Gas tank A is filled with 53.5 L of 02. Gas tank B is filled with 1.44 x 1024 molecules of O^2. Both tanks are at STP. Which tank contains a greater mass of oxygen?
To compare the mass of oxygen in each tank, we need to use the molar mass of oxygen (O₂), which is 32 g/mol.
In tank A:
The volume is given as 53.5 L. At STP (Standard Temperature and Pressure), 1 mole of any gas occupies a volume of 22.4 L.
So, the number of moles of O₂ in tank A is 53.5 L / 22.4 L/mol = 2.384 mole.
The mass of oxygen in tank A is then calculated as:
Mass = number of moles x molar mass = 2.384 mole x 32 g/mol = 76.288 g.
In tank B:
The number of molecules is given as 1.44 x 10²⁴ molecules.
To find the number of moles, we should divide by Avogadro's number (6.022 x 10²³ molecules/mol).
So, the number of moles of O₂ in tank B is 1.44 x 10²⁴ molecules / 6.022 x 10²³ molecules/mol = 2.39 mole.
The mass of oxygen in tank B is then calculated as:
Mass = number of moles x molar mass = 2.39 mole x 32 g/mol = 76.48 g.
Comparing the two masses, we find:
Mass of oxygen in tank A = 76.288 g
Mass of oxygen in tank B = 76.48 g
Therefore, tank B contains a greater mass of oxygen.