Some Basic Concepts of Chemistry Test

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Question 1
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Two students performed the same experiment separately and each one of them recorded two readings of mass which are given below. Correct reading of mass is 3.0 g. On the basis of given data, mark the correct option out of the following statements.

Student Readings

A 3.01 2.99

B 3.05 2.95

A
Results of both the students are neither accurate nor precise

B
Results of student A are both precise and accurate

C
Results of student B are neither precise nor accurate

D
Results of student B are both precise and accurate

Question 2
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A measured temperature on Fahrenheit scale is 200° F. What will this reading be on Celsius scale?

A
40°C

B
94°C

C
93.3°C

D
30°C

Question 3
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What will be the molarity of a solution, which contains 5.85 g of NaCl(s) per 500 mL?

A
\(4\, mol\, L^{-1} \)

B
\(20\, mol\, L^{-1} \)

C
\(0.2\, mol\, L^{-1} \)

D
\(2\, mol\, L^{-1} \)

Question 4
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If 500 mL of a 5M solution is diluted to 1500 mL, what will be the molarity of the solution obtained?

A
1.5 M

B
1.66 M

C
0.017 M

D
1.59 M

Question 5
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The number of atoms present in one mole of an element is equal to Avogadro number. Which of the following element contains the greatest number of atoms?

A
4g He

B
46g Na

C
0.40g Ca

D
12g He

Question 6
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If the concentration of glucose (\(C_6H_{12}O_6\)) in blood is 0.9 g \(L^{–1}\), what will be the molarity of glucose in blood?

A
5 M

B
50 M

C
0.005 M

D
0.5 M

Question 7
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What will be the molality of the solution containing 18.25 g of HCl gas in 500 g of water?

A
0.1 m

B
1 M

C
0.5 m

D
1 m

Question 8
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One mole of any substance contains 6.022 x \(10^{23}\) atoms/molecules. Number of molecules of \(H_2SO_4\) present in 100 mL of 0.02M \(H_2SO_4\) solution is.........

A
12.044 x \(10^{20}\) molecules

B
6.022 x \(10^{23}\) molecules

C
1 x \(10^{23}\) molecules

D
12.044 x \(10^{23}\) molecules

Question 9
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What is the mass percent of carbon in carbon dioxide?

A
0.034%

B
27.27%

C
3.4%

D
28.7%

Question 10
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In the following questions a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct option out of the choices given below each question.

Assertion (A): The empirical mass of ethene is half of its molecular mass.

Reason (R): The empirical formula represents the simplest whole number ratio of various atoms present in a compound.

A
Both A and R are true and R is the correct explanation of A

B
A is true but R is false

C
A is false but R is true

D
Both A and R are false

Question 11

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Match the following:

	Column I		Column II
(i)	88 g of \(CO_2\)	(a)	0.25 mol
(ii)	6.022 x \(10^{23}\) molecules of \(H_2O\)	(b)	2 mol
(iii)	5.6 litres of \(O_2\) at STP	(c)	1 mol
(iv)	96 g of \(O_2\)	(d)	6.022 x \(10^{23}\) molecules
(v)	1 mol of any gas	(e)	3 mol

(i) → (d); (ii) → (c); (iii) → (a); (iv) → (e); (v) → (b)

(i) → (b); (ii) → (c); (iii) → (a); (iv) → (e); (v) → (d)

(i) → (d); (ii) → (e); (iii) → (a); (iv) → (c); (v) → (b)

(i) → (d); (ii) → (e); (iii) → (c); (iv) → (a); (v) → (b)

Question 12
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One mole of oxygen gas at STP is equal to......

(i) 6.022 x \(10^{23}\) molecules of oxygen

(ii) 6.022 x \(10^{23}\) atoms of oxygen

(iii) 16 g of oxygen

(iv) 32 g of oxygen

A
(i)

B
(iv)

C
(i),(iv)

D
(ii),(iv)

Question 13
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The empirical formula and molecular mass of a compound are \(CH_2O\) and 180 g respectively. What will be the molecular formula of the compound?

