6 litre chlorine is reacted with 10 litre sodium. The excess amount of sodium is _

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The balanced equation is 2Na+Cl2=2NaCl Ratio is = 2:1:2. 6 litre chlorine reacts with 12 litre sodium. So, there is no excess of sodium.

What volume of carbon di oxide would be required to burn completely 500 ml of acetylene?

Correct! Wrong!

The balanced equation of combustion of acetylene is 2C2H2+5O2=4CO2+2H2O 2Vols = 500 ml or, 4 vols = 1000ml

A person adds 2 gms of sugar (C12H22O11)in order to sweeten his coffee. The number of carbon atoms added to his coffee would be ____. (Molar mass of sugar = 342)

Correct! Wrong!

1 mole of any substance contains 6.023 × 1023 atoms. 1 mole of any substance would weigh molar mass of that substance. Therefore, 342 gms of sugar = 1 mole of sugar 342 gms of sugar = 6.023 × 1023 molecules of sugar or 12 × 6.023 × 1023 atoms of carbon When 2 gms of sugar are added, the carbon atoms added = 12 × 6.023 × 1023 atoms of carbon × 2 ÷ 342 = 4.226 × 1022 atoms of carbon.

Atomicity is _

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Number of atoms in a molecule

Ozone is _

Correct! Wrong!

Formula of ozone is O3. So, the atomicity is 3 i.e. it is a triatomic molecule.

Of the options given below, which pair has same percentage of carbon?

Correct! Wrong!

Calculate the percentage of carbon in each compound. % age = mass of carbon present × 100 ÷ molar mass of the compound C6H12O6 = 6 × 12 × 100 ÷ 180 = 40% C12H22O11 = 12 × 12 × 100 ÷ 342 = 42% CH3COOH = 12 × 2 × 100 ÷ 60 = 40 % C2H5OH = 12 × 2 × 100 ÷ 46 = 52%

The molarity of commercially available concentrated sulphuric acid of 95% by mass would be ____. (Given the density of sulphuric acid is 1.84 gm cm-3)

Correct! Wrong!

Density = 1.84 gm/cc; 1 cc contains 1.84 gm of sulphuric acid Therefore, 1 litre will contain 1.84 × 1000 = 1840 gms. Percentage purity of sulphuric acid = 95 % Therefore, mass of pure sulphuric acid present = 95 × 1840 ÷ 100 = 1748 gms. Hence, molarity = mass/molar mass = 1748 ÷ 98 = 17.8 M

In Boyle’s Law the fixed parameter is _

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Boyle’s law state that at constant temperature pressure of a given mass of a dry gas is inversely proportional to its volume.

A student analysed a given inorganic salt to determine the water of crystallization. The observations recorded are: Fe2+= 14.32 %; SO42- = 49 %; NH4+= 9.2 % and H2O = 27.57 % The reported number of moles of water in the salt would be ____ .

Correct! Wrong!

Therefore, the number of moles of water = 6 moles in the salt (It is the water of crystallization)

Octatomic molecule is

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Octatomic molecule composed of 8 similar atoms.

What is the empirical formula of Butane?

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Molecular Formula is = C4H10 Ratio of C, H is = 4:10 Simple ratio = 2:5 Empirical Formula = C2H5

What is the total mass of products in the following equation: 2KClO3→2KCl+3O22KClO3→2KCl+3O2 (catalyst)

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Total mass of product = 2(39 + 35.5) + 3(32) = 149 + 96 = 245g

In Avogadro Law, the fixed parameter is

Correct! Wrong!

Avogadro’s Law states that equal volumes of all gases under similar conditions of temperature and pressure contain the same number of molecules.

160 c.c acetylene reacts with 500c.c oxygen. Calculate the total volume of resulting gaseous mixture.

Correct! Wrong!

The balanced equation of combustion of acetylene is 2C2H2 (g) +5O2 (g) =4CO2 (g) +2H2O (l) 2 VOLS = 160 c.c 1 vol = 80 c.c 5 vol of oxygen = 400c.c so, (500-400) c.c = 100 c.c is unreacted. 4 vols = 320 c.c Water is in liquid state. Total volume = (100+320) c.c = 420 c.c

An analysis of an inorganic salt gave the following percentage composition: Na = 14.28 %; S = 9.92 %; H = 6.20 % Assuming all the hydrogen combines with oxygen to form water, and the molecular mass of the crystalline salt is 322, the correct molecular formula would be ____ .

Correct! Wrong!

Hence, the empirical formula is Na2SH20O14 The molecular formula = n × empirical formula or n = molecular weight/ empirical formula weight Molecular weight = 322 Empirical formula weight = 2 × 23 + 1 × 32 + 20 × 1 + 14 × 16 = 322 n = 322 / 322 = 1 So, the molecular formula is same as empirical formula.

Of the options given, ____ is the heaviest.

Correct! Wrong!

Option A - 1 mole of Oxygen = 32 gms Option B - 10 moles of hydrogen = 2 × 10 = 20 gms Option C - 44 gms of carbon dioxide Option D - 1 molecule of sulphur dioxide = 64/ 6.023 × 1023 = 10.6 × 10-23 gms Hence, Option C is the heaviest.

Given are four mathematical relationships. The incorrect expression is ____.

Correct! Wrong!

The incorrect expression is Number of moles = Atomic mass ÷ Mass of the element in grams. The correct expression for Number of moles = mass in gms ÷ molar mass

Mass and temperature both are fixed in _

Correct! Wrong!

Boyle’s law state that at constant temperature pressure of a given mass of a dry gas is inversely proportional to its volume.

Molecular mass of sugar is (in a. m. u) _

Correct! Wrong!

Formula is C12H22O11 Molecular mass= (12×12) + (1×22) + (11×16) = 144 + 22 + 176 = 342 a. m. u

What is the ratio of carbon dioxide prepared from CO and O2?

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The reaction is 2CO+O2=2CO And the ratio is = 2:1:2

150c.c of ethylene burnt in sufficient air. The amount of required oxygen is

Correct! Wrong!

The balanced equation of combustion of acetylene is C2H4+3O2 = 2H2O 1 vol ethylene require 3 volumes of oxygen. (3×150) = 450c.c of oxygen.

____ moles of magnesium phosphate will contain 0.25 moles of oxygen.

Correct! Wrong!

8 moles of oxygen are present in =1 mole of magnesium phosphate (Mg3 (PO4)2) 0.25 moles of oxygen = 1 × 0.25 ÷ 8 = 3.125 × 10-2 moles

The mass of carbon present in 0.5 mole of K4[Fe(CN)6] is ____.

Correct! Wrong!

1 mole of K4[Fe (CN)6] contains 6 gm. atom of carbon atoms. 0.5 mole of K4[Fe (CN)6] will contain 6 x 0.5 = 3 gm atom of carbon atoms. Hence, mass of carbon present in 0.5 mole of K4[Fe (CN)6] = 3 x 12 = 36 gms.

What volume of oxygen would be required to burn completely 350 ml of acetylene?

Correct! Wrong!

The balanced equation of combustion of acetylene is 2C2H2+5O2=4CO2+2H2O 2Vols = 350 ml or, 5 vols = 875 ml

Phosphorus is

Correct! Wrong!

Tetratomic molecule composed of 4 similar atoms.

ICSE Class 10th Chemistry 4 - Mole Concept and Stoichiometry MCQs
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