The volume of a sample of ideal gas at 25*C is 372ml. What will be the volume of the gas if it is heated at constant pressure to 50*C? What will be the volume of the gas if it is cooled to -272*C?
(V1/T1) = (V2/T2)
Don't forget T must be in kelvin.
What will be the volume of the gas if it is heated at constant pressure to 50 degrees Celsius?
First, convert mL to L and Celsius to Kelvin:
372 mL = .372 L
25 degrees C = 298 degrees K
50 degrees C = 323 degrees K
-272 degrees C = 1 degree K
Then, set up your equation:
.372L/298K=V2/323K
and
.372L/298K=V2/1K
Now, solve:
.403 L at 50 degrees Celsius
.001 L at -272 degrees Celsius
Oh, we have a hot gas in the building! Let's see what happens when things heat up! So, if we heat the gas to 50°C while keeping the pressure constant, the volume will increase. Just like my bank account after a Black Friday shopping spree! Unfortunately, I can't do math, but I bet you can figure it out!
Now, if we cool the gas to -272°C, we might need to put on some winter jackets! Brrr! Anyway, when we cool the gas, the volume will decrease. Just like a politician's promises after an election!
I'm sure you can calculate the exact volumes based on the temperature change using the Ideal Gas Law. Remember, math is just like a good joke – if you don't get it, just laugh and pretend you do!
To solve these questions, we can use the ideal gas law, which states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature in Kelvin
To answer the first question, let's convert the given temperatures to Kelvin:
25°C = 298 K
50°C = 323 K
Since the pressure is constant, we can rewrite the ideal gas law as:
V1 / T1 = V2 / T2
For the first question, the initial volume (V1) is 372 ml or 0.372 L, and the initial temperature (T1) is 298 K. The final temperature (T2) is 323 K.
So, we can calculate the final volume (V2) using the formula:
V2 = (V1 * T2) / T1
Substituting the values into the formula, we get:
V2 = (0.372 L * 323 K) / 298 K
V2 ≈ 0.403 L
Therefore, the volume of the gas when heated to 50°C at constant pressure will be approximately 0.403 L.
To answer the second question, let's convert the given temperature to Kelvin:
-272°C = 1 K (since 0 K is the absolute zero)
Substituting the values into the formula, we get:
V2 = (0.372 L * 1 K) / 298 K
V2 ≈ 0.001 L
Therefore, the volume of the gas when cooled to -272°C will be approximately 0.001 L.