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Chemistry Part-I

States of Matter

What will be the pressure of the gaseous mixture when 0.5 L of

Chemistry Part-I

Class 11

NCERT

Chapter 1: Some Basic Concepts of Chemistry

44 questions

Chapter 2: Structure of Atom

85 questions

Chapter 3: Classification of Elements and Periodicity in Properties

50 questions

Chapter 4: Chemical Bonding and Molecular Structure

44 questions

Chapter 5: States of Matter

28 questions

What will be the pressure exerted by a mixture of

3.2 g

of methane and

4.4 g

C O_{2}

contained in a

9 d m^{3}

flask at

27 C

What will be the pressure of the gaseous mixture when 0.5 L of H

_{2}

at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27

^{\circ} C

Density of a gas is found to be 5.46 dm

^{3}

at 27

^{\circ} C

at 2 bar pressure. What will be its density at STP?

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Chapter 6: Thermodynamics and Thermochemistry

36 questions

Chapter 7: Equilibrium

101 questions

Question

Medium

Solving time: 4 mins

What will be the pressure of the gaseous mixture when 0.5 L of H $_{2}$ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27 $^{\circ} C$ ?

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Updated on: Mar 27, 2023

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Chemistry Part-I (NCERT)

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Henry Discussed

What will be the pressure of the gaseous mixture when 0.5 L of H

_{2}

at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27

^{\circ} C

11 mins ago

Discuss this question LIVE

11 mins ago

Text solutionVerified

(i) The partial pressure of hydrogen gas

P^{'} = \frac{P V}{V ^{'}} = \frac{0.8 \times 0.5}{1} = 0.40

bar

(ii) The partial pressure of oxygen gas

P^{''} = \frac{P V}{V ^{'}} = \frac{0.7 \times 2.0}{1} = 1.40

bar

So, the total pressure of gaseous mixture is

P + P^{''} = 0.40 + 1.40 = 1.80

bar

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Practice more questions from Chemistry Part-I (NCERT)

What will be the pressure exerted by a mixture of

3.2 g

of methane and

4.4 g

C O_{2}

contained in a

9 d m^{3}

flask at

27 C

What will be the pressure of the gaseous mixture when 0.5 L of H

_{2}

at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27

^{\circ} C

Density of a gas is found to be 5.46 dm

^{3}

at 27

^{\circ} C

at 2 bar pressure. What will be its density at STP?

View all

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Question Text	What will be the pressure of the gaseous mixture when 0.5 L of H $_{2}$ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27 $^{\circ} C$ ?
Updated On	Mar 27, 2023
Topic	States of Matter
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 3
Upvotes	399
Avg. Video Duration	5 min

What will be the pressure of the gaseous mixture when 0.5 L of H $_{2}$ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27 $^{\circ} C$ ?

Text solutionVerified

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What will be the pressure of the gaseous mixture when 0.5 L of H $_{2}$ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27 $^{\circ} C$ ?