40.0 dm3 of an ideal gas at 250C and 750 mm Hg is expanded to 50.0 dm3. The pressure of the gas changed to 765 mm Hg. What is the temperature of the gas?
Correct answer: C. (298)(765)(50)/(750)(40)
- A. (298)(750)(50)/(40)(765)
- B. (298)(750)(40)/(50)(765)
- C. (298)(765)(50)/(750)(40)
- D. (40)(750)/(298)(50)(765)
Explanation
PV=nRTAccording to the ideal gas equation: PV = nRT. P1V1/T1=P2V2/T2 OrT2=P2V2T1/ P1V1 So T2 Should be solved as follows T2 =765*50*298/750*40
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About Ideal Gas Equation
The ideal gas equation, PV = nRT, relates pressure, volume, amount and absolute temperature when gas particles are assumed to have negligible volume and no intermolecular forces. Applications include finding molar mass, density or an unknown gas variable, with careful use of Kelvin temperature and consistent units, and comparison with real-gas behaviour.
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