1.4 mol of gas at a temperature of -170 degreed celcius fills a 2.9 L container.
what is the gas pressure?
PV=nRT
solve for P change temp to K,
as a check, at STP you would have for 1.4 mols, (22.4*1.4)=about 30 liters
that is at temp 273K, your temp is (-170+273=about 100K) so you should have then 30*/2.7 liters or 12 liters about at standard pressure. But you have 2.7liters, so pressure= 12/2.7 =about 4 atmospheres
so do your calc, and it should be about 4 atm.
thank you i really appreciate it
To determine the gas pressure, you can use the ideal gas law equation:
PV = nRT
Where:
P = gas pressure
V = volume of the gas (in liters)
n = amount of substance (in moles)
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in kelvin)
First, let's convert the temperature from Celsius to Kelvin by adding 273.15 to it:
T = -170 + 273.15 = 103.15 K
Now we can substitute the given values into the equation:
PV = nRT
P * 2.9 = 1.4 * 0.0821 * 103.15
P * 2.9 = 11.12362
Now, rearranging the equation to solve for P:
P = 11.12362 / 2.9
P ≈ 3.84 atm
Therefore, the gas pressure is approximately 3.84 atm.