Ethane burns in oxygen to form C O 2 and H 2 O according to the equation, 2 C 2 H 6 + 7 O 2 → 4 C O 2 + 6 H 2 O If 1 250 c c of oxygen is burnt with 300 c c of ethane. Calculate the volume of C O 2 formed.

2 C 2 H 6 + 7 O 2 → 4 C O 2 + 6 H 2 O According to the above reaction where ethane burns in the presence of oxygen, 2 volumes of ethane reacts with oxygen to give 4 volumes of carbon dioxide. This means the volume of carbon dioxide formed is two times the volume of ethane. So the volume of carbon dioxide formed from 300 cc of ethane would be two times the amount of ethane = ( 300 × 2 ) cc Therefore, the amount of carbon dioxide formed from 300 cc of ethane is 600 cc .

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Ethylene oxide C₂H₄O is manufactured by burning of ethylene in air.
2C₂H₄ + O₂ → 2C₂H₄O. 60 g of ethylene oxide is obtained from 42 g of ethylene. Calculate the percentage yield.

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Important Questions on Some Basic Concepts of Chemistry

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

The amount of metallic

Zn

(Atomic weight

= 65.4

) required to react with aqueous sodium hydroxide to produce

1 g

H_{2}

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

In the following reaction:

$A + 2 B + 3 C ⇌ A B_{2} C_{3}$
$6.0 g$ of $A$ , $6.0 \times 10^{23}$ atoms of $B$ and $0.036 mol$ of $C$ reacted and formed $4.8 g$ of compound $A B_{2} C_{3}$ . If the atomic mass of $A$ and $C$ are $60$ and $80 amu$ , respectively. What is the atomic mass of $B$ in $amu$ ? (Avogadro number $= 6 \times 10^{23}$ )

EASY

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

What is the quantity of hydrogen gas liberated when

46 g

sodium reacts with excess ethanol? (Given Atomic mass of

Na = 23 g

)

EASY

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

LiOH

reacts with

{CO}_{2}

to form

{Li}_{2} {CO}_{3}

(atomic mass of

Li = 7

). The amount of

{CO}_{2}

(in g) consumed by

1 g

LiOH

is closest to

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

Galena (an ore) is partially oxidized by passing air through it at high temperature. After some time, the passage of air is stopped, but the heating is continued in a closed furnace such that the contents undergo self-reduction. The weight (in $kg$ ) of $Pb$ produced per $kg$ of $O_{2}$ consumed is ____. (Atomic weights in $g {mol}^{- 1} : O = 16, S = 32, Pb = 207$ )

Give the answer to the nearest integer value.

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

When 22.4 L of

C_{4} H_{8}

at STP is burnt completely, 89.6 L of

C O_{2}

gas at STP and 72 g of water are produced.
The volume of the oxygen gas at STP consumed in the reaction is closest to

EASY

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

1

gram of a carbonate

(M_{2} {CO}_{3})

on treatment with excess

HCl

produces

0.01186

moles of

{CO}_{2}

. The molar mass of

M_{2} {CO}_{3}

{gmol}^{- 1}

is:

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

The amount of arsenic pentasulphide that can be obtained when

35.5 g

arsenic acid is treated with excess

H_{2} S

in the presence of conc.

HCl

(assuming

100 %

conversion) is

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

The ammonia is prepared by treating ammonium sulphate with calcium hydroxide is completely used by ${NiCl}_{2} \cdot 6 H_{2} O$ to form a stable coordination compound. Assume that, both the reactions are $100 %$ completed. If $1584 g$ of ammonium sulphate and $952 g$ of ${NiCl}_{2} \cdot 6 H_{2} O$ are used in the preparation, the combined weight (in grams) of gypsum and the nickel ammonia coordination compound produced is ____.

