A rigid container holds hydrogen gas at a pressure of 3.0 atm and a temperature of 20 degrees Celsius. What will the pressure be if the temperature is lowered to -33 degrees Celsius? Please give your final answer in atm.
Answer
You can use the gas laws
P1/T1 = P2/T2
You have to use degrees Kelvin
Change C to K by adding 273.
P1/T1 = P2/T2
P1 = 3.0 ATM
T1 = 20+273 = 293K
P2 = ?
T2 = -33+273=240
3.0/293 = P2/240
P2 =(3.0/293)*240
P2 = 2.457337
= 2.46 ATM
I don't know the answer but you TOTALLY must be in my physics class haha. Physics for Life Science?
Yas
Well, if the container gets colder, we might need to bring in some penguins to keep it company. 🐧 But let's focus on the question!
To find the new pressure, we can use the ideal gas law equation:
PV = nRT
Since the volume of the container is rigid, it stays constant, so we can rewrite the equation as:
P1/T1 = P2/T2
Where P1 is the initial pressure, T1 is the initial temperature, P2 is the final pressure, and T2 is the final temperature.
Plugging in the given values, we have:
3.0 atm / (20 + 273) K = P2 / (-33 + 273) K
Simplifying this equation, we find:
3.0 atm * (-33 + 273) K = P2 * (20 + 273) K
Now, let's do some calculations and have some fun with numbers!
P2 = (3.0 atm * (-33 + 273) K) / (20 + 273) K
P2 = (3.0 atm * 240 K) / 293 K
P2 ≈ 2.452 atm
So, the final pressure will be approximately 2.452 atm. Enjoy the new temperature, and maybe invite a frozen clown to the party! 🤡❄️
To solve this problem, we need to use the Ideal Gas Law, which states that:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature in Kelvin
To convert the temperature from Celsius to Kelvin, we use the equation:
T(K) = T(°C) + 273.15
First, let's convert the initial temperature of 20 degrees Celsius to Kelvin:
T1 = 20 + 273.15 = 293.15 K
Next, let's convert the final temperature of -33 degrees Celsius to Kelvin:
T2 = -33 + 273.15 = 240.15 K
Since the volume and the number of moles are constant, we can rewrite the Ideal Gas Law as:
P1/T1 = P2/T2
Now, let's plug in the given values:
P1 = 3.0 atm
T1 = 293.15 K
T2 = 240.15 K
3.0 atm / 293.15 K = P2 / 240.15 K
To solve for P2, we need to cross-multiply and divide:
P2 = (3.0 atm) * (240.15 K) / 293.15 K
P2 ≈ 2.455 atm
Therefore, the pressure will be approximately 2.455 atm when the temperature is lowered to -33 degrees Celsius.