A
\(C_9H_{18}O_9\)

B
\(CH_2O\)

C
\(C_6H_{12}O_6\)

D
\(C_2H_4O_2\)

Question 14

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Match the following physical quantities with units

	Physical quantity		Unit
(i)	Molarity	(a)	g m\(L^{-1}\)
(ii)	Mole fraction	(b)	mol
(iii)	Mole	(c)	Pascal
(iv)	Molality	(d)	Unitless
(v)	Pressure	(e)	mol \(L^{-1}\)
(vi)	Luminous intensity	(f)	Candela
(vii)	Density	(g)	mol \(kg^{-1}\)
(viii)	Mass	(h)	N\(m^{-1}\)
		(i)	Kg

(i) → (d) (ii) → (e) (iii) → (b) (iv) → (g) (v) → (f), (h) (vi) → (c) (vii) → (a) (viii) → (i)

(i) → (e) (ii) → (d) (iii) → (b) (iv) → (g) (v) → (f), (h) (vi) → (c) (vii) → (a) (viii) → (i)

(i) → (e) (ii) → (d) (iii) → (b) (iv) → (g) (v) → (c), (h) (vi) → (f) (vii) → (a) (viii) → (i)

(i) → (e) (ii) → (d) (iii) → (b) (iv) → (f) (v) → (g), (h) (vi) → (a) (vii) → (c) (viii) → (i)

Question 15
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If the density of a solution is 3.12 g m\(L^{–1}\), the mass of 1.5 mL solution in significant figures is......

A
4.7g

B
4680 x 10\( ^{-3}\) g

C
4.680g

D
46.80g

Question 16
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Which of the following statements about a compound is incorrect?

A
A molecule of a compound has atoms of different elements

B
A compound cannot be separated into its constituent elements by physical methods of separation

C
A compound retains the physical properties of its constituent elements

D
The ratio of atoms of different elements in a compound is fixed

Question 17
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In the following questions a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct option out of the choices given below each question.

Assertion (A): One atomic mass unit is defined as one twelfth of the mass of one carbon-12 atom.

Reason (R): Carbon-12 isotope is the most abundunt isotope of carbon and has been chosen as standard.

A
Both A and R are true and R is the correct explanation of A

B
Both A and R are true but R is not the correct explanation of A

C
A is true but R is false

D
Both A and R are false

Question 18
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Sulphuric acid reacts with sodium hydroxide as follows:

\(H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O\)

When 1L of 0.1M sulphuric acid solution is allowed to react with 1L of 0.1M sodium hydroxide solution, the amount of sodium sulphate formed and its molarity in the solution obtained is

(i) 0.1 mol \(L^{–1}\)

(ii) 7.10 g

(iii) 0.025 mol \(L^{–1}\)

(iv) 3.55 g

A
(i),(ii)

B
(ii),(iii)

C
(i),(iv)

D
(ii),(iv)

Question 19
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In the following questions a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct option out of the choices given below each question.

Assertion (A): Significant figures for 0.200 is 3 where as for 200 it is 1.

Reason (R): Zero at the end or right of a number are significant provided they are not on the right side of the decimal point.

A
Both A and R are true and R is correct explanation of A

B
Both A and R are true but R is not a correct explanation of A

C
A is true but R is false

D
Both A and R are false

Question 20
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Which of the following pairs have the same number of atoms?

(i) 16 g of \(O_2\)(g) and 4 g of \(H_2\)(g)

(ii) 16 g of \(O_2\) and 44 g of C\(O_2\)

(iii) 28 g of \(N_2\) and 32 g of \(O_2\)

(iv) 12 g of C(s) and 23 g of Na(s)

A
(i),(iii)

B
(ii),(iii)

C
(ii),(iv)

D
(iii),(iv)

Question 21
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Which of the following solutions have the same concentration?

(i) 20 g of NaOH in 200 mL of solution

(ii) 0.5 mol of KCl in 200 mL of solution

(iii) 40 g of NaOH in 100 mL of solution

(iv) 20 g of KOH in 200 mL of solution

A
(i),(ii)

B
(i),(iii)

C
(ii),(iii)

D
(ii),(iv)

Question 22
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Which of the following statements is correct about the reaction given below:

4Fe(s) + 3\(O_2\)(g) → 2\(Fe_2O_3\)(g)

A
Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore it follows law of conservation of mass

B
Total mass of reactants = total mass of product; therefore, law of multiple proportions is followed

C
Amount of \(Fe_2O_3\) can be increased by taking any one of the reactants (iron or oxygen) in excess

D
Amount of \(Fe_2O_3\) produced will decrease if the amount of any one of the reactants (iron or oxygen) is taken in excess

Question 23
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Which of the following reactions is not correct according to the law of conservation of mass.

A
\(2Mg(s)+O_2(g)\rightarrow2MgO(s)\)

B
\(C_3H_8(g) + O_2(g) \rightarrow CO_2(g) + H_2O(g)\)

C
\(P_4(s) + 5O_2(g) \rightarrow P_4O_{10}(s)\)

D
\(CH_4(g) + 2O_2(g)\rightarrow CO_2(g) + 2H_2O (g)\)

Question 24
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16 g of oxygen has same number of molecules as in

(i) 16 g of CO

(ii) 28 g of \(N_2\)

(iii) 14 g of \(N_2\)

(iv) 1.0 g of \(H_2\)

A
(i),(ii)

B
(ii),(iii)

C
(iii),(iv)

D
(i),(iv)

Question 25
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Which of the following statements indicates that law of multiple proportion is being followed.

