568 cm3 of chlorine at 25° C will occupy what volume at -25° C while the pressure remains constant?

Answer 1

Hey Tia for this question we need to assume two things. That being pressure and the number of moles of chlorine remain constant. The two things that are changing are volume and temperature of the chlorine, which means we are dealing with Charles's law. Which is V1/T1=V2/T2, where V is equal to the volume of the gas and T is equal to the temperature of the gas, the 1 next to the number means initial and 2 is equal to final. So in words that means the initial volume/initial temperature=final volume/final temperature. Now it is important to convert the Celsius into Kelvin so the calculations can work, which we can do by adding 273.15 to each Celsius value.

25+273.15=298.15

-25+273.15=248.15

So from here we just need to plug these numbers into the equations and we get the following.

568/298.15=V2/248.15

1.90508=V2/248.15

From here we need to multiply both sides by 248.15 and when we do we get the following.

V2=472.7459cm³ but since the Celsius figures only had 2 sig figs we must round this answer to 2 sig figs.

V2=470 cm³

If you have any questions feel free to ask at any time.