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11th Chemistry Monthly Test - 2 ( Basic Concepts of Chemistry and Chemical Calculations )

MABS Institution

11th Chemistry Monthly Test - 2 ( Basic Concepts of Chemistry and Chemical Calculations )-Aug 2020

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

40 ml of methane is completely burnt using 80 ml of oxygen at room temperature The volume of gas left. after cooling to room temperature is

40 ml CO₂ gas
40 ml CO₂ gas and 80 ml H₂O gas
60 ml CO₂ gas and 60 ml H₂O gas
120 ml CO₂ gas

The oxidation state of a element in its uncombined state is

zero
+1
-1
none

A compound has an empirical formula C₂H₄O. If the value of n = 2 the molecular formula of the compound is___________

C₂H₄O
CH₂O
CH₂
C₄H₈O₂

Identify the incorrect statement about a compound.

A molecule cannot be separated into its constituent elements by physical methods of separation
A molecule of a compound has atoms of different elements
A compound retains the physical properties of its constituent element
The ratio of atoms of different elements in a compound is fixed

If Avogadro number were changed from 6.022 x 10²³to 6.022 x 10²⁰, this would change

the ratio of chemical species to each other in a balanced equation
the ratio of elements to each other in a compound
the definition of mass in units of grams
the mass of one mole of carbon

The solid state of matter is converted into gas by

sublimation
deposition
freezing
condensation

Which of the following contain same number of carbon atoms as in 6 g of carbon-12.

7.5 g ethane
8 g methane
both (a) and (b)
none of these

The number of water molecules in a drop of water weighing 0.018 g is

6.022 x 10²⁶
6.022 x10²³
6.022 x 10²⁰
9.9 x 10²²

Which one of the following represents 180g of water?

5 Moles of water
90 moles of water
\(\frac { 6.022\times { 10 }^{ 23 } }{ 180 } \) molecules of water
6.022 x 10²⁴molecules of water

Match the list I with List II and select the correct answer using. the code given below the lists.

List I List II

A Diamond 1 Heterogeneous mixture

B Aerated drinks 2 Element

C Distilled water 3 Homogeneous mixture

D Sand 4 Compound

A B C D

2 3 4 1
A B C D

4 3 1 2
A B C D

3 1 4 2
A B C D

2 1 4 3

Part - B

Generic 2 - Answer All Question

Which contains the greatest number of moles of oxygen atoms
i) 1 mol of ethanol
ii) 1 mol of formic acid
iii) 1 mol of H₂O

Balance the following equations by ion electron method \({ Na }_{ 2 }{ S }_{ 2 }{ O }_{ 3 }+{ I }_{ 2 }\longrightarrow { Na }_{ 2 }{ S }_{ 4 }{ O }_{ 6 }+NaI\)

Define relative atomic mass.

Balance the following equations by ion electron method - \({ C }_{ 2 }{ O }_{ 4 }^{ 2- }+{ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }\longrightarrow { Cr }^{ 3+ }+{ CO }_{ 2 }\) (in acid medium)

Calculate the average atomic mass of naturally occurring magnesium using the following data

Isotope Istopic atomic mass Abundance(%)

Mg²⁴ 23.99 78.99

Mg²⁶ 24.99 10.00

Mg²⁵ 25.98 11.01

Distinguish between oxidation and reduction.

What do you understand by the term mole.

Part - C

Generic 3 - Answer All Question

Find the molecular mass of FeSO₄7H₂O.

What will be the molecular formula for the compound, whose empirical formula is CH₂CI and molar mass is 98.96 g?

The percentage of all the elements present o in a compound is 95. What does it indicate?

Balance the following reaction:
C₂O₄²-+Cr₂O₇^2-\(\rightarrow \)Cr³⁺+CO₂

Calculate the empirical and molecular formula of a compound containing 76.6% carbon, 6.38 % hydrogen and rest oxygen its vapour density is 47

How much mass (in gram units) is represented by the following?
0.2 mol of NH₃

Calculate the molar volume of the following 460g of formic acid

Part - D

Generic 5 - Answer All Question

A Compound on analysis gave Na = 14.31% S = 9.97% H= 6.22% and 0= 69.5% calculate the molecular formula of the compound if all the hydrogen in the compound is present in combination with oxygen as a water of crystallization. (molecular mass of the compound is 322).

The reaction between aluminum and ferric oxide can generate temperatures up to 3273 K and is used in welding metals. (Atomic mass of AC = 27 u atomic mass of O = 16 u )
2Al + Fe₂O₃ \(\longrightarrow \) Al₂O₃ + 2Fe; If in this process, 324 g of aluminum is allowed to react with 1.12 kg of ferric oxide
i) Calculate the mass of Al₂O₃ formed
ii) How much of the excess reagent is left at the end of the reaction?

Arrange the elements silver, Zinc and copper in the order of their decreasing electron releasing tendency and justify your arrangement with an appropriate experiment.

Calculate the molar mass of the following compounds. -
i) urea [CO(NH₂)₂]
ii) acetone [CH₃ COCH₃]
iii) boric Acid [H₃BO₃]
iv) Sulphurci Acid [H₂SO₄]
Explain displacement reaction.

Write note on decomposition reaction

Balance the following equations by oxidation number method
i) \({ K }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 }+KI+{ H }_{ 2 }SO_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ Cr }_{ 2 }({ SO }_{ 4 })+{ I }_{ 2 }+{ H }_{ 2 }O\)
ii) \({ K }Mno_{ 4 }+{ Na }_{ 2 }{ So }_{ 3 }\longrightarrow { MnO }_{ 2 }+{ Na }_{ 2 }{ So }_{ 4 }+KOH\)
iii) \(Cu+{ HNO }_{ 3 }\longrightarrow Cu\left( { NO }_{ 3 } \right) _{ 2 }+{ NO }_{ 2 }+{ H }_{ 2 }O\)
iv) \({ KMn }O_{ 4 }+{ H }_{ 2 }{ C }_{ 2 }{ O }_{ 4 }+{ H }_{ 2 }{ SO }_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ MnSO }_{ 4 }+{ CO }_{ 2 }+{ H }_{ 2 }O\)

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