Question

Determine the volume (in L) of chlorine that forms from the decomposition of 5.0g of Cl₂ under each set of conditions.

a) Standard temperature and pressure (STP)
b) Non-STP conditions

Answer 1

To find the volume of chlorine formed from the decomposition of 5.0g of Cl₂, we can use the molar volume of gases at standard temperature and pressure (STP). At STP, one mole of any gas occupies a volume of 22.4 L. Therefore, 5.0g of Cl₂ will form approximately 1.58 L of chlorine gas at STP.

Step-by-step explanation:

To determine the volume of chlorine formed from the decomposition of 5.0g of Cl₂, we need to use the molar volume of gases at standard temperature and pressure (STP). At STP, one mole of any gas occupies a volume of 22.4 L. The molar mass of Cl₂ is 70.90 g/mol, which means that 1 mole of Cl₂ weighs 70.90 g. Therefore, to find the volume of Cl₂ formed, we can use the following calculation:

moles of Cl₂ = mass of Cl₂ / molar mass of Cl₂ = 5.0g / 70.90 g/mol = 0.0705 mol

volume of Cl₂ = moles of Cl₂ * molar volume at STP = 0.0705 mol * 22.4 L/mol = 1.58 L

So, under standard temperature and pressure conditions, 5.0g of Cl₂ will form approximately 1.58 L of chlorine gas.

Under non-STP conditions, the volume of chlorine formed will depend on the specific temperature and pressure. To calculate the volume of chlorine under non-STP conditions, we would need additional information such as the temperature and pressure.