A
Sample of carbon dioxide taken from any source will always have carbon and oxygen in the simple ratio 1:2

B
Carbon forms two oxides namely \(CO_2\) and CO, where masses of oxygen which combine with fixed mass of carbon are in the simple ratio 2:1

C
When magnesium burns in oxygen, the amount of magnesium taken for the reaction is equal to the amount of magnesium in magnesium oxide formed

D
At constant temperature and pressure 200 mL of hydrogen will combine with 100 mL oxygen to produce 200 mL of water vapour

Question 26
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Which of the following terms are unitless?

(i) Molality

(ii) Molarity

(iii) Mole fraction

(iv) Mass percent

A
(i),(iv)

B
(iii),(iv)

C
(ii),(iii)

D
(i),(ii)

Question 27
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In the following questions a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct option out of the choices given below each question.

Assertion (A): Combustion of 16 g of methane gives 18 g of water.

Reason (R): In the combustion of methane, water is one of the products.

A
Both A and R are true but R is not the correct explanation of A

B
A is true but R is false

C
A is false but R is true

D
Both A and R are false

Question 28
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One of the statements of Dalton’s atomic theory is given below: “Compounds are formed when atoms of different elements combine in a fixed ratio”. Which of the following laws is not related to this statement?

(i) Law of conservation of mass

(ii) Law of definite proportions

(iii) Law of multiple proportions

(iv) Avogadro law

A
(i),(ii)

B
(ii),(iii)

C
(iii),(iv)

D
(i),(iv)

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Question Analysis

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Unanswered - 28

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Student	Readings
A	3.01	2.99
B	3.05	2.95

Some Basic Conc...

Question 1

Results of both the students are neither accurate nor precise

Results of student A are both precise and accurate

Results of student B are neither precise nor accurate

Results of student B are both precise and accurate

Question 2

40°C

94°C

93.3°C

30°C

Question 3

\(4\, mol\, L^{-1} \)

\(20\, mol\, L^{-1} \)

\(0.2\, mol\, L^{-1} \)

\(2\, mol\, L^{-1} \)

Question 4

1.5 M

1.66 M

0.017 M

1.59 M

Question 5

4g He

46g Na

0.40g Ca

12g He

Question 6

5 M

50 M

0.005 M

0.5 M

Question 7

0.1 m

1 M

0.5 m

1 m

Question 8

12.044 x \(10^{20}\) molecules

6.022 x \(10^{23}\) molecules

1 x \(10^{23}\) molecules

12.044 x \(10^{23}\) molecules

Question 9

0.034%

27.27%

3.4%

28.7%

Question 10

Both A and R are true and R is the correct explanation of A

A is true but R is false

A is false but R is true

Both A and R are false

Question 11

(i) → (d); (ii) → (c); (iii) → (a); (iv) → (e); (v) → (b)

(i) → (b); (ii) → (c); (iii) → (a); (iv) → (e); (v) → (d)

(i) → (d); (ii) → (e); (iii) → (a); (iv) → (c); (v) → (b)

(i) → (d); (ii) → (e); (iii) → (c); (iv) → (a); (v) → (b)

Question 12

(i)

(iv)

(i),(iv)

(ii),(iv)

Question 13

\(C_9H_{18}O_9\)

\(CH_2O\)

\(C_6H_{12}O_6\)

\(C_2H_4O_2\)

Question 14

(i) → (d) (ii) → (e) (iii) → (b) (iv) → (g) (v) → (f), (h) (vi) → (c) (vii) → (a) (viii) → (i)

(i) → (e) (ii) → (d) (iii) → (b) (iv) → (g) (v) → (f), (h) (vi) → (c) (vii) → (a) (viii) → (i)

(i) → (e) (ii) → (d) (iii) → (b) (iv) → (g) (v) → (c), (h) (vi) → (f) (vii) → (a) (viii) → (i)

(i) → (e) (ii) → (d) (iii) → (b) (iv) → (f) (v) → (g), (h) (vi) → (a) (vii) → (c) (viii) → (i)

Question 15

4.7g

4680 x 10\( ^{-3}\) g

4.680g

46.80g

Question 16

A molecule of a compound has atoms of different elements

A compound cannot be separated into its constituent elements by physical methods of separation

A compound retains the physical properties of its constituent elements