How many milliliters of [tex] \text{Cl}_2 [/tex] gas must you have to obtain 0.20 g at STP?

STP = Standard Temperature (273 K) Pressure (1 atm)
we also have the mass of cl2, 0.2g. We use this to find the number of moles.
Use the ideal gas law. PV = nRT P= pressure in atm V= volume in Liters n = number of moles of gas R = 0.082058 T = Temperature in Kelvin
P = 1 atm V = ? (we are looking for this) n = moles = mass/molar mass = 0.2g/(2*35.453) = 0.0028 moles R = 0.082058 T = 273 K
(1)V = (0.0028)(0.082058)(273) V = 0.063 L = 60 mL (1 sig fig)
good luck!

Answered by cxcharlie | 2024-06-10

To obtain 0.20 g of Cl₂ at STP, you need approximately 63 mL of chlorine gas. This is calculated by first determining the moles from the mass and then using the molar volume at STP. The molar mass of Cl₂ is about 70.906 g/mol, leading to the final calculation of volume required.
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Answered by cxcharlie | 2024-12-23