If methane at a pressure of 3.2 atm and at 21 °C is introduced into a container, the gas be heated to ______°C to increase the pressure to 12 atm.

To determine the temperature at which the pressure of methane increases to 12 atm, we can use the combined gas law. The combined gas law allows you to relate the initial and final conditions of a gas when pressure, volume, and temperature change.

The combined gas law is given by:

(P1 * V1) / T1 = (P2 * V2) / T2

Where:
P1 and P2 are the initial and final pressures, respectively.
V1 and V2 are the initial and final volumes, respectively.
T1 and T2 are the initial and final temperatures, respectively.

We are given the initial pressure (P1 = 3.2 atm), the initial temperature (T1 = 21 °C), and the final pressure (P2 = 12 atm). We need to find the final temperature (T2).

Convert the temperatures to Kelvin:
T1 = 21 °C + 273.15 = 294.15 K

Rearrange the combined gas law equation to solve for T2:
T2 = (P2 * V2 * T1) / (P1 * V1)

Since we don't have any information about the volume of the container or any volume changes, we can assume it remains constant. This means V1 = V2, so we can simplify the equation to:
T2 = (P2 * T1) / P1

Substitute the given values into the equation:
T2 = (12 atm * 294.15 K) / 3.2 atm

T2 = 1103.5875 K

Convert the temperature back to Celsius:
T2 = 1103.5875 K - 273.15 = 830.44 °C

Therefore, the gas would need to be heated to approximately 830.44 °C to increase the pressure to 12 atm.

i got 831 i don't think this is right???

K=C+273

=21+273
=294k

P1/T1=P2/T1

3.3/294=12/T1

T1=1102.5k
Therefore need to be increased by 829.5 degrees Celsius.
Is this correct?

I got something different:

3.2/294 = 12/K

That gives us the Kelvin temp then subtract 273 to get C.

Temperature and Pressure are proportional. If you increase the temperature, the pressure will increase.

P1/T1 = P2/T2

Temperature has to be in Kelvin

C + 273 = K

i got 352 is that right