I need help with this ideal gas law problem I know how to set the equation up but I'm not getting the correct answer.
How many moles of gas can be contained in a 1.44 L flask at 32Celsius and 93.5kPa?
It's easier for you to show your work and let us find the error.
ok so far I have
(0.9288atm)(1.44L)/(0.08206R)(305K)
are we supposed 2 divide something after we solve the equation
When I convert 93.5 kPa to atm I get
93.5 x (1 atm/101.325) = 0.9277.
The rest of the solution looks ok to me. I get an answer of 0.05309 = n and I would round that to 0.531 mols to three significant figures.
Ok I understand where the 0.9277 came from but when I put the equation in my calculator I keep getting 4965.218621
I made two typos. 93.5/101.325 = 0.92278
If you want to show each step I shall be happy to check it.
n = PV/RT
n = 0.92278*1.44/(0.08206*305)
That should give you 0.92278*1.44 = 1.3287.
Now divide by 0.08206 to give 16.19 and that divided by 305 = 0.0531
(The other typo was omitting the 0 on 0.0531 = n).
To solve this ideal gas law problem, we need to use the equation:
PV = nRT
Where:
P is the pressure of the gas in kPa,
V is the volume of the gas in liters,
n is the number of moles of gas,
R is the ideal gas constant (0.0821 L·atm/(mol·K)), and
T is the temperature of the gas in Kelvin.
First, let's convert the given temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 32°C + 273.15
T(K) = 305.15 K
Next, let's rearrange the ideal gas law equation to solve for the number of moles, n:
n = PV / RT
Now, let's plug in the values:
P = 93.5 kPa
V = 1.44 L
R = 0.0821 L·atm/(mol·K)
T = 305.15 K
n = (93.5 kPa * 1.44 L) / (0.0821 L·atm/(mol·K) * 305.15 K)
Simplifying further:
n = (134.64 kPa·L) / (25.083065 L·atm/(mol·K))
n = 5.36 mol
Therefore, there are 5.36 moles of gas in the 1.44 L flask at a temperature of 32°C and a pressure of 93.5 kPa.