A pressurized can of whipped cream has an internal pressure of 1.080 atm at 25°C. If it is placed in a freezer at -8°C, what is the new value for its internal pressure (in atmospheres)?

I did this but got a negative number that wasn't correct

If you will show you work I will find ?the error. Did you use kelvin for T.

(1.080)(-8)=(265)(P)

-8.64=265P
265p/ -8.64= -30.67

You didn't answer my question and you did NOT use kelvin. You must convert celsius to kelvin.

kelvin = 273 + C.

i thought i did

298/-8.64=-34.49

298=273+20

No you didn't. Actually, you converted the -8C to kelvin, then used 265(the correct value for T2 and -8 (the same number) for T1.

K = 273 + C
25C = 298K since 273+ 25 = 298.
-8C
273-8 = 265K.

(P1/T1) = (P2/T2)
(1.08/298) = (P2/265)
P2 =

To calculate the new value for the internal pressure of the pressurized can of whipped cream when placed in a freezer, you need to use the ideal gas law equation. The ideal gas law relates the pressure (P), volume (V), and temperature (T) of a gas using the equation PV = nRT, where n is the number of moles of gas and R is the ideal gas constant.

In this case, since the can is sealed and its volume remains constant, we can use the rearranged form of the ideal gas law:

P1/T1 = P2/T2

Where P1 is the initial pressure, T1 is the initial temperature, P2 is the final pressure, and T2 is the final temperature.

First, let's convert the temperatures to Kelvin since the ideal gas law equation requires temperatures in Kelvin. To convert from Celsius to Kelvin, you need to add 273.15:

Initial temperature T1 = 25°C + 273.15 = 298.15 K
Final temperature T2 = -8°C + 273.15 = 265.15 K

Now, we can plug these values into the equation:

P1/T1 = P2/T2

1.080 atm / 298.15 K = P2 / 265.15 K

Now, let's solve for P2:

P2 = (1.080 atm * 265.15 K) / 298.15 K

P2 = 0.960 atm

Therefore, the new value for the internal pressure of the pressurized can of whipped cream in the freezer is approximately 0.960 atm. Note that the pressure cannot be negative, so if you obtained a negative value, there might have been an error in your calculations.