Chemistry
Following questions refer to one mole of chlorine gas.
(a) What is the volume occupied by this gas at S.T.P.?
(b) What will happen to the volume of gas, if pressure is doubled?
(c) What volume will it occupy at 273°C?
(d) If the relative atomic mass of chlorine is 35.5, what will be the mass of 1 mole of chlorine gas?
Related Questions
(a) Calculate the mass of substance 'A' which in gaseous form occupies 10 litres at 27°C and 700 mm pressure. The molecular mass of 'A' is 60.
(b) A gas occupied 360 cm3 at 87°C and 380 mm Hg pressure. If the mass of gas is 0.546 g, find it's relative molecular mass.
A gas cylinder can hold 1 kg of hydrogen at room temperature and pressure.
(a) What mass of carbon dioxide can it hold under similar conditions of temperature and pressure?
(b) If the number of molecules of hydrogen in the cylinder is X, calculate the number of carbon dioxide molecules in the cylinder. State the law that helped you to arrive at the above result
A compound A consists of 4.8% carbon and 95.2% bromine by mass. Its vapour density is 252. Find its :
(i) empirical formula
(ii) molecular formula
From the equation:
C + 2H2SO4 ⟶ CO2 + 2H2O + 2SO2
Calculate:
(i) The mass of carbon oxidized by 49 g of sulphuric acid.
(ii) The volume of sulphur dioxide measured at STP, liberated at the same time.