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Calculate the pressure exerted by one mole of methane in a 450 mL container at 25^@C using van der Waals' equation. What pressure will be predicted by ideal gas equation ? (Given :
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Calculate the number of moles of gas present in the container of volume 10 L at 300 K. If the manometer containing glycerin shows 5 m difference in level as shown diagram.
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Calculate the temperature of 4.0 moles of a gas occupying 5 dm^3 at 3.32 bar (R = 0.083 bar dm^3 K^-1 mol^-1) .
Five moles of ideal gas expand isothermally and reversibly from pressure 10 ATM to 2 ATM at 300 K. What is the largest mass which can be lifted through a height of
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SOLVED: An ideal gas is heated at constant volume During this process the pressure increased from 1.00 atm to 3.98 atm. If the final temperature of the gas is found to be
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An ideal gas at 0.80 atmospheres and 87°C occupies 0.450 liter. How many moles are in the sample? - YouTube
