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CBSE Questions for Class 9 Chemistry Atoms And Molecules Quiz 5 - MCQExams.com

An ionic compound of element M and chlorine has the formula MCl3, the molecular mass of MCl3 is 118.5 u. What is the molecular mass of the oxide of an element M?
  • 28
  • 44
  • 72
  • 99
The difference between ions and atoms is of :
  • relative size
  • electronic configuration
  • presence of charge
  • All of the above
14 g of element X combine with 16 g of oxygen. On the basis of this information, which of the following is a correct statement?
  • The element X could have an atomic weight of 7 and its oxide is XO.
  • The element X could have an atomic weight of 14 and its oxide is X2O.
  • The element X could have an atomic weight of 7 and its oxide is X2O
  • The element X could have an atomic weight of 16 and its oxide is X2O
Smallest particle of an element or a compound which is capable of independent existence is called:
  • atom
  • molecule
  • element
  • compound
A chemical equation is balanced in accordance with the law of
  • conservation of mass
  • multiple proportion
  • constant proportion
  • reciprocal proportion
Which law stated that 'matter is neither created nor destroyed'?
  • Law of multiple proportion
  • Law of conservation of energy
  • Law of constant composition
  • Law of conservation of mass
Which of these is not a molecule?
  • H2
  • Cl
  • O3
  • NaCl
The law of conservation of mass was given by :
  • Dalton
  • Proust
  • Lavoisier
  • Berzelius
One mole of any substance contains 6.023×1023 particles. It was determined by
  • Berzilius
  • Avogadro
  • Dalton
  • Perin
Which atom contains exactly 15 neutrons?
  • P32 (atomic number =17)
  • S32 (atomic number =16)
  • O15 (atomic number =8)
  • N15 (atomic number =7)
Amongst the following, which has the highest molecular mass?
  • Cl2
  • N2
  • CH3OH
  • NH3
In a chemical reaction, when 14 g of sodium carbonate reacted with 10g of acetic acid (ethanoic acid), then it was observed that, 16.67 g of sodium acetate solution in water and 7.33 g of carbon dioxide were produced. Which law does this depicts?
  • Law of definite proportions
  • Law of conservation of mass
  • Law of constant proportions
  • Avogadro's law
Which of the following elements has the same molecular mass as its atomic mass?
  • Nitrogen
  • Neon
  • Oxygen
  • Chlorine
The value of Avogadro number is
  • 6.25×1018
  • 6.022×1023
  • 96500
  • 3.12×1018
Any sample of pure water, irrespective of its source, contains 88.89% oxygen and 11.11 % hydrogen by mass. The data supports the:
  • Law of conservation of mass
  • Law of constant composition
  • Law of multiple proportion
  • Law of reciprocal proportion
720 g of water contains ______ moles of water.
  • 20
  • 40
  • 60
  • 80
Smallest possible unit of a compound which has independent existence is :
  • molecule
  • atom
  • ion
  • electron
The mass of Na present in 11.7 g of NaCl is:
  • 2.3 g
  • 4.6 g
  • 6.9 g
  • 7.1 g
Since Avogadro number is 6.023×1023 and atomic mass of nitrogen is 14 amu, one mole of N2 gas will have:
  • 0.5×6.023×1023 atoms
  • 2×6.023×1023 atoms
  • 14×6.023×1023 atoms
  • 28×6.023×1023 atoms
Radius of atom is of the order :
  • 1010108cm
  • 10121014cm
  • 10141016cm
  • 10161020cm
One atomic mass unit is equivalent to
  • 1.67×1027g
  • 1.66×1027kg
  • 1.67×1027mg
  • 1.6×1024g
2.40 g of the element Z combines exactly with 1.6 g of oxygen to form a compound with the formula ZO2. What is the relative atomic mass of Z?
  • 24.0
  • 32.0
  • 48.0
  • 64.0
The mass of one atom of carbon-12 is:
  • 1 g
  • 12 g
  • 12×6.02×1023 g
  • 126.02×1023 g
An atom is:
  • The smallest particle of matter known
  • The smallest particle of a gas
  • The smallest indivisible particle of an element that can take part in a chemical change
  • Radioactive emission
Atomic theory was given by:
  • John Dalton
  • Neils Bohr
  • E. Rutherford
  • Haber Bosch
'All matter is composed of very small particles called Parmanu' was first suggested by:
  • John Dalton
  • J.J. Thomson
  • Kanad
  • William J. Crooke
Which of the following contains the largest number of molecules?
  • 0.2 mole of H2
  • 8.0 mole of H2
  • 17 g of H2O
  • 6.0 g of CO2
Which of the following weighs the most?
  • 1023 molecules of H2
