A gas cylinder can hold 1 kg of hydrogen at room temperature and pressure
(a) What mass of carbon dioxide can it held under the similar condition 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 gas cylinder can hold 1 kg of hydrogen at room temperature and pressure
(a) What mass of carbon dioxide can it held under the similar condition 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.
Here temperature, pressure and volume ( cylinder) all are constant.
so, the number of moles must be constant.
mole of hydrogen gas = given massmolar mass=10002=500mole.
mole of carbon dioxide = given massmolar mass
500=given wt44
given wt =500×44=22kg
b) here the number of moles is constant
so, no of molecules also constant because of
no of molecules = mole × Avogadro's constant
so, the number of molecules of carbon dioxide are also equal to X
The Avagadro's law is applied here which states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules.
Here temperature, pressure and volume ( cylinder) all are constant.
so, the number of moles must be constant.
mole of hydrogen gas = given massmolar mass=10002=500mole.
mole of carbon dioxide = given massmolar mass
500=given wt44
given wt =500×44=22kg
b) here the number of moles is constant
so, no of molecules also constant because of
no of molecules = mole × Avogadro's constant
so, the number of molecules of carbon dioxide are also equal to X
The Avagadro's law is applied here which states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules.
