles of $\displaystyle Cl_2$ $\displaystyle = \dfrac {71 \ g}{71 \ g/g atom}=1$ moles.

The Avogadro's number is $\displaystyle 6.023 \times 10^{23}$ molecules/mol.

The number of atoms of $\displaystyle Cl_2$ $\displaystyle =2$ atoms/molecule $\times 1$ mol $\displaystyle \times 6.023 \times 10^{23}$ molecules/mol
$\displaystyle =1.205 \times 10^{24}$ atoms
Question 8
1 / -0

Who was the first scientist to propose that all matter was made of small spheres called atoms?

A
John Dalton (early 1800's)

B
Ernest Rutherford (1911)

C
Niel's Bohr (1913)

D
Joseph John Thomson (1897)

Solution

John Dalton was the first scientist to propose that all matter was made of small spheres called atoms. The main points of Dalton's Atomic theory given by John Dalton are:-
(a) Elements are extremely small particles called atoms.
(b) Atoms of a given element are identical in size, mass, and other properties,
(c) Atoms cannot be sublimed, created, or destroyed.
(d) Atoms of different elements combine in simple whole-number ratios to form chemical compounds.
(e) In chemical reactions, atoms are combined, separated, or rearranged.
Option $A$ is correct.
Question 9
1 / -0

A smallest particle of a compound that can have the independence existence and that can retain all the properties of that compound is called as:

A
molecule

B
ion

C
atom

D
element

Solution

A smallest part of the compound that can have the independence existence and that can retain all the properties of that compound is called as molecule. Ex: $H_2,Cl_2$
Question 10
1 / -0

Which of the following term is denoted as Formula Mass Unit?

A
Compounds

B
Molecules

C
Molecules contains ions as constituents

D
None

Solution

Formula unit mass is the sum of the atomic masses of all the ions in the ionic compound. Formula unit mass is assigned to the ionic compounds.
Hence option C is correct.

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Atoms and Molecules Test - 53

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Question 1

62.02×102362.02\times { 10 }^{ 23 }62.02×1023 atoms

622×1023622\times { 10 }^{ 23 }622×1023 atoms

6.023×10236.023\times { 10 }^{ 23 }6.023×1023 atoms

6.02×10−236.02\times { 10 }^{ -23 }6.02×10−23 atoms

Solution

Question 2

10g10 g10g

20g20 g20g

30g30 g30g

40g40 g40g

Solution

Question 3

28.88

27

30

34

Solution

Question 4

Calcium chloride, potassium carbonate

Calcium oxide, hydrochloric acid

Carbon monoxide, ammonia

Carbon dioxide, nitrous oxide

Solution

Question 5

50 g50\ g50 g of FeFeFe

5 moles5\ moles5 moles of N2N_2N2​

0.1 g atom0.1\ g \ atom0.1 g atom of AgAgAg

0.1 g0.1\ g0.1 g of CaCaCa

Solution

Question 6

5.31×10−23g5.31\times { 10 }^{ -23 }g5.31×10−23g

5.33×1023g5.33\times { 10 }^{ 23 }g5.33×1023g

5.25×1023g5.25\times { 10 }^{ 23 }g5.25×1023g

5.02×10−23g5.02\times { 10 }^{ -23 }g5.02×10−23g

Solution

Question 7

1.205×10−241.205\times { 10 }^{ -24 }1.205×10−24 atoms

1.205×10231.205\times { 10 }^{ 23 }1.205×1023 atoms

1.205×10241.205\times { 10 }^{ 24 }1.205×1024 atoms

1.205×10−231.205\times { 10 }^{ -23 }1.205×10−23 atoms

Solution

Question 8

John Dalton (early 1800's)

Ernest Rutherford (1911)

Niel's Bohr (1913)

Joseph John Thomson (1897)

Solution

Question 9

molecule

ion

atom

element

Solution

Question 10

Compounds

Molecules

Molecules contains ions as constituents

None

Solution

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$62.02\times { 10 }^{ 23 }$ atoms

$622\times { 10 }^{ 23 }$ atoms

$6.023\times { 10 }^{ 23 }$ atoms

$6.02\times { 10 }^{ -23 }$ atoms

$10 g$

$20 g$

$30 g$

$40 g$

$50\ g$ of $Fe$

$5\ moles$ of $N_2$

$0.1\ g \ atom$ of $Ag$

$0.1\ g$ of $Ca$

$5.31\times { 10 }^{ -23 }g$

$5.33\times { 10 }^{ 23 }g$

$5.25\times { 10 }^{ 23 }g$

$5.02\times { 10 }^{ -23 }g$

$1.205\times { 10 }^{ -24 }$ atoms

$1.205\times { 10 }^{ 23 }$ atoms

$1.205\times { 10 }^{ 24 }$ atoms

$1.205\times { 10 }^{ -23 }$ atoms