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.
is it 352???
I answered you below..in your earlier post.
To find the temperature at which methane needs to be heated to increase its pressure from 3.2 atm to 12 atm, you can use the combined gas law equation:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = initial pressure (3.2 atm)
V1 = initial volume (assuming it is constant, so we can ignore it for this problem)
T1 = initial temperature (21 °C converted to Kelvin by adding 273.15, so T1 = 21 + 273.15 = 294.15 K)
P2 = final pressure (12 atm)
V2 = final volume (again, assuming it is constant, so we can ignore it)
T2 = final temperature (what we need to find)
Rearranging the equation and plugging in the values:
(T2) = (P2 * V1 * T1) / (P1)
(T2) = (12 * V1 * 294.15 K) / (3.2)
Since we are only interested in finding the temperature difference, we can simply divide the value of T2 by the Kelvin scale factor:
T2 = [(12 * V1 * 294.15 K) / (3.2)] - 273.15
However, you have not provided the value for V1 (initial volume). Therefore, we need more information to calculate the exact temperature.