States of Matter
A 2.24L cylinder of oxygen at 1 atm and 273 K is found to develop a leakage. When the leakage was plugged the pressure dropped to 570 mm of Hg. The number of moles of gas that escaped will be :
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At constant pressure, a sample of helium gas has a volume of 800 ml at 27oC. Calculate the temperature at which the volume will become 20% of its initial volume.
Equal weights of methane and hydrogen are mixed in an empty container at 25∘C. The fraction of the total pressure exerted by hydrogen is
Calculate the volume occupied by 5.0g of acetylene gas at 50∘C and 740mm pressure.
Two closed vessels of equal volume containing air at pressure P1 and temperature T1 are connected to each other through a narrow tube. If the temperature in one of the vessels is now maintained at T1 and that in the other at T2, what will be the pressure in the vessels?
A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.
The value of van der Waals constant a for the gases O2, N2, NH3, and CH4 are 1.360, 1.390, 4.170, and 2.253L2atmmol−2, respectively. The gas which can most easily be liquefied is
Assertion :Hot soup tastes better than the cold soup. Reason :Hot soup has high surface tension and it does not spread properly on our tongue.
X and Y are two volatile liquids with molar weights of 10gmol−1 and 40gmol−1 respectively. Two cotton plugs, one soaked in X and the other soaked in Y, are simultaneously placed at the ends of a tube of length L=24 cm, as shown in the figure. The tube is filled with an inert gas at 1 atm pressure and a temperature of 300K. Vapours of X and Y react to form a product whichh is first observed at a distance dcm from the plug soaked in X. Take X and Y to have equal molecular diameters and assume ideal behaviour for the inert gas and two vapours. The value of d in cm (shown in figure), as estimated from Graham's law, is