The pressure of a gas sample in a rigid
container is 810.0 mmHg at 22 oC. What is the
pressure, in mmHg, at 50 oC?
I have a rough idea on how to solve, but which equation do I use?
nevermind, got it!
To solve this problem, you can use the combined gas law equation. The combined gas law relates the temperature, pressure, and volume of a gas sample, assuming the number of moles of gas remains constant. The equation is as follows:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 and P2 = Initial and final pressures, respectively
V1 and V2 = Initial and final volumes, respectively
T1 and T2 = Initial and final temperatures, respectively
In this specific case, you are given the initial pressure (P1 = 810.0 mmHg) and temperature (T1 = 22 °C). You need to find the final pressure (P2) at a final temperature (T2 = 50 °C).
First, you need to convert both temperatures to Kelvin by adding 273.15 to them. So, T1 = 22 + 273.15 = 295.15 K and T2 = 50 + 273.15 = 323.15 K.
Now you can substitute the given information into the equation:
(P1 * V1) / T1 = (P2 * V2) / T2
Since the volume (V) and the number of moles of gas are not specified, they cancel out of the equation. Thus, you can solve for P2:
P2 = (P1 * T2) / T1
Now, you can plug in the known values:
P2 = (810.0 mmHg * 323.15 K) / 295.15 K
After performing this calculation, you will find the final pressure (P2) in mmHg.