.500 l of gas at STP is changed to 150c at the same volume. Whats the new pressure
PV = n R T
n R and V are constant here
P = (nR/V) T
or
P/T is constant
T initial = 273 Kelvin
Tfinal = 423 K
P/423 = Pstp/273
P = (1 atm or 10^5 Pascals)* (423/273)
the pressure is proportional to the absolute (Kelvin) temperature
(new pressure) / (old pressure) = (new temperature) / (old temperature)
To determine the new pressure of gas, we need to apply the ideal gas law equation, which states:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles of gas
R = Ideal gas constant
T = Temperature in Kelvin
In this case, we have the following information:
Initial volume (V1) = 0.500 L
Initial pressure (P1) = ? (to be determined)
Initial temperature (T1) = Standard Temperature and Pressure (STP) = 273 K
Final volume (V2) = 0.500 L (same as initial volume)
Final temperature (T2) = 150°C = 150 + 273 = 423 K
Since the volume and moles of gas are constant, we can simplify the ideal gas law equation to:
P1/T1 = P2/T2
Now, let's substitute the known values into the equation:
P1/273 K = P2/423 K
To find P2 (new pressure), we can rearrange the equation:
P2 = (P1 * 423 K) / 273 K
Now, we can plug in the values to calculate P2:
P2 = (P1 * 423) / 273
Since the volume remains constant, the pressure will have the same value. Therefore, the new pressure (P2) would be equal to the initial pressure (P1).
Hence, the new pressure of the gas is equal to the initial pressure.