IIT JAM Exam  >  IIT JAM Questions  >  The density of a mixture of O2 and N2 at NTP ... Start Learning for Free
The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm?
Verified Answer
The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is ...
Let 1 mole of the gas is present. So, 22.4 L will be the volume of the mixture.
Density(ρ) =Mass(m)Volume(V)Density(ρ) =Mass(m)Volume(V)
So, the molar mass of the mixture = mass(m) = density x volume =1.3 x 22.4 =29.12 g/molmass(m) = density x volume =1.3 x 22.4 =29.12 g/mol
Let percentage of oxygen present in the mixture = x 
So, the percentage of nitrogen will be =1-x
Molar mass of oxygen =32 g mol-1
Molar mass of nitrogen =28 g mol-1
So, 32(x) +28(1-x) = 29.12
32x-28x=29.12-28
4x=1.12
x=0.28
So, partial pressure exerted by oxygen =0.28 atm
 
This question is part of UPSC exam. View all IIT JAM courses
Most Upvoted Answer
The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is ...
Density of the mixture:
The given density of the mixture of O2 and N2 at NTP (Normal Temperature and Pressure) is 1.3 g litre⁻¹.

Partial pressure of N2:
We need to find the partial pressure of N2 in the mixture.

Explanation:
To determine the partial pressure of N2, we need to consider the ideal gas law. The ideal gas law equation is as follows:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

Step 1: Calculate the number of moles:
The number of moles of a substance can be calculated using the equation:

n = mass / molar mass

Given the density of the mixture is 1.3 g litre⁻¹, we can convert it to kg m⁻³ by dividing by 1000 and multiplying by 1000 (since 1 L = 1000 cm³).

Density = mass / volume
1.3 g litre⁻¹ = mass / (1 L)
mass = 1.3 g

To convert grams to kilograms, we divide by 1000:
mass = 1.3 g / 1000 = 0.0013 kg

Now, we need to calculate the number of moles using the molar mass of the mixture. The molar mass of the mixture can be obtained by considering the molar mass of O2 and N2 and their respective mole fractions.

Assuming the mole fraction of N2 is x, the mole fraction of O2 would be (1 - x).

Molar mass of N2 = 28 g/mol
Molar mass of O2 = 32 g/mol

Molar mass of the mixture = (x * 28) + ((1 - x) * 32)

Now, using the given density of the mixture, we can calculate the number of moles:

density = mass / volume
density = (mass of mixture) / (volume of mixture)
1.3 g litre⁻¹ = (0.0013 kg) / (volume of mixture)

Step 2: Calculate the volume:
To calculate the volume of the mixture, we can use the ideal gas law equation.

PV = nRT

Rearranging the equation, we have:

V = (nRT) / P

Now we can substitute the values into the equation. The temperature at NTP is 273 K, and the ideal gas constant R is 0.0821 L atm K⁻¹ mol⁻¹.

V = [(mass of mixture) / (molar mass of mixture)] * (R * T) / P

Step 3: Calculate the partial pressure of N2:
To find the partial pressure of N2, we need to consider the mole fraction of N2 (x) in the mixture.

The mole fraction of N2 is given by:

x = (number of moles of N2) / (total number of moles)

The total number of moles can be calculated by dividing the mass of the mixture by the molar mass of the mixture.

Now we can substitute the values into the equation:

partial pressure of N2 = x * total pressure

Answer:
Community Answer
The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is ...
B
Explore Courses for IIT JAM exam
The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm?
Question Description
The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm?.
Solutions for The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm? in English & in Hindi are available as part of our courses for IIT JAM. Download more important topics, notes, lectures and mock test series for IIT JAM Exam by signing up for free.
Here you can find the meaning of The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm? defined & explained in the simplest way possible. Besides giving the explanation of The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm?, a detailed solution for The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm? has been provided alongside types of The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm? theory, EduRev gives you an ample number of questions to practice The density of a mixture of O2 and N2 at NTP is 1.3 g litre-¹.What is the partial pressure of N2. (a)1.725 atm (b)0.725 atm (c)0.593 atm (d)1.593 atm? tests, examples and also practice IIT JAM tests.
Explore Courses for IIT JAM exam
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
10M+ students study on EduRev