The graph drawn between pressure and temperature at constant volume for a given mass of different molecular weights $$M_{1}$$ and $$M_{2}$$ are the straight lines as shown in the figure then
Explanation
Constant volume thermometer works on
At constant pressure, density of a gas is :
Hint: Density of a substance is given by $$\rho = \dfrac{m}{V}$$ , where $$m$$is the mass of the substance and $$V$$ is its volume.
Correction Option: B
Explanation for correct option:
$$ \Rightarrow PV \alpha nRT$$
$$ \Rightarrow PV = \dfrac{m}{M} RT$$, where $$m$$ and $$M$$ are weight and molecular weight of the gas.
$$ \Rightarrow P = \dfrac{m}{V}\dfrac{{RT}}{M}$$
Here, $$\rho = \dfrac{m}{V}$$ and $$R' = \dfrac{R}{M}$$, where $$R'$$ is the specific gas constant for the gas.
$$ \Rightarrow P = \rho R'T$$
$$ \Rightarrow \rho = \dfrac{P}{{R'T}}$$
$$\therefore \rho \alpha \dfrac{1}{T}$$
Hence, at constant pressure, density of a gas is inversely proportional to absolute temperature.
All gasses deviate from gas laws at
The temperature at which the volume of ideal gas is zero is:
Two identical tumblers are filled fully with water at a certain temperature. One of the tumblers is warmed up and the other cooled down. But it is observed that the water overflows from both the tumblers. The temperature at which they are fully filled is
If the slope of P-T graph for a given mass of a gas increases, then the volume of the gas
The temperature at which a body does not radiate energy
A box contains x molecules of a gas. How will the pressure of the gas be affected if the number of molecules is made 2x?
In a gas equation, PV = RT, V refers to the volume of:
The relation between volume V, pressure P and absolute temperature T of an ideal gas is PV = xT, where x is a constant. The value of x depend upon
The density of an ideal gas
If pressure and temperature of an ideal gas are doubled and volume is halved, the number of molecules of the gas
The absolute temperature T of a gas is plotted against its pressure P for two different constant volumes V$$_{1}$$ and V$$_{2}$$ where V$$_{1}$$ > V$$_{2}$$. T is plotted along x-axis and P along y-axis.
The universal gas constant has the units
Universal gas constant per molecule is called
Equation of gas in terms of pressure $$p$$ absolute temperature $$T$$ and density $$d$$ is :
An ideal gas is that which
The density of air at N.T.P. is $$1.293 gm/lit$$. If the pressure is tripled keeping its temperature constant its density becomes
A gas is kept at 13$$^{0}$$C in a vessel. If the volume of the gas is kept constant and is heated, the pressure will be doubled to its initial pressure at a temperature
A bubble rises from the bottom of a lake, 90m deep. On reaching the surface, its volume becomes(take atmospheric pressure equals to 10 m of water )
A cylinder contains a gas at temperature of 27$$^{0}$$C and a pressure 1MPa. If the temperature of the gas is lowered to -23$$^{0}$$ C , the change in pressure is
A volume 'V' and temperature 'T' was obtained, as shown in the diagram, when a given mass of gas was heated. During the heating process, the pressure is
A gas at 627$$^{0}$$ C is cooled so that its pressure becomes $$\dfrac{1}{3}$$ of its initial value at constant volume. Its final temperature is
At 27$$^{0}$$ C certain gas occupied a volume of 4 litres. If the volume of this is to be increased to 12 litres at the same pressure, the gas is to be heated to a temperature
A P-V diagram is obtained by changing the temperature of the gas as shown. During this process the gas is :
For an isochoric process the temperature at which the pressure of a gas will be double that of its pressure at 270$$^{0}$$ C is
A car tyre has air at 1.5 atm at 300 K.If P increases to 1.75 atm with volume same, the temperature will be ____
The volume of a gas is 5 litres at N.T.P. what will be its volume at 273$$^{0}$$ C and at a pressure of four atmospheres
A gas at 27$$^{0}$$C and pressure of 30atm is allowed to expand to atmospheric pressure and volume 15 times larger. The final temperature of gas is
A sample of an ideal gas occupies a volume V at pressure P and absolute temperature T. The mass of each molecule is m. The equation for density is
At 20$$^{o}C$$ temperature and 1atmosphere pressure if a gas has a volume of 293 ml .Its volume at NTP is
The pressure of a gas is increased four times and its absolute temperature two times. The ratio of its final volume to its initial volume is
A cylinder contains gas at a pressure of 2.5 atm. Due to leakage, the pressure falls to 2 atm, after sometime. The percentage of the gas which is leaked out is
The diagram shows the graphs of pressure vs density for a given mass of an ideal gas at two temperatures T$$_{1}$$ and T$$_{2}$$ :
A given amount of gas is heated until both its pressure and volume are doubled. If initial temperature is 27$$^{0}$$ C, its final temperature is
One litre of helium under a pressure of 2 atm and at 27$$^{0}$$C is heated until its pressure and volume are doubled. The final temperature attained by the gas is
The volume of a gas at $$27^o$$C and 2 atmospheric pressure is 2 litres. If the pressure is doubled and absolute temperature is made half, the new volume of gas is
A closed vessesl contains 8 gms of oxygen and 7gm of Nitrogen. Total pressure at a certain temperature is 10 atm. When all the oxygen is removed from the system without chage in temperature then the pressure will be
The volume occupied by 8 gm of oxygen at S.T.P. is
An air bubble rises from bottom to top of a liquid of density 1.5 g/cm$$^{3}$$. If its volume is doubled, the depth of liquids is
If pressure of an ideal gas contains in a closed vessel is increased by 0.5% the increase in temperature is 20k the initial temperature of the gas is
Two closed vessels of the equal volume contain air at 105kPa at 300K and are connected through a narrow tube. If one of the vessels is now maintained at 300K and the other at 400K then the pressure becomes.
At the top of a mountain a thermo meter read 7$$^{0}$$ C and barometer reads 70 cm of Hg. At the bottom of the mountain the barometer reads 76cm of Hg and thermometer reads 27$$^{0}$$ C. The density of air at the top of mountains is ______ times the density at the bottom.
At a given temperature and pressure 64 gm of Oxygen and X gm of H$$_{2}$$ occupy the same volume. Then x= ......gm
A one litre sphere and a two litre sphere are connected with a capillary tube of negligible volume. They contain an ideal gas at 27$$^{0}$$C at a pressure of 100cm of Hg. Keeping the temperature of one litre sphere constant at 27$$^{0}$$C, if temperature of two litre sphere is increased to 127$$^{0}$$C, then the final pressure is
At the bottom of a lake where the temperature is $${7}^{0}\,C$$ the pressure is $$2.8$$ atmosphere. An air bubble of radius $$1\, cm$$ at the bottom rises to the surface. Where the temperature is $${27}^{0}\, C$$. The radius of the air bubble at the surface is
During an experiment an ideal gas is found to obey an additional law V$$^{2}$$P= constant. The gas is initially at a temperature T and volume V. When it expands to a volume 2V, the temperature becomes
Two gases A and B having same pressure P, volume V and temperature T are mixed. if the mixture has volume and temperature as V and T respectively the pressure of mixture is
A vessel is filled with an ideal gas at a pressure of 200 atm and is at a temperature of 27$$^{0}$$ C. One half of the mass of the gas is removed from the vessel and the temperature of the remaining gas is increased to 87$$^{0}$$ C. At this temperature,the pressure of the gas will be
Please disable the adBlock and continue. Thank you.
