Asample 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

This is what i found on google “when one phosphate group is removed by breaking a phosphoanhydride bond in a process called hydrolysis, energy is released, and atp is converted to adenosine diphosphate (adp). likewise, energy is also released when a phosphate is removed from adp to form adenosine monophosphate (amp).” i hope this you .

Exothermic,  physical change after it is already baked