`821mLN_(2) (g)` was collected over liquid water at 300 K and 1 atm.If vapour pressure of `H_(2)O` is 30 torr then moles of `N_(2) (g)` in moist gas mixture is :
What is the density of wet air with 75% relative humidity at 1 atm and 300 K? Given : vapour pressure of H_(2)O is 30 torr and average molar mass of air is 29 g mol^(_1) .
A sample of air contains only N_(2)O_(2) and H_(2)O . It is saturated with water vapours and total pressure is 640 torr. The vapour pressure of water is 40 torr and the molar ratio of N_(2):O_(2) is 3:1. The partial pressure of N_(2) in the sample is :
A sample of air contains only N_(2), O_(2), and H_(2)O . It saturated with water vapours and total pressure is 6 "torr" . The vapour pressure of water is 40 "torr" and the mol ratio of N_(2):O_(2) is 3:1 . The partial pressure of N_(2) in the sample is
A mixture of CH_(4) and C_(2)H_(2) occupied a certain volume at a total pressure equal to 63 torr. The same gas mixture was burnt to CO_(2) and H_(2)O(l).CO_(2)(g) alone was collected in the same volume and at the same temperature, the pressure was found to be 99 torr. What was the mole fraction of CH_(4) in the original gas mixture?
8.2 L of an ideal weight 9.0 g at 300 K and 1 atm. pressure. The molecular mass of gas is
A gas 'X' is present with saturated water vapour over water liquid at total pressure of 1.5 atm. Vapour pressure of H_2O at same temperature is 0.5 atm. What is the solubility of gas 'X' in terms of moles in 10 moles H_2O . The slope of the graph is 5000.
