1 atm = ?___mmHg.

1 atm = ?___ cmHg.

One litre flask contains air, water vapour and a small amount of liquid water at a pressure of 200 mmHg. If this is connected to another one litre evacuated flask, what will be the final pressure of the gas mixture at equilibrium? Assume the temperature to be 50^@C . Aqueous tension at 50^@C=93 mmHg

1 mmHg= ?___ torr ?

Density of oxygen at STP is 1.429 g.L^-1 What will be the mass of 2.5 L of oxygen gas at 27^@C and at 780 mmHg pressure?

A and B cells are contiguous. Cell A has OP=10 atm, TP=7 atm and DPD=3 atm. Cell B has OP=8 atm. TP=3 atm and DPD=5 atm. The result would be

The volume of some amount of gas at STP is 2L.What will be its volume at 91^@C and at 570 mmHg pressure?

At 540, the equilibrium constant K_(p) for PCl_(5) dissociation equilibrium at 1.0 atm 1.77 atm. Calculate equilibrium constant in molar concentration (K_(c)) at same temperature and pressure.

The volume of a fixed mass of gas at STP is 500 cm^3. What will be its volume at 700 mmHg pressure if its temperature remains constant?

Work done during isothermal expension of one mole of an ideal gas from 10 atm to 1 atm at 300 K is

Enthalpy of fusion of ice at 0^(@)C and 1 atm is 6.02 kJ *mol^(-1) . The change in entropy (J*K^(-1)) of the surroundings when 9 g of water is frozen at 0^(@)C and 1 atm pressure is-