A contaienr of volume 2 litre contains `H_(2)` gas at 300 K as shown `(P_("atm")=76cm "of" Hg)`

The pressure (in cm Hg) of `H_(2)` in the contaienr is

If 4 litre of H_(2) gas at 400 mm Hg and 47^(@)C is transferred to 19 litre flask at 107^(@)C . Then pressure of H_(2) gas is:

Two container each containing liquid water are connected as shown in diagram. Given that vapour pressure of H_(2)O(l) at 300K and 350K and 22 mm of Hg and 40mm of Hg. The final pressure in each container if valve is opened while keeping the containers at the given temperatre is :

If same amount of gas is trapped over liquid (a) and liquid (b) in following containers. Assuming temperature and cross-sectional area of container are same. P_(atm)=760mm Hg,d_(Hg)=13.6 g//mL Find the pressure (in cm Hg) of gas over the liquid (b).

If same amount of gas is trapped over liqquid (a) and liquid (b) in following container4s. Assuming temperature and cross-sectional area of container are same. P_("atm")=760mmHg,d_(Hg)=13.6g//mL If same amount of gas is trapped over liquid (a) and liquid (b) in following containers. Assuming temperature and cross-sectional area of container are same. P_(atm)=760mm Hg,d_(Hg)=13.6 g//mL Find the pressure (in cm Hg) of gas over liquid (a)

O_(2) gas is placed in a 4 litre container containing 3 L of liquid water as shown and total pressure exerted by gases is 720mm Hg. What will be the pressure of O_(2)(g) if given container is attached to a empty container of 3 litre at same temperature? Given : [V.P. of H_(2)O at 27^(@)C=20mm of Hg]

A evacuated bulb of unknown volume is filled with H_(2) gas at room temperature (30^(@)C) . The pressure of the gas in the bulb is 750 mm Hg. A portion of the gas is transferred to a different flask and found to occupy a volume of 50.0 mL at 1 atm pressure and at the same temperature. the pressure of the H_(2) gas remaining in the original bulb drops to 600 mm Hg. What is the volume of the bulb assuming H_(2) gas is an ideal gas ?

A container is divided into two compartments. One compartment contains 2 moles of N_(2) gas at 1 atm and 300 K and other compartment contains H_(2) gas at the same temperature and pressure. Volume of H_(2) compartment is four times the volume of N_(2) compartment [Assuming no reaction under these conditions] If the container containing N_(2) and H_(2) are further heated to 1000 K, forming NH_(3) with 100% yeild calculate the final total pressure.

An evacuated bulb of unknown volume is filled with a sample of H_(2) gas at a temperature T The pressure of the gas in the bulb is 756mm Hg A portion of the H_(2) gas is transferred to a different flask and found to occupy a volume of 40.0mL at 1.00 atn and the same temperature T The pressure of the H_(2) gas remaining in the original bulb drops to 625mm hg at the same temperature T Assuming H_(2) is an ideal gas, what is the volume of the bulb ? .

In the above figure mercury columns of 10 cms each are trapped between gas columns of 10 cm each . If P_(atm)=75 cm of Hg then the gas pressure in the topmost column will be

In the above figure mercury columns of 10 cms each are trapped between gas columns of 10 cm each . If P_(atm)=75 cm of Hg then the gas pressure in the topmost column will be