ln, a closed vessel, 50 ml of A 2 B 3 completely reacts with 200 ml of C 2 according to the following equation: 2 A 2 B 3 ( g ) + 5 C 2 ( g ) → 3 C 3 B 2 ( g ) + C A 4 ( g ) The composition of the gaseous mixture in the system will be:

75 ml C 2 , 75 m l C 3 B 2 , 25 m l C A 4

100 ml C 2 , 50 m l C 3 B 2 , 50 m l C A 4

25 ml C 2 , 75 m l C 3 B 2, 25 m l C A 4

10 ml C 2 , 25 m l C 3 B 2 , 100 m l C A 4

On complete combustion, 44 g of a sample of a compound gives 88 g CO 2 and 36 g of H 2 O. The molecular formula of the compound may be:

Chemistry - Basic Concepts Chemistry - Quiz-6

60 mL of a mixture of nitrous oxide and nitric oxide was exploded with excess of hydrogen. If 38 mL of $N_{2}$ was formed, calculate the volume of each gas in the mixture. All measurements are made at constant P and T.

0%

20 ml +30 ml
0%

44 ml + 16 ml
0%

10 ml+40 ml
0%

4 .25 ml +25 ml

2.0 g sample containing ${Na}_{2} {CO}_{3}$ and ${NaHCO}_{3}$ loses 0.248 g when heated to 300 $°$ C, the temperature at which ${NaHCO}_{3}$ decomposes to ${Na}_{2} {CO}_{3}$ , ${CO}_{2}$ and $H_{2} O$ . What is the % of ${Na}_{2} {CO}_{3}$ in mixture?

0%

66.5
0%

50.6
0%

60.5
0%

6.65

1.640 ml

2.540 ml

3.500 ml

4.600 ml

0%

A sample of ${CaCO}_{3}$ and ${MgCO}_{3}$ weighed 2.21 g is ignited to constant mass of 152 g. What is the composition of mixture? Also calculate the volume of ${CO}_{2}$ evolved at $0 ° C$ and 76 cm of pressure.
0%
2
0%
3
0%
4

The average molar mass of the mixture of ${CH}_{4}$ and $C_{2} H_{4}$ present in the mole ratio of a:b is 20 g mol^-1. When the mole ratio is reversed, the molar mass of the mixture will be:

0%

24 gram
0%

42 gram
0%

20 gram
0%

15 gram

Vapour density of a volatile substance is 4 $({CH}_{4} = 1)$ . Its molar mass would be:

0%

8
0%

2
0%

64
0%

128

The haemoglobin from the red blood corpuscles contains approximately 0.33% iron by mass. The molar mass of haemoglobin is 67,200. The number of iron atoms in each molecule of haemoglobin is -
(atomic mass of iron=56):

0%
2
0%
3
0%
4
0%
5

The vapour density of a volatile chloride of a metal is 95 and the specific heat of the metal is 0.13 cal/g. The equivalent mass of the metal will be:

0%

6
0%

12
0%

18
0%

24

Which mixture is lighter than humid air?

0%

$N_{2} + O_{2} + {SO}_{2}$
0%

$N_{2} + O_{2} + {CO}_{2}$
0%

$N_{2} + O_{2} + C_{2} H_{6}$
0%

$N_{2} + O_{2} + He$

$O_{3}$ is absorbed by:

0%

Pyrogallol
0%

Menthol
0%

Turpentine oil
0%

Clove oil

Read the following statements (S) and Explanation (E). Choose the correct answers from the codes (1), (2), (3) and (4):

S : An element may have variable equivalent mass.

E : Such elements should possess variable valency.

0%

S is correct but E is wrong
0%
S is wrong but E is correct
0%
Both S and E are correct and E is correct explanation of S
0%
Both S and E are correct but E is not correct explanation of S

0.5 g of fuming $H_{2} {SO}_{4}$ (oleum) is diluted with water. The solution requires 26.7 mL of 0.4 N $NaOH$ for complete neutralization. Find the % of free ${SO}_{3}$ in the sample of oleum. Also report % of oleum solution.

0%

104.68 %
0%

98 %
0%

106.13%
0%

56 %

Calculate the mass of $CaO$ required to remove the hardness of $10^{6}$ litre of water containing 1.62 g of calcium bicarbonate per litre.

0%

5.6*10^-6
0%

5.6*10^5
0%

4.8*10^9
0%

1.2*10^-4

At 100ºC and 1 atm, if the density of liquid water is 1.0 g cm^–3 and that of water vapor is

0.0006 g cm^-3, then the volumeoccupied by water molecules in 1 litre of steam at that temperature will be:

0%

6 cm³
0%

60 cm³
0%

0.6 cm³
0%

0.06 cm³

The hydrated salt Na₂SO₄.nH₂O, undergoes 55% loss in weight on heating and becomes anhydrous. The value of n will be -

0%

5
0%

3
0%

7
0%

10

10 g of a silver coin when dissolved completely in
excess of conc. HNO $_{3}$ gives 8.5 g of silver nitrate.
The percentage purity of the coin is

0%

25%
0%

54%
0%

67%
0%

100%

What is the molality of pure water?

