Question

Enter your answer in the provided box. A sample of sulfur hexafluoride gas occupies 9.53 L at 215°C. Assuming that the pressure remains constant, what temperature (in °C) is needed to reduce the volume to 4.36 L? Report your answer to the proper number of significant figures.

Answer 1

Step-by-step explanation:

According to ideal gas equation, the product of pressure and volume equals to the product of number of moles, gas constant and temperature.

Mathematically, PV = nRT

Since, it is given that pressure is constant and Charle's law states that at constant pressure volume of an ideal gas is directly proportional to the absolute temperature.

Therefore,
`V \propto T`

`(V)/(T)` = constant

So, number of moles will also be constant then. Hence, the formula will be as follows.

`(V_(1))/(T_(1))` =
`(V_(2))/(T_(2))`

As it is given that
`V_(1)` is 9.53 L,
`V_(2)` is 4.36 L,
`T_(1)` is
`215^(o)C` that is also equal to (215 + 273) K = 488 K.

Now, putting these values into the formula as follows.

`(V_(1))/(T_(1))` =
`(V_(2))/(T_(2))`

`(9.53 L)/(488 K)` =
`(4.36 L)/(T_(2))`

`T_(2)` = 223.26 K

Temperature in degree celsius will be (223.26 K - 273 K) =
`-49.73^(o)C`

Thus, we can conclude that temperature (in °C) is needed to reduce the volume to 4.36 L is
`-49.73^(o)C`.