1.0 g of benzene is burnt completely in presence of 4.0g `O_(2)` in a completely evacuated bomb calorimeter of volume 1L. What is the pressure inside the bomb at `30^(@)C`, if the volume and pressure of water vapour produced are neglected?

Write the volume of vapour of 1 g water at 1 atmospheric pressure.

A sample of gas has a volume of 0.2 L, measured at 1 atm pressure and 0^@ C. At the same pressure but at 273^@ C, its volume becomes

A container of 1 L capacity contains a mixture of 4 g of O_(2) and 2 g H_(2) at 0 ^(@)C . What will be the total pressure of the mixture ?

At 25^(@)C , buring 0.2 "mole" H_(2) with 0.1 mole O_(2) to produce H_(2)O(l) in a bomb calorimeter (constant volume) raises the temperature of the apperaturs 0.88^(@)C . When 0.01mol toulene is burned in this calorimeter, the temperature is raised by 0.615^(@)C . Calculate DeltaH^(Theta) combustion of toluene. Delta_(f)H^(Theta) H_(2)O(l) =- 286 kJ mol^(-1) .

At 25^(@)C , buring 0.2 "mole" H_(2) with 0.1 mole O_(2) to produce H_(2)O(l) in a bomb calorimeter (constant volume) raises the temperature of the apperaturs 0.88^(@)C . When 0.01mol toulene is burned in this calorimeter, the temperature is raised by 0.615^(@)C . Calculate DeltaH^(Theta) combustion of toluene. Delta_(f)H^(Theta) H_(2)O(l) =- 286 kJ mol^(-1) .

A 1.0 L flask contains 2.0 g of N_(2), 0.4 g H_(2) and 9.0 of O_(2) at 27^(@)C . What is the pressure in the flask?

The heat of combusion of benzene in a bomb calorimeter (i.e constant volume) was found to be 3263.9kJ mo1^(-1) at 25^(@)C Calculate the heat of combustion of benzene at constan pressure .

The heat of combusion of benzene in a bomb calorimeter (i.e constant volume) was found to be 3263.9kJ mo1^(-1) at 25^(@)C Calculate the heat of combustion of benzene at constan pressure .