When the volume of a gas is changed from mL to 852 mL,

the temperature will change from

315°C to 452°C.

The initial volume is 593.76mL

Step-by-step explanation:

As you do not say anithing about the pressure, i guess that the pressure remains constant.

If the gas is an ideal gas, we have:

P*V = n*R*T

where P is pressure, n is number of moles and R is a constant.

Now, initially we have:

P*Vi = n*R*315°C

finally we have:

P*825mL = n*R*452°C

Now we can take the quiotient of those two equations and get:

(P*Vi)/(P*852mL) = (n*R*315°C)/( n*R*452°C)

Now we have:

Vi/852mL = 315/452

Vi =  (315/452)*852mL = 593.76mL

So when we expand the gas at constant pressure, we increase the temperature.  

step-by-step explanation: