Question: how to solve for a 28.4 L sample of methane gas is heated from 35.0° C to 76.0° C. The initial pressure of the gas is 1.00 atm at 35.0° C. Assuming constant volume, what is the final pressure of the gas?
Could someone give me the setup for this? I know I have to change my temp to K, but there is three different temps and I wanted to use the formula P1V1T1/P2V2/T2, but I only have one a V1 and no V2. I need to find P2 and V2. Help please
a. Your formula you want to use is not right. I suspect you just made a typo.
b. Of course there is only one volume. The problem says constant volume; therefore, you don't need a volume.
c. There are not three Temps. I see only two. The gas goes from 35C to 76 C and it starts at 1 atm.
d. Use (P1/T1) = (P2/T2) and solve for P2.
To solve this problem, you can use the Ideal Gas Law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
In this case, you want to find the final pressure (P2) of the gas, assuming constant volume.
To set up the equation, you need to convert the temperatures from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature. So, you can convert the initial temperature (T1 = 35.0°C) and final temperature (T2 = 76.0°C) as follows:
T1 = 35.0°C + 273.15 = 308.15 K
T2 = 76.0°C + 273.15 = 349.15 K
Given:
Initial pressure (P1) = 1.00 atm
Initial volume (V1) = 28.4 L
Since the volume (V) is constant, you can eliminate V1 and V2 from the equation, leaving you with:
P1/T1 = P2/T2
Now, you can plug in the known values:
1.00 atm / 308.15 K = P2 / 349.15 K
To solve for P2, you can rearrange the equation:
P2 = (1.00 atm * 349.15 K) / 308.15 K
P2 ≈ 1.14 atm
Therefore, the final pressure of the gas is approximately 1.14 atm.
To solve this problem, you can use the combined gas law equation:
P1V1/T1 = P2V2/T2
Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure (what we want to find)
V2 = final volume (constant volume, so V2 = V1)
T2 = final temperature
Since we are assuming constant volume, V2 is equal to the initial volume, V1. So we don't need to find V2.
The given information is:
P1 = 1.00 atm
T1 = 35.0°C
First, let's convert the temperatures to Kelvin:
T1 = 35.0°C + 273.15 = 308.15 K
T2 = 76.0°C + 273.15 = 349.15 K
Now, we can substitute the values into the combined gas law equation:
(1.00 atm) * (V1) / (308.15 K) = (P2) * (V1) / (349.15 K)
Notice that V1 cancels out on both sides of the equation. So, we are left with:
1.00 / 308.15 = P2 / 349.15
Now, we can solve for P2:
P2 = (1.00 / 308.15) * 349.15
Calculating this expression will give you the final pressure, P2, in atm.