Dry ice is solid carbon dioxide. A 0.050 g sample of dry ice is placed in an evacuated 4.6 L vessel at `30^(@)C`. Calculate the pressure inside the vessel after all the dry has been converted to `CO_(2)` gas.
10 g of O_(2) were introduced into an evacuated vessel of 5 litre capacity maintained at 27^(@)C . Calculate the pressure of the gas in atmosphere in the container.
Decomposition of ammonium chloride is an endothermic reaction. The equilibrium may be represented as: NH_(4)Cl(s) hArr NH_(3)(g)+HCl(g) A 6.250 g sample of NH_(4)Cl os placed in an evaculated 4.0 L container at 27^(@)C . After equilibrium the total pressure inside the container is 0.820 bar and some solid remains in the container. Answer the followings The amount of solid NH_(4)Cl left behind in the container at equilibrium is
Decomposition of ammonium chloride is an endothermic reaction. The equilibrium may be represented as: NH_(4)Cl(s) hArr NH_(3)(g)+HCl(g) A 6.250 g sample of NH_(4)Cl os placed in an evaculated 4.0 L container at 27^(@)C . After equilibrium the total pressure inside the container is 0.820 bar and some solid remains in the container. Answer the followings If the volume of container were doubled at constant temperature, then what would happen to the amount of solid in the container.
44g dry ice is placed in a bottle of 1 litre capacity and tightly corked Calculate the total pressure in bttle after complete evaporation of dry ice at 300K .
A vessel of 4.00L capacity contains 4.00 g of methane and 1.00 g of hydrogen at 27^(@)C . Calculate the partial pressure of each gas and also the total pressure in the container.
2 moles each of hydrogen, carbon dioxide and chlorine are mixed in a close vessel of volume 3 litres and temperature 0^@ C . Calculate the pressure exerted by the mixture. ( R=8.31 J mol^(-1) K^(-1) )
