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A vessel of 120 mL capacity contains a certain amount of gas at 35 °C and 1.2 bar pressure.
According to Boyle’s Law P1 V1 = P2 V2 Here the temperature is constant. Therefore 1.2 X 120 = P2 X 180 OR P2 = 1.2 X 120 /180 = 0.8 bar Therefore, the pressure would be 0.8 bar.
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Give reasons: (a) A gas fills completely the vessel in which it is kept. (b) A gas exerts pressure on the walls of the container.
(a) There is little attraction between particles of gas. Thus, gas particles move freely in all directions. Therefore, gas completely fills the vessel in which it is kept. (b) Particles of...
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Seema visited a Natural Gas Compressing Unit and found that the gas can be liquefied under specific conditions of temperature
(c) Low temperature, high pressure
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Most living organisms cannot survive at temperature above 45°C. How are some microbes able to live in habitats with temperatures exceeding 100°C?
Archaebacteria (Thermophiles) are ancient forms of bacteria found in hot water springs and deep sea hydrothermal vents. They are able to survive in high temperatures (which far exceed 100°C) because...
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Why is the amount of gas collected in one of the test tubes double of the amount collected in the other in electrolysis of water experiment?
The gas which is collected in double the amount in the electrolysis of water experiment is hydrogen. This is because water (H2O) contains two parts of hydrogen element as compared...
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Even Carnot engine cannot give 100% efficiency because we cannot.
(c) Reach absolute zero temperature. We cannot reach absolute zero temperature.
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"Heat cannot by itself flow from a body at lower temperature to a body at higher temperature",
(a) Second law of thermodynamics.
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Curie temperature is the temperature above which.
(a) A ferromagnetic material becomes paramagnetic above Curie temperature.
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For an ideal gas, number of moles per litre in terms of its pressure P, gas constant R and temperature T is.
(c) : From ideal gas equation, PV = nRT Therefore, n/V = P/RT (number of moles = n/V)
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A gas behaves more closely as an ideal gas at (a) low pressure and low temperature
(b) low pressure and high temperature
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