Atomic weights in $g {mol}^{- 1}$ :

$H = 1; N = 14 O = 16; S = 32 Cl = 35 .5; Ca = 40 Ni = 59$

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

20.0 g of a magnesium carbonate sample decomposes on heating to give carbon dioxide and 8.0 g magnesium oxide. What will be the percentage purity of magnesium carbonate in the sample?

(Atomic weight: Mg = 24)

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

The molecular formula of a commercial resin used for exchanging ions in water softening is

C_{8} H_{7} S O_{3} N a

(molecular weight = 206)

. What would be the maximum uptake of

C a^{2 +}

ions by the resin if expressed in

mol

per

gm

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

A mixture of

100 m mol

Ca {(OH)}_{2}

and

2 g

of sodium sulphate was dissolved in water and the volume was made up to

100 mL .

What is the mass of calcium sulphate formed and the concentration of

{OH}^{-}

in resulting solution, respectively? (Molar mass of

Ca {(OH)}_{2}, {Na}_{2} {SO}_{4}

and

{CaSO}_{4}

are

74, 143

and

136 g {mol}^{- 1},

respectively;

K_{sp}

Ca {(OH)}_{2} is 5 .5 \times 10^{- 6}

)

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

Excess of

NaOH (aq)

was added to

100 mL

{FeCl}_{3} (aq)

resulting into

2.14 g

Fe {(OH)}_{3}

. The molarity of

{FeCl}_{3} (aq)

is:

(Given the molar mass of

Fe = 56 g

{mol}^{- 1}

and molar mass of

Cl = 35 .5 g {mol}^{- 1}

)

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

When 262 g of xenon (atomic mass = 131) reacted completely with 152 g of fluoride (atomic mass = 19), a mixture of

X e F_{2}

and

X e F_{6}

was produced. The molar ratio of

X e F_{2} : X e F_{6}

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

300 K

and

1 atm

15 mL

of a gaseous hydrocarbon requires

375 mL

air containing

20 % O_{2}

by volume, for complete combustion. After combustion, the gases occupy

345 mL

. Assuming that the water formed is in liquid form and the volumes were measured at the same temperature and pressure, the formula of the hydrocarbon is:
(Assume complete combustion of reactant)

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

Ethane burns in oxygen to form

{C O}_{2}

and

H_{2} O

according to the equation,

2 C_{2} H_{6} + 7 O_{2} \to 4 {C O}_{2} + 6 H_{2} O

1250 c c

of oxygen is burnt with

300 c c

of ethane. Calculate the volume of

{C O}_{2}

formed.

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

5 L

of an alkane requires

25 L

of oxygen for its complete combustion. If all volumes are measured at constant temperature and pressure, the alkane is

EASY

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

What is the mass of the precipitate formed when 50 mL of

16.9 %

solution of

A g N O_{3}

is mixed with 50 mL of

5.8 %

NaCl solution?

(Ag = 107.8, N = 14, O = 16, Na = 23, Cl = 35.5)

EASY

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

For the following reaction, the mass of water produced from

445 g

C_{57} H_{110} O_{6}

is:

2 C_{57} H_{110} O_{6} (s) + 163 O_{2} (g) \to 114 {CO}_{2} (g) + 110 H_{2} O (l)

MEDIUM

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Stoichiometry and Stoichiometric Calculations

A mixture of

2.3 g

formic acid and

4.5 g

oxalic acid is treated with concentrated

H_{2} {SO}_{4}

. The evolved gaseous mixture is passed through

KOH

pellets. What will be the weight in grams of the remaining product at

STP

Ethylene oxide C2H4O is manufactured by burning of ethylene in air. 2C2H4 + O2 → 2C2H4O. 60 g of ethylene oxide is obtained from 42 g of ethylene. Calculate the percentage yield.

Important Questions on Some Basic Concepts of Chemistry

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Ethylene oxide C₂H₄O is manufactured by burning of ethylene in air.
2C₂H₄ + O₂ → 2C₂H₄O. 60 g of ethylene oxide is obtained from 42 g of ethylene. Calculate the percentage yield.