Boyle's Law
Trending Questions
The pressure exerted by an ideal gas molecule is given by the expression
In an adiabatic process, the density of a diatomic gas becomes 32 times its initial value. The final pressure of the gas is found to be n times the initial pressure. The value of n is:
32
326
128
A vessel of 120 mL capacity contains a certain amount of gas at 35∘C and 1.2 bar pressure.
The gas is transferred to another vessel of volume 180 mL at 35∘C. What would be its pressure?
What is the full form of the atm in terms of chemistry?
- 5%
- 5.26%
- 10%
- 4.26%
- The pressure of gas decreases
- The kinetic energy of the gas moleules remains the same
- The kinetic energy of the gas molecules decreases
- The number of molecules of the gas increases
What gas law apply in space?
- 9100
- 1009
- 10
- 110
A closed vessel contains mole of a monoatomic ideal gas at . If mole of the same gas at is added to it, the final equilibrium temperature of the gas in the vessel will be close to _______.
What is KMT and what are its assumptions?
(The density of the lake and mercury are 1 g/ml and 13.6 g/ml respectively. Ignore the surface tension)
- 651 m
- 453 m
- 784m
- 102 m
please give explanation with answer
Differentiate between liquid pressure and atmospheric pressure.
- 202.50 mm of Hg
- 217.40 mm of Hg
- 115.50 mm of Hg
- 150.40 mm of Hg
The graph for Boyles law is called
Isotherm
Hypertherm
Hypotherm
None of these
Why cant temperature go below absolute zero?
- 1 atm
- 2 atm
- 1 torr
- 4 atm
The density of neon is highest at
STP
- 125 mmHg
- 150 mmHg
- 410 mmHg
- 205 mmHg
When a gas is compressed keeping the temperature constant it results in
If the line is normal to the curve , then:
Data is insufficient
Given: Patm=76 cm of Hg
- 10.52 cm
- 9.50 cm
- 4.61 cm
- 3.53 cm
The compressibility factor of a gas is defined as Z=PV/RT. The compressibility factor of ideal gas is
0
Infinity
1
-1
- P0=h(l1+l2)l1−l2 cm of Hg
- P0=h(l1+l2)l2−l1 cm of Hg
- P0=h(l1−l2)l1+l2 cm of Hg
- P0=76 cm of Hg
- 10
- 15
- 50
- 25