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What is the volume of 1.50 moles of chlorine gas (Cl2) at 273 K and 1.00 atm? 22.4 L 33.6 L 57.5 L 71.0 L

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Ideal Gas Law equation: PV= nRT
⇒ V= nRT/ P
⇒ V= (1.50 mol)* (0.08206 L*atm/ (K*mol))* 273 K/ 1.00 atm= 33.6 L.

The final answer is 33.6 L.

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User Panos Bariamis
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