Answered

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A sample of chlorine gas starting at 688 mm Hg is placed under a pressure of 994 mm Hg and reduced to a volume of 500.2 mL. What was the initial volume, in mL, of the chlorine gas container if the process was performed at constant temperature?

Sagot :

(P1V1=nRT1)/(P2V2=nRT2)

Constant temperature → (P1V1)/(P2V2)

688 mm Hg → 0.905 atm

994 mm Hg → 1.30789 atm

500.2 mL → 0.5002 L

(P1V1)/(P2V2)

(0.905)V1/(1.30789)(0.5002)

V1 = 0.72288 L → 722.88 mL

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