Question

Question #5954a

Answer 1

It depends on the temparature and pressure.

Explanation:

First, find the amount of substance(mol) of the gas.

If the temparature and pressure are at STP(`0`℃, `10^5` Pa), the molar volume of ideal gas is `V_m=22.711` L/mol.
When the temparature is `0`℃ and the pressure is `1` atm(`1.01325xx10^5` Pa), the molar volume is `V_m=22.414` L/mol.

Then, the amount of substance is `n=V/V_m` where `V` is the volume(in this question, `V=5000` L).

Otherwise, you should use the ideal gas law.
`pV=nRT`, where:
`p`: pressure (Pa)
`V`: volume (`m^3`)
`n`: amount of substance(mol)
`R`: gas constant (`=8.3145 m^3 Pa K^-1 mol^-1`)
`T`: temparature (K).

Once you find the amount of substance, multiply it by the molar mass of chlorine molecule (`Cl_2=70.906` g/mol).

For example, the amount of substance of `5000` L `Cl_2` at STP is `n=5000/22.711= 220.16` moles, and its mass is `220.16*70.906=15610.6… = 1.561xx10^4` grams.