0%

1 m
0%

18 m
0%

55.5 m
0%

None of the above

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

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

0%

Both the assertion and the reason are true and the reason is the correct explanation of the assertion.
0%
Both the assertion and the reason are true and the reason is not the correct explanation of the assertion.
0%
The assertion is true but the reason is false.
0%
The assertion is false but the reason is true.

A bottle of $H_{3} {PO}_{4}$ solution contains 70% (w/w) acid. If the density of the solution is 1.54 g ${cm}^{- 3}$ , the volume of the $H_{3} {PO}_{4}$ solution required to prepare 1 L of 1 N solution is

0%

90mL
0%

45 mL
0%

30 mL
0%

23 mL

The density of a 2 M aqueous solution of NaOH is 1.28 g/ $c m^{3}$ . The molality of the solution is

[molecular mass of NaOH = 40 $g m o l^{- 1}$ ]

0%

1.20 m
0%

1.56 m
0%

1.67 m
0%

1.32 m

Assertion: 1 g $O_{2}$ and 1 g $O_{3}$ have an equal number of oxygen atoms.

Reason: $O_{2}$ and $O_{3}$ have different molar masses.

0%

Both the assertion and the reason are true and the reason is the correct explanation of the assertion.
0%
Both the assertion and the reason are true and the reason is not the correct explanation of the assertion.
0%
The assertion is true but the reason is false.
0%
The assertion is false but the reason is true.

ln, a closed vessel, 50 ml of $A_{2} B_{3}$ completely reacts with 200 ml of C₂ according to the following equation:

$2 A_{2} B_{3} (g) + 5 C_{2} (g) \to 3 C_{3} B_{2} (g) + C A_{4} (g)$

The composition of the gaseous mixture in the system will be:

0%

100 ml $C_{2}, 50 m l C_{3} B_{2}, 50 m l C A_{4}$
0%

25 ml $C_{2}, 75 m l C_{3} B_{2,} 25 m l C A_{4}$
0%

75 ml $C_{2}, 75 m l C_{3} B_{2,} 25 m l C A_{4}$
0%

10 ml $C_{2}, 25 m l C_{3} B_{2,} 100 m l C A_{4}$

3. $C_{2} H_{4} O$

0%

$C_{4} H_{6}$
0%

$C_{2} H_{6} O$
0%

$C_{3} H_{6} O$
0%
On complete combustion, 44 g of a sample of a compound gives 88 g CO₂ and 36 g of H₂O. The molecular formula of the compound may be:

The maximum number of atoms is present in the following -

0%

1 g of Li_(s)
0%

1 g of Mg_(s)
0%

1 g of O₂ _(g)
0%

1 g of Ag_(s)

The same number of molecules as 16 g of dioxygen is present in -

0%

16 g O $_{3}$
0%

16 g SO $_{2}$
0%

32 g SO $_{2}$
0%

All of above

The number of moles present in 2.5 litres of 0.2 M $H_{2} {SO}_{4}$ is -

0%

0.25
0%

0.5
0%

0.75
0%

0.2

Which of the following statements is correct?

0%
1 mole of electrons weights 5.4 mg
0%
1 mole of electrons weights 5.4 kg
0%
1 mole of electrons weights 0.54 mg
0%
1 mole of electrons has 1.6 $\times 10^{- 19}$ C of charge

Which of the following is the odd one with regard to mass?

0%

1 g atom of sulphur
0%

0.5 moles of CO $_{2}$
0%

1 mole of O $_{2}$
0%

3 x 10 ²³ molecules of SO $_{2}$

The weight of one molecule of a compound C₆₀H₁₂₂ is

0%

$5.005 \times 10^{23} g$
0%

$6.023 \times 10^{23} g$
0%

$4.1 \times 10^{- 21} g$
0%

$1.4 \times 10^{- 21} g$

Breakfast cereal is advertised to contain 110 mg of sodium/ 100 grams of cereal. The percent of sodium in the cereal is

0%

0.110%
0%

0.0110 %
0%

11.0%
0%

0.22 %

The percentage weight of Zn in white vitriol [ZnSO₄.7H₂O] is approximately equal to (Zn=65, S=32, O=16 and H=1)

0%

21.56%
0%

32.58%
0%

22.65%
0%

26.55%

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Practice Chemistry Quiz Questions and Answers

0:0:1

Practice Chemistry Quiz Questions and Answers

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