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Chemistry Unit 1 Test

Total questions: 40

Worksheet time: 40mins

Name
Class
Date
1.

Empirical formula is the simplest atomic ratio of atoms in a molecule. Which compound does not have empirical formula CH2O

a)

Acetic acid

b)

Glucose

c)

Methanol

d)

Methyl methanoate

2.

At STP a gas which has maximum volume

a)

2g of O2 

b)

24g of CH4

c)

4g of He

d)

4g of H2

3.

Combustion analysis cannot determine empirical formula of

a)

Glucose

b)

Amino acid

c)

Acetylene

d)

Ethanol

4.

The number of carbon atoms in 45g of C6H12O6

a)

6 × NA

b)

1.50 × NA

c)

3 × NA

d)

0.25 × NA

5.

Volume of nitric oxide gas produced by the following reaction of 14g N2 with excess of oxygen is

a)

22.4dm3

b)

11.2dm3

c)

5.6dm3

d)

48.8dm3

6.

What is the mass of CaCO3 which on heating produces 0.5 moles of CO2 gas

a)

12.5g

b)

25g

c)

50g

d)

100g

7.

Select the suitable term about 17g of OH–

a)

1g atom

b)

1g formula

c)

1g ion

d)

1g molecule

8.

When 2g H2 gas and 16g O2 gas react completely to produce H2O. What is non- limiting reactant

a)

Hydrogen

b)

Oxygen

c)

Water

d)

Both are consumed completely

9.

A sample of liquid consisting of carbon, hydrogen and oxygen was subjected to combustion analysis, 24g of compound gave 22g of CO2. What is %age of carbon

a)

12.5%

b)

50%

c)

25%

d)

99%

10.

1gram atom of carbon is present in one mole of which of the following specie/substance

a)

CaCO3

b)

CH3CHO

c)

CH3COOH

d)

CaC2

11.

A man drinks 250cm3 water in a glass containing 18gram glucose(C6H12O6) the minimum number of atoms received by him are of

a)

Hydrogen

b)

Carbon

c)

Oxygen

d)

All are equal

12.

Number of grams of NaOH required for complete neutralization of 1mole of H2SO4 on its complete ionization

a)

0g

b)

80g

c)

100g

d)

40g

13.

H2O, HF and Na+ have same

a)

Mass number

b)

Number of electrons

c)

Number of protons

d)

Number of neutrons

14.

Mass of Al in 51g of Al2O3

a)

7g

b)

54g

c)

24g

d)

13.5g

15.

Mass of one magnesium atom is

a)

3.98x10-23g

b)

24g/NA

c)

24amu

d)

All of these

16.

How many moles of NH3 are produced on reacting 3 moles of N2 with 10 moles of H2

a)

8 moles

b)

2 moles

c)

4moles

d)

6 moles

17.

Relationship between empirical and molecular formula is M.F = n(E.F). For which compound value of n=1

a)

C2H4O2

b)

C6H12O6

c)

CH3CH3

d)

C12H22O11

18.

Mole of SO3 if it contains 16g of oxygen

a)

1/2

b)

1/3

c)

1/4

d)

1/8

19.

The atomic mass, formula mass and molecular mass of a substance expressed in grams is called mole. Which one of the following statements is incorrect about mole?

a)

1 mol of N=14 g

b)

1 mol of NH3=17 g

c)

1 mol of NaCl=1 mol of ions

d)

1 mol of O2=32 g

20.

A flask contains 224.6 cm3 of SO2 at STP. The flask contains amount of SO2 :

a)

0.54 g

b)

0.64 g

c)

0.32 g

d)

0.65g

21.

It is not correct regarding 22.0 g of N2 O :

a)

It occupies 11.2dm3 volume of gas at STP

b)

It contains atom of oxygen

c)

It contains 1 mole of nitrogen

d)

It contains lg molecule of N2 O

22.

A 0.5 mole of magnesium burns with excess oxygen. How much MgO is formed?

a)

40g

b)

20 g

c)

30g

d)

15 g

23.

Methane reacts with steam to form  and  as shown in fig,

What volume of H2 can be obtained from 100cm3 of methane at STP?

a)

300cm3

b)

200cm3

c)

100cm3

d)

150cm3

24.

Natural gas consists of primarily methane (CH4 ). The complete combustion of methane (CH4 ) gives carbon dioxide (CO2 ) and water.

When 2 moles of CH4 and 1 mole of O2 are allowed to combine? How many grams of excess reagent are left unreacted after the completion of reaction?

a)

20g

b)

24g

c)

22g

d)

26g

25.

1 a.m.u. is approximately equal to

a)

Mass of proton

b)

1.661x10-24g

c)

Reciprocal of NA

d)

All of these

26.

0.25 moles of phosphoric acid produces moles of H+ ions when it is 100% ionized

a)

0.25 moles

b)

0.75 moles

c)

1.5 moles

d)

0.5 moles

27.

Mass of one mole of heavy water is

a)

2

b)

20

c)

12

d)

18

28.

According to equation

4NH3 + 5O2 ⟶ 4NO + 6H2O

When 1mole of NH3 and 1 mol of O2 react then

a)

1 mole of H2 O is produced

b)

All oxygen is consumed

c)

1.5 mole of NO is formed

d)

All NH3 is consumed

29.

How many moles of oxygen (O2) are required for complete combustion of two moles of propane (C3 H8 )?

a)

2

b)

4

c)

10

d)

6

30.

The term gram atom can be used for

a)

16 g of O2

b)

96 g of SO4-2

c)

58.5 g of NaCl

d)

4 g of He

31.

Total number of atoms present in 49.0 g H3PO4 are (Ar H = 1, P = 31, O = 16):

a)

4 NA atoms

b)

It contains 1g molecules of H3PO4

c)

2 Na atoms

d)

It contains 0.6g atoms of H3PO4

32.

The mass of one mole of electrons is (1NA = 6.0 × 1023 )

a)

5.50×10-4g

b)

1.84×102 g

c)

1.008×103 g

d)

1.673×103 g

33.

For a reaction A+2B⟶C The amount of C formed by starting the reaction with 3 moles of A and 4 moles of B :

a)

2 moles

b)

4 moles

c)

4 moles

d)

5 moles

34.

One mole of propane has the same:

a)

Number of H-atoms as one mole of methane (CH4)

b)

Number of C-atoms as in one mole of butane (C4 H10)

c)

Mass as half a mole of hexane (C6 H14)

d)

Number of molecules as in one mole of ethane (C2 H6 )

35.

Which of the following is not true for a mole?

a)

It is a counting unit

b)

It contains 6.023×1023 particles

c)

It contains different number of particles for different substances

d)

It is the gram atomic or gram formula mass of a substance

36.

How many molecules of NH3 would be formed if 5.6dm3 of N2 gas react with excess of H2 according to following equation

N2 + 3H2 → 2NH3

a)

1.505 x1023

b)

3.01 x 1023

c)

6.02 x 1023

d)

2.4 x1024

37.

Which of followings contains the maximum number of atoms

a)

1g of oxygen atom

b)

1g of ozone

c)

1g of oxygen gas

d)

All contain same number of atoms

38.

Mass of 1.505 x 1023 molecules of NH3 is

a)

17g

b)

8.5g

c)

34g

d)

4.25g

39.

1g pf unknown gas has volume of 11.2dm3 at STP. Unknown gas is

a)

CO2

b)

CH4

c)

HCI

d)

H2

40.

18.02g of H2O sample has

a)

0.2 NA H-atoms

b)

0.1 NA O-atoms

c)

6.02 x 1023 moles of H2O

d)

6.02 x 1023 molecules of H2O

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