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How can I calculate the volume, in liters, of 1.50 mol Cl2 at STP?

1 Answer

May 25, 2014

To calculate this we can use the Ideal gas law of $P V = n R T$ $PV=nRT$

At STP (Standard Temperature and Pressure)
P = 1 atm
V = ?
n = 1.50 mol
R = 0.0821 $\frac{a t m L}{m o l K}$ $(atmL)/(molK)$
T = 273 K

$(1 a t m) (V) = (1.50 m o l) (0.0821 \frac{a t m L}{m o l K}) (273 K)$ $(1 atm)(V) = (1.50 mol) (0.0821 (atmL)/(molK))(273K)$

$V = \frac{(1.50 m o l) (0.0821 \frac{a t m L}{m o l K}) (273 K)}{1 a t m}$ $V= ((1.50 mol) (0.0821 (atmL)/(molK))(273K))/(1 atm)$

$V = 33.6 \frac{L}{m} o l$ $V= 33.6 L/mol$

I hope this was helpful.
SMARTERTEACHER

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