60 ml of a mixture of nitrous oxide N 2 O and nitric oxide ( NO ) was exploded with excess of hydrogen. If 38 ml of N 2 was formed, calculate the volume of each gas in the mixture.

Both nitrous oxide and nitric oxide react with hydrogen to produce hydrogen gas and water vapour. The reactions can be represented as, 2 NO + 2 H 2 → N 2 + 2 H 2 O N 2 O + H 2 → N 2 + H 2 O Suppose the volume of NO in the mixture is ' 2 x ' ml and N 2 O is ' 60 - 2 x ' ml . 2 NO + 2 H 2 → N 2 + 2 x x 2 H 2 O N 2 O + H 2 → N 2 + H 2 O 60 - 2 x 60 - 2 x Total volume of N 2 formed = 60 - 2 x + x According to the question, 60 - 2 x + x = 38 x = 22 ml Hence, volume of NO in the mixture = 2 × 22 = 44 ml , and volume of N 2 O in the mixture = 60 - 44 = 16 ml .

A sample of gaseous hydrocarbon occupying 1 . 12 litre at NTP , completely burnt in air and produced 2 . 2 g of CO 2 and 1 . 8 g H 2 O . Calculate the mass of compound taken and volume of O 2 at NTP required for its burning. Also calculate molecular formula of hydrocarbon.

1 . 12 litre of hydrocarbon occupies mole = 1 . 12 22 . 4 = 0 . 05 Mole of CO 2 formed = 2 . 2 44 = 0 . 05 Mole of H 2 O formed = 1 . 8 18 = 0 . 10 Let the hydrocarbon be C a H b C a H b + a + b 4 O 2 ⟶ aCO 2 + b 2 H 2 O ∴ 1 mole of C a H b gives = a mole CO 2 ∴ 0 . 05 mole of C a H b will give = 0 . 05 a mole of CO 2 ∴ 0 . 05 a = 0 . 05 ∴ a = 1 ∴ 1 mole of C a H b gives = b 2 mole H 2 O ∴ 0 . 05 mole of C a H b will give = 0 . 05 × b 2 mole H 2 O = 0 . 05 × b 2 = 0 . 10 ∴ b = 4 ∴ Hydrocarbon is CH 4 . ∴ Mass of 1 . 12 litre CH 4 at STP = 16 × 1 . 12 22 . 4 = 0 . 8 g Also, CH 4 + 2 O 2 ⟶ CO 2 + 2 H 2 O mole CH 4 requires = 2 × 32 gO 2 ∴ 0 . 05 mole CH 4 requires = 2 × 32 × 0 . 05 = 3 . 2 gO 2 = 2 . 24 litre O 2

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Earn 100

A mixture of ${NO}_{2}$ and $CO$ having total volume of $100 ml$ contains $70 ml$ of ${NO}_{2}$ at $1 atm$ , mixture is left for sometime and some ${NO}_{2}$ get dimerised to $N_{2} O_{4}$ such that final volume of the mixture become $80 ml$ at $1 atm$ . Calculate mole fraction of ${NO}_{2}$ in final equilibrium mixture.

Important Questions on Some Basic Concepts of Chemistry

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 1 - Some Basic Concepts of Chemistry>Exercise-1>Q 62

One litre of oxygen gas is passed through an ozonizer and the final volume of the mixture becomes

820 mL

if this mixture is passed through oil of turpentine. Find the final volume of gas remaining.

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 1 - Some Basic Concepts of Chemistry>Exercise-1>Q 63

Identify the molecular weight of the compound '

X

' containing carbon and hydrogen atoms only with

3 σ

and

2 π

bonds in one molecule.

HARD

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Alpha Question Bank for Engineering: Chemistry>Chapter 1 - Some Basic Concepts of Chemistry>Exercise-1>Q 65

40 m L

of ammonia gas taken in an eudiometer tube was subjected to sparks till the volume did not change any further. The volume was found to increase by

40 m L, 40 m l

of oxygen was then mixed and the mixture was further exploded. The gases remained were

30 m L

Deduce the formula of ammonia.

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Alpha Question Bank for Engineering: Chemistry>Chapter 1 - Some Basic Concepts of Chemistry>Exercise-1>Q 67

60 ml

of a mixture of nitrous oxide

(N_{2} O)

and nitric oxide

(NO)

was exploded with excess of hydrogen. If

38 ml

N_{2}

was formed, calculate the volume of each gas in the mixture.

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Alpha Question Bank for Engineering: Chemistry>Chapter 1 - Some Basic Concepts of Chemistry>Exercise-1>Q 69

A sample of gaseous hydrocarbon occupying

1.12

litre at

NTP

, completely burnt in air and produced

2.2 g

{CO}_{2}

and

1.8 g H_{2} O

. Calculate the mass of compound taken and volume of

O_{2}

NTP

required for its burning. Also calculate molecular formula of hydrocarbon.

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Alpha Question Bank for Engineering: Chemistry>Chapter 1 - Some Basic Concepts of Chemistry>Exercise-1>Q 70

The volume of

{CO}_{2}

produced by the combustion of

40 mL

of gaseous acetone in excess of oxygen is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 1 - Some Basic Concepts of Chemistry>Exercise-1>Q 71

500 ml of a hydrocarbon gas burnt in excess of oxygen yields 2500 ml of

C O_{2}

and 3 litres of water vapour, all the volumes being measured at the same temperature and pressure. The formula of hydrocarbon is

HARD

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Alpha Question Bank for Engineering: Chemistry>Chapter 1 - Some Basic Concepts of Chemistry>Exercise-1>Q 73

$7.5 ml$ of a gaseous hydrocarbon was exploded with $36 ml$ of oxygen. The volume of gases on cooling was found to be $28.5 ml, 15 ml$ of which was absorbed by $KOH$ and the rest was absorbed in a solution of alkaline Pyrogallol. If all volumes are measured under same conditions, the formula of hydrocarbon is-

A mixture of NO2 and CO having total volume of 100 ml contains 70 ml of NO2 at 1 atm, mixture is left for sometime and some NO2 get dimerised to N2O4 such that final volume of the mixture become 80 ml at 1 atm. Calculate mole fraction of NO2 in final equilibrium mixture.

Important Questions on Some Basic Concepts of Chemistry

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