solve for the new pressure when each of the following temperature changes occurs, with n and V constant:
b. an aerosol can has a pressure of 1.40 atm at 12 celcius.what is the final pressure in the aerosol can if it is used in a room where the temperature is 35 celcius?
Same process as previous question.
To solve this problem, we can use the ideal gas law which states that the product of pressure (P) and volume (V) is proportional to the product of the number of moles of gas (n) and the temperature (T) of the gas. Mathematically, it can be represented as:
PV = nRT
In this case, we are given that the number of moles (n) and the volume (V) of the aerosol can are constant. Therefore, we can rewrite the equation as:
P1/T1 = P2/T2
Where:
P1 is the initial pressure of the aerosol can
T1 is the initial temperature of the aerosol can
P2 is the final pressure in the aerosol can
T2 is the final temperature in the room
Now let's plug in the given values:
P1 = 1.40 atm
T1 = 12°C + 273 = 285 K (converting Celsius to Kelvin)
T2 = 35°C + 273 = 308 K
Now, rearrange the equation to solve for P2:
P2 = (P1 * T2) / T1
Substituting the values we obtained:
P2 = (1.40 atm * 308 K) / 285 K
P2 ≈ 1.51 atm
Therefore, the final pressure in the aerosol can, when used in a room where the temperature is 35°C, would be approximately 1.51 atm.