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Chemistry Part-I

States of Matter

A mixture of dihydrogen and dioxygen at one bar pressure conta

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

2.9

g of gas at

95^{\circ} C

occupied the same volume as 0.184 g of dihydrogen at

17^{\circ} C

at the same pressure. What is the molar mass of the gas?

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

In terms of Charles' law, explain why - 273

^{\circ} C

is the lowest possible temperature.

View all question

Chapter 6: Thermodynamics and Thermochemistry

36 questions

Chapter 7: Equilibrium

101 questions

Question

Easy

Solving time: 2 mins

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

Name: Video solution 1: [Solved] A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen. - Chemistry Part-I
Uploaded: 2023-02-21T18:15:44.000Z
Duration: 4 min
Description: Video solution 1: [Solved] A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen. - Chemistry Part-I

Views: 6,372 students

Updated on: Feb 21, 2023

Book:

Chemistry Part-I (NCERT)

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A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

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Text solutionVerified

In 100 g of mixture, the mass of hydrogen and oxygen will be 20 and 80 g respectively.
The number of moles of hydrogen are

n = \frac{20}{2} = 10

.
The number of moles of oxygen are

n^{'} = \frac{80}{32} = 2.5

.
The mole fraction of hydrogen is

\frac{10}{10 + 2.5} = 0.8

.
Partial pressure of hydrogen is

0.8 x P = 0.8 x 1 = 0.8

bar

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Practice more questions from Chemistry Part-I (NCERT)

2.9

g of gas at

95^{\circ} C

occupied the same volume as 0.184 g of dihydrogen at

17^{\circ} C

at the same pressure. What is the molar mass of the gas?

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

In terms of Charles' law, explain why - 273

^{\circ} C

is the lowest possible temperature.

View all

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Question Text	A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.
Updated On	Feb 21, 2023
Topic	States of Matter
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 2
Upvotes	236
Avg. Video Duration	5 min

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

Text solutionVerified

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A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

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