I reall need help, i know what formulas to use i just don't know how to do it. Can some one please work with me to get to the correct answer?
1.The air in a dry, sealed 2L soda bottle has a pressure of 0.998 atm at sea level at a temperature of 34C. what will be it's pressure, if it is brought to higher altitude where the temperature is only 23C?
P1/T1 = P2/T2.
P1 = 0.998 atm.
T1 = 273 + 34 = ??Kelvin.
P2 = solve for this.
T2 = 273 + 23 = ??Kelvin.
Substitute and solve for P2 (in atm)
Am i using the Gay-Lussacs law?
I think so but I'm not absolutely positive. I don't pay much attention to the names, I just know how to work the problem. I remember the name of Boyle's Law.
Lol, Thank you. Ima work it out and im going to write my answer and can you tell me if im right or wrong?
Ok, So when i worked it out i got .962 And I moved the decimal right and made it 9.62x10^-1
Is this right?
Sure, I'd be happy to help you work through this problem. To solve this question, we can use the ideal gas law equation: PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles of gas
R = Ideal gas constant
T = Temperature
In this case, we have the initial pressure (P1 = 0.998 atm), initial temperature (T1 = 34°C), final temperature (T2 = 23°C), and the volume (V = 2L).
First, let's convert the temperatures from Celsius to Kelvin since the ideal gas law equation requires the temperature to be in Kelvin.
T1 = 34°C + 273.15 = 307.15 K
T2 = 23°C + 273.15 = 296.15 K
Now, let's plug in the known values into the equation and solve for the final pressure (P2):
(P1)(V) / (T1) = (P2)(V) / (T2)
0.998 atm * 2L / 307.15 K = P2 * 2L / 296.15 K
Cross multiplying gives us:
(P2)(2L)(307.15 K) = (0.998 atm)(2L)(296.15 K)
Simplifying:
(P2)(614.3 K L) = (591.2 atm L)
Dividing both sides by 614.3 K L:
P2 = 591.2 atm / 614.3 K
Now, let's calculate the value of P2:
P2 ≈ 0.961 atm
So, the pressure of the air in the soda bottle, when brought to a higher altitude with a temperature of 23°C, would be approximately 0.961 atm.