volume of 8.00 grams of hydrogen gas at 32.0 degrees celcius and 1.50 atm
That is 3.97 moles of H2 gas. I assume that you know where that came from. I used 1.008 amu for the mass of an H atom. Each H2 molecule has two of them.
Call 3.97 "n" and use the ideal gas law
P V = n R T
where T = 305 K
You should look up and memorize the appropriate value of R. If you want P to be in atm,
R = 0.08206 l-atm/mole-K
OR remember that 1 mole of a gas at 1 atm and 273K (0 C) has a volume of 22.4 l. Your volume per mole be higher because i gets multiplied by a factor 305/273 because of the higher temperature.
15.2g
This question is quite simple if you really think about it. well lets see what the problem is asking you to do.
I did the work and the answer always seems to come as 15.2g
So the answer is definitely 15.2g
What is a mole?
To find the volume of a gas, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, let's convert the temperature from Celsius to Kelvin. To do this, we add 273.15 to the Celsius temperature.
T = 32.0°C + 273.15 = 305.15 K
Since we are given the pressure (P = 1.50 atm), we need to find the number of moles (n) of hydrogen gas. To find the number of moles, we use the molar mass of hydrogen.
The molar mass of hydrogen (H₂) is 2.016 g/mol.
n = mass / molar mass
n = 8.00 g / 2.016 g/mol ≈ 3.968 mol
Now, we have all the necessary information to calculate the volume (V). Rearranging the ideal gas law equation, we have:
V = (nRT) / P
Substituting the values:
V = (3.968 mol × 0.0821 L·atm/(mol·K) × 305.15 K) / 1.50 atm
Calculating this expression will give the volume of the hydrogen gas in liters.