Asample of sulfur hexafluoride gas occupies a volume of 9.10 l at 198ác. assuming that the pressure remains constant, what temperature (in ác) is needed to reduce the volume to 2.50 l?

Temperature -143.6°C is needed to reduce the volume to 2.50 L

There are several gas equations in various processes:  

•1. Avogadro's hypothesis  

In the same temperature and pressure, in the same volume conditions, the gas contains the same number of molecules  

So it applies: the ratio of gas volume will be equal to the ratio of gas moles  

•2. Boyle's Law  

At a fixed temperature, the gas volume is inversely proportional to the pressure applied  

•3. Charles's Law  

When the gas pressure is kept constant, the gas volume is proportional to the temperature  

•4. Gay Lussac's Law  

When the volume is not changed, the gas pressure in the tube is proportional to its absolute temperature  

•5. Law of Boyle-Gay-Lussac  

Combined with Boyle's law and Gay Lussac's law  

P1 = initial gas pressure (N / m2 or Pa)  

V1 = initial gas volume (m3)  

P2 = gas end pressure  

V2 = the final volume of gas  

T1 = initial gas temperature (K)  

T2 = gas end temperature  

In the problem, the conditions that are set constant are Pressure, so we use Charles' Law

V1 / T1 = V2 / T2

V1 = 9.1 L

T1 = 198 °C+273 = 471 K

V2 = 2.5 L

Then :

a description of Charles’s law

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Charles's law

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State Boyle's, Charles's, and Gay-Lussac's laws

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Keywords : Charles Law, temperature, pressure, vollume, gas, sulfur hexafluoride

the answer is true. hope it .

pv=nrt

explanation: