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WorksheetsChemistry XI (CHAPTER 1)
Total questions: 46
Worksheet time: 29mins
To convert given mass of substance into mole, we ___ it by molar mass.
Divide
Multiply
Add
Substract
If moles are needed to be converted into mass, we simply ___ them with molar mass.
Divide
Multiply
Add
Substract
Hydrogen gas is commercially prepared by ___.
Ethane process
Steam methane process
Steam ethane process
Methane process
The actual amount of product which is formed in experiment is called ___.
Practical yield
Actual yield
Both
None of these
The unit for molar mass is ___.
g/mol
mg/mol
kg/mol
mol
A mole is defined as gram atomic mass of any substance (atoms, molecules, ions) which contains ___ particles.
6.02×10^23
6.02×10^24
6.02×10^25
6.02×10^26
The number of particles present in one mole of any substance is called ___.
Mole
Avogadro's Number
Heap
Pile
The difference between the mass of one atom of an element is specified by ___.
atm
mol
a.m.u
grams
Exponential notation is represented as the ___ of two numbers N×10^x.
Sum
Product
Cross multiply
None of these
To reduce a number up to desired significant figures and adjust the last reported digit is known as ___.
Significant numbers
Rounded off data
Rounded off numbers
None of these
The maximum amount of product obtained by a balanced chemical reaction by using its Limiting reactant is known as ___.
Practical yield
Theoretical yield
Actual yield
None of these
The mass in grams of one mole of any pure substance is known as ___.
Atomic mass
Molar mass
Molecular mass
Molar volume
The digits in a number which show reliability in measurement are known as ___.
Significant numbers
Rounded off data
Rounded off numbers
None of these
____ is one of the two crystalline forms of carbon which is a constituent component of lead pencils.
Fullerene
Graphite
Diamond
All of these
___ is the SI unit used for measuring the amount of substance of specific number of particles.
Mole
Avogadro's Number
Heap
Pile
The reactant that is not completely consumes is often called ___.
Excess reactant
Excess agent
Excess reagent
Excess product
If we need to convert moles into number of particles or vice versa, ___ is used as converting factor.
Molar mass
Molar volume
Molecular mass
Avogadro's number
It can be determined by dividing molar mass with ___.
Mole
Molar volume
Molecular mass
Mass density
Molar volume of all ideal gases at STP is ___.
22.3 dm3
22.4 dm
22.4 dm2
22.4 dm3
The numerical value of Avogadro's number is ___.
6.02×10^23
6.02×10^24
6.02×10^25
6.02×10^26
This difference between theoretical and practical yield is due to ___.
The reactants may form any side product.
Either some amount of reactant may not react.
There may occur reversible reaction.
All of them
The reactant which is entirely consumed first during chemical reaction is called ___.
Limiting reaction
Limiting product
Limiting reagent
Limiting agent
The mass of oxygen in 9.8 grams of sulphuric acid is.
1.6g
3.2g
8g
6.4g
The volume of one mole of a gas at standard temperature (273K) and pressure (1 atm) is referred as ___.
Molar mass
Molar volume
Molecular mass
Avogadro's number
The mass of 3.25 moles of water H2O is ___.
57.5 gm
58.5 gm
50 gm
3.25 gm
No. of moles =?
Given mass (g) / Molar mass of substance
Given no. of atoms / Molar mass of substance
Given mass (g) /Atomic mass of substance
No. of particles of the substance / Avogadro's number
A ___ is defined as gram atomic mass of any substance (atoms, molecules, ions) which contains 6.02×10^23 particles.
Heap
Avogadro's Number
Mole
Pile
To solve the difficulty chemists have devised a unit called ___ as a convenient way to count the number particles in chemical substance by weighing them.
Mole
Avogadro's Number
Heap
Pile
On ___ solid ammonium nitrate NH4NO3, it decomposes to produce nitrous oxide N2O.
Melting
Cooling
Heating
None of these
Generally actual yield is:
Greater than theoretical yield
Less than theoretical yield
Equal to theoretical yield
Sometimes greater and sometimes less than theoretical yield
The no. of moles in 25.5g of sodium metal are ___.
1.01 moles
1.12 moles
0.11 moles
1.11 moles
Maximum numbers of molecules present in the following sample of gas.
100g O2
100g CH4
100g CO2
100g Cl2
Percentage yield = ??×100.
Theoretical yield / Percentage yield
Practical yield / Theoretical yield
1000 / Theoretical yield
None of these
C2H4(g)+3O2(g)⟶ ?
2CO2(g)+2H2O(I)
2CO2(g)+2HO(I)
CO2(g)+H2O(I)
CO2(g)+2H2O(I)
The minimum number of moles are present in:
1 dm3 of methane gas STP
5 dm3 of helium gas at STP
10 dm3 of hydrogen gas at STP
22.4 dm3 of chlorine gas at STP
If the volume occupied by oxygen gas (O2) at STP is 44.8 dm3, the number of molecule of O2 in the vessels are:
24.08×10^23
12.04×10^23
6.02×10^23
3.01×10^23
Calculate the mass of 4.39×10^24 atoms of Gold (Au) when molar mass of gold is 197 g/mol.
18.756 gm
15.365 gm
14.765 gm
14.365 gm
No. of moles in 6.4g of SO^2:
0.1 moles
0.2 moles
0.2 moles
1 moles
No. of atoms in a 60g of carbon is:
3.01×10^23
3.01×10^24
6.02×10^23
6.02×10^24
Volume in cm3 of 34.8g O2 gas at STP:
26789 cm3
26880 cm3
27780 cm3
23478 cm3
The number of carbon atoms on 1 mole of sugar C12H22O11 are approximately:
6×10^23
24×10^23
60×10^23
72×10^23
Calculate the number of moles in 2.35×10^25 atoms of Aluminum (AI).
39 moles
40 moles
41 moles
42 moles
The no. of molecules in 610g of Benzoic acid C7H6O2 are ___.
30.1×10^23
30.7×10^23
31.1×10^23
32.1×10^20
Which of the following sample of substances contains the same number of atoms as that of 20g calcium?
16g S
20g C
19g K
24g Mg
Number of formula units in 333g of CaCl2 are:
18.06×10^24
18.06×10^23
18.06×10^25
18.06×10^26
Which of the following statements is incorrect?
The mass of 1 mole Cl2 gas is 35.5 g
One mole of H2 gas contains 6.02×1023 of H2 molecules
Number of atoms in 23g Na and 24g Mg are equal
One mole of O2 at S.T.P occupies 22.4 dm3 volume
