Assertion: The number of molecules in 2 moles of NH 3 is equal to the number of molecules in 4 moles of CH 4 . Reason: Both are chemically similar species.

Both Assertion and Reason are false statements.

Both the assertion and the reason are true and the reason is not the correct explanation of the assertion.

The assertion is true but the reason is false.

Both the assertion and the reason are true and the reason is the correct explanation of the assertion.

Assertion: When 4 moles of H 2 reacts with 2 moles of O 2 , then 4 moles of water are formed. Reason: O 2 will act as a limiting reagent.

Assertion is a true statement but Reason is false.

Both Assertion & Reason are true and the reason is the correct explanation of the assertion.

Both Assertion & Reason are true but the reason is not the correct explanation of the assertion.

Assertion and Reason are false statements.

Chemistry - Basic Concepts Chemistry - Quiz-8

Which of the following statements is correct about the reaction is given below?

$4 Fe (s) + 3 O_{2} (g) \to 2 {Fe}_{2} O_{3} (g)$

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Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore it follows law of conservation of mass
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Total mass of reactants = total mass of product, therefore, law of multiple proportions is followed
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Amount of Fe₂O₃ can be increased by taking any one of the reactants (iron or oxygen) in excess
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Amount of Fe₂O₃ produced will decrease if the amount of any one of the reactants (iron or oxygen) is taken in excess

Which of the following reactions is not correct according to the law of conservation of mass?

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$2 Mg (s) + O_{2} (g) \to 2 MgO (s)$
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$C_{3} H_{8} (g) + O_{2} (g) \to {CO}_{2} (g) + H_{2} O (g)$
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$P_{4} (s) + 5 O_{2} (g) \to P_{4} O_{10} (s)$
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${CH}_{4} (g) + 2 O_{2} (g) \to {CO}_{2} (g) + 2 H_{2} O (g)$

Which of the following statement indicates that the law of multiple proportions is being followed?

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A sample of carbon dioxide taken from any source will always have carbon and oxygen in the ratio of 1:2.
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Carbon forms two oxides namely, CO₂ and CO, where masses of oxygen that combine with a fixed mass of carbon are in the simple ratio of 2:1.
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When magnesium burns in oxygen, the amount of magnesium used for the reaction is equal to the amount of magnesium formed in magnesium oxide.
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At constant temperature and pressure, 200 mL of hydrogen will combine with 100 mL of oxygen to produce 200 mL of water vapour.

Match the following.

COLUMN I	COLUMN II
A. 88 g of CO₂	1. 0.25 mol
B. 6.022×10²³molecules of H₂O	2. 2 mol
C. 5.6 L of O₂at STP	3. 3 mol
D. 96 g of O₂	4. 1 mol

Codes

A B C D

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4. 4 1 3 2
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3. 1 4 3 2
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2. 1 2 3 4
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1. 2 4 1 3

Match the following physical quantities with units.

Physical quantity	Unit
A. Molarity	1. mol kg^-1
B. Molality	2. mol L^-1
C. Pressure	3. Candela
D. Luminous intensity	4. Pascal

Codes

A B C D

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4. 4 1 3 2
0%

3. 1 4 3 2
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2. 2 1 4 3
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1. 1 4 2 3

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

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

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Both the assertion and the reason are true and the reason is the correct explanation of the assertion.
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Both the assertion and the reason are true and the reason is not the correct explanation of the assertion.
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The assertion is true but the reason is false.
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The assertion is false but the reason is true.

Assertion(A): The significant figure for 0.200 is 3, whereas the significant figure for 200 is 1.

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

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Both the assertion and the reason are true and the reason is the correct explanation of the assertion.
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Both the assertion and the reason are true and the reason is not the correct explanation of the assertion.
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The assertion is true but the reason is false.
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The Assertion is false but the reason is true.

Assertion: The combustion of 16 g of methane gives 18 g of water.

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

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Both the assertion and the reason are true and the reason is the correct explanation of the assertion.
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Both the assertion and the reason are true and the reason is not the correct explanation of the assertion.
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The assertion is true but the reason is false.
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The assertion is false but the reason is true.

One mole of carbon atom weighs 12 g, the number of atoms in it is equal to, (Mass of carbon – 12 is $1.9926 \times 10^{- 23} g$ )

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(1) $1.2 \times 10^{23}$
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(2) $6.022 \times 10^{22}$
0%

(3) $12 \times 10^{22}$
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(4) $6.022 \times 10^{23}$

When 22.4 L of H₂ (g) is mixed with 11.2 L of Cl₂ (g), each at STP, the moles of HCl(g) formed is equal to -

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1 mole of HCl (g)
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2 moles of HCl (g)
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0.5 mole of HCl (g)
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1.5 mole of HCl (g)

Assertion: 1 a.m.u = $1 .66 \times 10^{- 24} gram .$

Reason: The actual mass of one atom of C-12 is equal to $1.99 \times 10^{- 23} g .$

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Both the assertion and the reason are true and the reason is the correct explanation of the assertion.
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Both the assertion and the reason are true and the reason is not the correct explanation of the assertion.
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The assertion is true but the reason is false.
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The assertion is false but the reason is true.

