Question

A sample of sulfur hexafluoride gas occupies 8.50 L at 165°C. Assuming that the pressure remains constant, what temperature (in °C) is needed to reduce the volume to 3.70 L?

Answer 1

To find the temperature needed to reduce the volume of sulfur hexafluoride gas from 8.50 L to 3.70 L at constant pressure, we use Charles's Law and calculate it to be approximately -83°C.

Step-by-step explanation:

The subject of this question is Chemistry, specifically relating to the concepts of gas laws. To solve for the temperature needed to reduce the volume of sulfur hexafluoride gas from 8.50 L to 3.70 L at constant pressure, we can use Charles's Law.

Charles's Law states that the volume of a gas is directly proportional to its temperature in kelvins, assuming the pressure is constant. The formula is V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature respectively.

First, we need to convert the initial temperature from Celsius to Kelvin by adding 273.15, which gives us 165 + 273.15 = 438.15 K. Then we apply Charles's Law:

(8.50 L / 438.15 K) = (3.70 L / T2)

We solve for T2:

T2 = (3.70 L × 438.15 K) / 8.50 L

T2 = 190.097 K

To convert this temperature back to Celsius, we subtract 273.15:

T2 = 190.097 K - 273.15

T2 = -83.053°C

So, the temperature needed to reduce the volume to 3.70 L is approximately -83°C.