At 2173K temp, and 9 atm pressure, the compressibility fog a gas is 0.9 . The volume of 1 mill-moles of gas at this temperature and pressure is :
The volume of 1 mole of a gas at standard temperature and pressure is:
The volume of 0.5 mole of gas at 1 atm pressure and 273^(@)C temperature is
Volume of 0.5 mole of a gas at 1 atm. Pressure and 273 K is
The volume of gas A is twice than that of gas B. The compressibility factor of gas A is thrice than that of gas B at same temperature. The pressures of the gases for equal number of moles are:
5.5mg of nitrogen gas dissolves in 180g of water at 273 K and 1 atm pressure due to nitrogen gas. The mole fraction of nitrogen in 180g of water at 5 atm nitrogen pressure is approximately
10 g of a gas at 1 atm and 273 K occupies 5 litres. The temperature at which the volume becomes double for the same mass of gas at the same pressure is:
Suppose 1.00 L of a gas with gamma = 1.30, initially at 285 K and 1.00 atm, is suddenly compressed adiabatically to half its initial volume. Find its final (a) pressure and (b) temperature. (C) If the gas is then cooled to 273 K at constant pressure, what is its final volume?