Assertion: The number of molecules in 2 moles of NH₃ is equal to the number of molecules in 4 moles of CH₄.

Reason: Both are chemically similar species.

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Both the assertion and the reason are true and the reason is not the correct explanation of the assertion.
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The assertion is true but the reason is false.
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Both Assertion and Reason are false statements.
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Both the assertion and the reason are true and the reason is the correct explanation of the assertion.

Assertion: When 4 moles of H₂ reacts with 2 moles of O₂, then 4 moles of water are formed.

Reason: O₂ will act as a limiting reagent.

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Both Assertion & Reason are true and the reason is the correct explanation of the assertion.
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Both Assertion & Reason are true but the reason is not the correct explanation of the assertion.
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Assertion is a true statement but Reason is false.
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Assertion and Reason are false statements.

Which has the maximum number of molecules among the following?

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64 g SO₂
0%

44 g CO₂
0%

48 g O₃
0%

8 g H₂

Percentage of C, H & N are given as follows :
C = 40% H = 13.33% N = 46.67%
The empirical formula will be :

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$C H_{2} N$
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$C_{2} H_{4} N$
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$C H_{4} N$
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$C H_{3} N$

Number of significant figures in the following numbers are :
(I) 161 cm
(II) 0.0161
(III) 1.61

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3 , 3, 3
0%
(3) 3 , 2 , 3
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(4) 3 , 4 , 4
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(2) 3 , 4 , 3

In haemoglobin (Molecular wt = 67200) iron found is 0.33% (by weight). The number of iron atom(s) in its one molecule will be

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1
0%
2
0%
3
0%
4

$4 N H_{3} + 5 O_{2} \to 6 H_{2} O + 4 N O$

When one mole ammonia and one mole oxygen are taken :
1. Oxygen is completely consumed

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3. Both and (2) are correct
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2. Ammonia is completely consumed
0%
3
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4. None of the above options is correct

The maximum number of molecules is present in:-

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5L of N₂ gas at STP
0%

0.5 g of H₂ gas
0%

10g of O₂ gas
0%

15 L of H₂ gas at STP

What is false for mole fraction :

0%
x < 1
0%
– 2 ≤ x ≤ 2
0%
0 ≤ x ≤ 1
0%
Always non-negative

Volume of CO₂ obtained by the complete decomposition of 9.85 gm. BaCO₃ is :

0%

2.24 lit.
0%

1.12 lit.
0%

0.84 lit.
0%

0.56 lit

1 M and 2.5 litre NaOH solution mixed with another 0.5 M and 3 litre NaOH solution. Molarity of the resultant solution is : -

0%

0.80 M
0%

1.0 M
0%

0.73 M
0%

0.50 M

Which has maximum number of molecules : -

0%

7 gm N₂
0%

2 gm H₂
0%

16 gm NO₂
0%

16 gm O₂

The percentage of C, H and N in an organic compound are 40%, 13.3% and 46.7% respectively , The empirical formula of the compound is :

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C₃H₁₃N₃
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CH₂N
0%

CH₄N
0%

CH₆N

Molarity of liquid HCl if density of liq. HCl is 1.17 gm/cc : -

0%

36.5
0%
18.25
0%
32.05
0%
42.10

Molar mass of (i) $H_{2} O$ (ii) ${CO}_{2}$ (iii) ${CH}_{4}$ are respectively:

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18,16,44
0%

18,44,16
0%

16,18,44
0%

44,16,18

In sodium sulphate (Na2SO4), the mass percent of sodium, sulfur and oxygen is

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32.4%, 45.05%, 22.6%
0%

22.6%, 45.05%, 32.4%
0%

32.4%, 22.6%, 45.05%
0%

45.05%, 32.4%, 22.6%

The amount of ${CO}_{2}$ (in grams) that could be produced when 2 moles of carbon is burnt in 16 g of dioxygen is -

0%

22
0%

44
0%

0.5
0%

11

The amount of copper (in grams) that can be obtained from 100 g of copper sulfate ( ${CuSO}_{4}$ )is

0%

54.00
0%

39.81
0%

63.50
0%

159.50

In an iron oxide, the mass percent of iron and oxygen are 69.9 and 30.1, respectively. The empirical formula of the oxide of iron will be

0%

Fe₃O₂
0%

Fe₂O₂
0%

Fe₂O₃
0%

Fe₃O₄

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Practice Chemistry Quiz Questions and Answers

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Practice Chemistry Quiz Questions and Answers

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