Question

A sample of sulfur hexafluoride gas occupies 6.63 L at 241°C. Assuming that the pressure remains constant, what temperature (in °C) is needed to reduce the volume to 3.01 L? Report your answer to the proper number of significant figures. -173°C

Answer 1

The objective is to calculate the temperative Cin oC) is needed to reduce the volume to 3.01L to the following data. Aus Given that, The ideal gas law as follows: PV=nRT Here, Ra Gas constant = 8.3145 J K'mol The ideal gas law for these two conditions for Sulfur hexafluviatide is following: Pixui. P2 X Vz Tixni TaXMq. Here, na initial and final number of mol. P, and Pq=P. vis initial volume = 6. 6L.

Vq = final volume =3.01 To=24100 = 2414273k=514k. Now, calculate the required temperature of gas by putting all values in the above ideal gas law Pixui PqXvq TIXMI. T2 X M2 - To = Pq X Ve , Tini na Pixni 8x3.01 514x4 K . . 8x6.634 -13.01x514)/6.63 £1547.14 16.63 2233.35k. Now it converted into degree Celsius as follows: 233.35k-273 == 39.65 ~ -40°c. At constant pressure;F-40°C temperature is required to reduce volume of Sulfur hexafluoride gas from 6.63 1 to 3.01L