A sample of sulfur hexafluoride gas occupies a volume of 4.000 liters at 7.836x10 C assuming the pressure is constant what will the final temperature be if the volume is increased to 9.840 liters?

So you know the ideal gas law

PV = nRT

well R is a constant, Pressure is given to be constant and of course the moles, n are constant.

What is left is direct variation.

Initial temp and volume

V = kT

final temp and volume

v = kt

crate a ratio, I think this is called charles law

V/v = T/t

4 / 9.840 = 7.836x10 / t

solve for final temp, will be in Celsius since T is in Celsius

* * round answer to 4 significant figures ...

t = (78.36 * 9.84) / 4

t = 192.8 C