One mole of an ideal gas is sealed in a 22.4- container at a pressure of 1 and a temperature of 273 . The temperature is then increased to 305 , but the container does not expand. What will the new pressure be?
If v is constant...
P1/T1=P2/T2 Solve for P2.
thank you. i tried doing that and i got 25.02, which is wrong, im not sure what im doing wrong..
You are not using p1 as 1 atm, which is given. You put the volume in for P1.
yes that is what i did i multiplied 22.4 times 305 divided by 273 and i got it wrong
C,mon.
P1 = 1
T1 = 273 (I guess that K, you don't say).
P2 = ??
T2 = 305 Kelvin?
Bob Pursley told you you can't use volume of 22.4 for pressure. Pressure is 1 in the problem.
To find the new pressure, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal Gas Constant
T = Temperature
Since the volume is constant and the number of moles remains the same, we can rearrange the equation as follows:
P₁V₁ = P₂V₂
Where:
P₁ = Initial pressure
V₁ = Initial volume
P₂ = New pressure
V₂ = Volume remains the same
Given:
P₁ = 1 atm
V₁ = 22.4 L
T₁ = 273 K
T₂ = 305 K
Using the relationship P₁V₁ = P₂V₂ and plugging in the given values:
1 atm * 22.4 L = P₂ * 22.4 L
Simplifying the equation:
22.4 atm = P₂ * 22.4 L
Now, we solve for P₂:
P₂ = (1 atm * 22.4 L) / 22.4 L
P₂ = 1 atm
Therefore, the new pressure will be 1 atm.