An ideal gas at 27^(@)C is compressed ad...

An ideal gas at `27^(@)C` is compressed adiabatically to `(8)/(27)` of its original volume. The rise in temperature is `(gamma = (5)/(3))`

A

275 K

B

375 K

C

475K

D

175K

Text Solution

Verified by Experts

The correct Answer is:

B

Topper's Solved these Questions

THERMODYNAMICS
AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT (SECTION -D) (Assertion - Reason Type Questions)|10 Videos
THERMODYNAMICS
AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT (SECTION -B) (Objective Type Questions)|30 Videos
THERMAL PROPERTIES OF MATTER
AAKASH INSTITUTE ENGLISH|Exercise Assignment (Section-J) Akash Challengers Questions|7 Videos
UNITS AND MEASUREMENTS
AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT (SECTION - D)|15 Videos

Similar Questions

Explore conceptually related problems

An ideal gas at 27^(@)C is compressed adiabatically to 8//27 of its original volume. If gamma = 5//3 , then the rise in temperature is

The volume of a given mass of gas at NTP is compressed adiabatically to 1/5th of its original volume. What is the new pressure ? gamma =1.4.

A diatomic gas initially at 18^(@) is compressed adiabatically to one- eighth of its original volume. The temperature after compression will b

A diatomic ideal gas is compressed adiabatically to 1/32 of its initial volume. If the initial temperature of the gas is T_i (in Kelvin) and the final temperature is a T_i , the value of a is

A diatomic ideal gas is compressed adiabatically to 1/32 of its initial volume. If the initial temperature of the gas is T_i (in Kelvin) and the final temperature is aT_i , the value of a is

A monatomic gas initially at 17^@ C has suddenly compressed adiabatically to one-eighth of its original volume. The temperature after compression is

An ideal gas at a pressure of 1 atm and temperature of 27^(@)C is compressed adiabatically until its pressure becomes 8 times the initial pressure , then final temperature is (gamma=(3)/(2))

A monoatomic gas at pressure P_(1) and volume V_(1) is compressed adiabatically to 1/8th of its original volume. What is the final pressure of gas.

A monoatomic gas is compressed adiabatically to (1)/(4)^(th) of its original volume , the final pressure of gas in terms of initial pressure P is

AAKASH INSTITUTE ENGLISH-THERMODYNAMICS-ASSIGNMENT (SECTION -C) (Previous Year Questions)

The efficiency of a Carnot engine operating between temperatures of 10...
Text Solution
|
We consider a thermodynamic system. If Delta U respresents the increas...
Text Solution
|
If the ratio of specific heat of a gas at constant pressure to that at...
Text Solution
|
An ideal gas at 27^(@)C is compressed adiabatically to (8)/(27) of its...
Text Solution
|
Two ideal Carnot engines operate in casade (all heat given up by one e...
Text Solution
|
The (W/Q) for a Carnot engine is 1/6. Now the temperature of sink is r...
Text Solution
|
The temperature of source and sink of a heat engine are 127^(@)C and 2...
Text Solution
|
The efficiency of carnot engine is 50% and temperature of sink is 500K...
Text Solution
|
An ideal gas heat engine operates in a Carnot cycle between 27^(@)C an...
Text Solution
|
One mole of an ideal gas at an initial temperature of T K does 6 R jou...
Text Solution
|
The amount of heat energy required to raise the temperature of 1 g of ...
Text Solution
|
Which of the following relations does not give the equation of an adia...
Text Solution
|
According to C.E van der Waal, the interatomic potential varies with t...
Text Solution
|
A gas at pressure p(0) is contained in a vessel. If the masses of all ...
Text Solution
|
The mean free path of collision of gas melecules varies with its diame...
Text Solution
|
At 0 K, which of the following properties of a gas will be zero ?
Text Solution
|
The units of constant b used in van der Waals' equation are ………….. .
Text Solution
|
The degrees of freedom of a triatomic gas is
Text Solution
|
To find out degree of freedom, the correct expression is:
Text Solution
|
The equation of state for 5 g of oxygen at a pressure P and temperatur...
Text Solution
|