  • 1 mole of H2O
  • 1 mole of N2
  • 1022 molecules of O2
6.4 g of oxygen will contain ______ number of oxygen molecules.
  • 6.023×1023
  • 6.023×1022
  • 1.2046×1023
  • 1.2046×1022
Which of the following statement is wrong?
  • An atom is electrically neutral.
  • The size of a cation is smaller than that of the corresponding atom.
  • The size of an anion is bigger than that of the corresponding atom.
  • An atom and its ion have an unequal number of protons.
Which of the following compound has formula mass of 322 u?
(H=1,C=12,0=16,Na=23,S=32,Cu=63.5)
  • Na2CO3.10H2O
  • CuSO4.5H2O
  • Na2CO3.9H2O
  • Na2SO4.10H2O
Hydrogen combines with nitrogen in a 3:14 weight ratio to form ammonia. If every molecule of ammonia contains three atoms of hydrogen and one atom of nitrogen, an atom of nitrogen must weigh :
  • 14 times the mass of a hydrogen atom
  • 14/3 times the mass of a hydrogen atom
  • 3 times the mass of a hydrogen atom
  • 3/14 times the mass of a hydrogen atom
The sum of masses of the atoms in the molecules is known as :
  • Atomic mass
  • Molecular mass
  • Gram molecular weight
  • None of the above
The weight of one molecule of a compound of molecular formula C60H122 is:
  • 1.2×1020g
  • 5.025×1023g
  • 1.4×1021g
  • 6.023×1020g
Formula unit mass of NaHCO3 is :
  • 84 u
  • 76 u
  • 52 u
  • 64 u
Which among the following has molecular mass of 36.5 u?
  • Carbon molecules
  • Hydrogen molecules
  • Sulphur molecules
  • Hydrochloric acid
Molecular mass of nitric acid is:
  • 22 u
  • 12 u
  • 33 u
  • 63 u
Hydrogen combines with oxygen in a 1:8 weight ratio to form water. If every molecule of water contains two atoms of hydrogen and one atom of oxygen, an atom of oxygen must weigh:
  • 8 times the mass of a hydrogen atom
  • 16 times the mass of a hydrogen atom
  • 1/16 times the mass of a hydrogen atom
  • 1/8 times the mass of a hydrogen atom
1.008 grams of hydrogen combines with 35.453 g of chlorine to form 36.463 g of a pure compound (hydrogen chloride). Dalton's explanation for this experimental fact might be: 
  • One atom of hydrogen combines with 35.453 atoms of chlorine in this reaction
  • Hydrogen and chlorine atoms always combine in a 1:35 ratio.
  • Chlorine accepts hydrogen's electron to form polar covalent hydrogen chloride
  • Hydrogen and chlorine atoms aren't created or destroyed in the process so the reactant mass is the same as the product mass.
The symbol of copper is:
  • Co
  • Cr
  • Cp
  • Cu
What is the atomic mass (u) of chlorine?
  • 34
  • 35.5
  • 33
  • 35
The illustrations show a conservation-of-mass experiment. The solution in the beaker lost mass because
439573.jpg
  • materials have less mass at high temperatures
  • the mass of the reactants and products was less than 100 g
  • sodium sulfate (Na2SO4) is lighter than air
  • some of the water molecules turned into gas
In the procedure shown above, a calcium chloride solution is mixed with a sodium sulfate solution to create the products shown. Which of the following is illustrated by this activity?
439568.jpg
  • Law of conservation of mass
  • Law of definite proportions
  • Dalton's law atomic theory
  • Theory of covalent bonding
Mass can neither be created nor destroyed. This is in agreement with which law of chemical combination?
  • Law of definite proportion
  • Law of multiple proportion
  • Law of conservation of mass
  • Law of conservation of momentum

Compounds formed by metals and non-metals contain charged species which are known as:

  • cations
  • anions
  • Both A and C
  • None of the above
Which is not one of the laws of chemical combinations?
  • Law of multiple proportion
  • Law of conservation of mass
  • Law of conservation of energy
  • Law of definite proportion
Calculate the formula unit mass (u) of Na2O .
Atomic mass of Na=23 u,O=16 u
  • 60
  • 62
  • 61
  • 59
In a chemical reaction, 100g baking soda mixture containing sodium bicarbonate and vinegar on heating gives 43g of carbon dioxide gas. What mass of solid residue is left in food?
  • 54 g
  • 55 g
  • 56 g
  • 57 g
The formula unit mass of X is 342 u. Among the following, X is :
  • H2SO4
  • PbI2
  • Al2(SO4)3
  • Al(OH)3
Formula unit mass of CaCO3 is:
  • 104 u
  • 106 u
  • 100 u
  • 1144 u
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