Determine the molar mass of the following:
0.94g of a gas that occupies 500L at 0 degrees celcius and 1.00 (STP).
I keep getting 32g/mol
PV=nRT
n=mass/MM =PV/RT
MM=mass*RT/PV=.94*
so the volume for one mole at STP is 22.4 liters, so here you must have 500/22.4 moles which is almost 23 moles.
well, if .94 grams is 23 moles, this must be the a gas made up of quarks, or unknown matter much lighter than hydrogen. I wonder if you meant .5L?
If so, then .5/22.4 moles=about .022 moles, so .94g/.022moles equals about a molecular mass of about 42.7 grams.
Work this out exactly. But I wonder what the 500L volume should be, it is not 500L
you were right...the 500L should have been 500ml. Thanks for your help!!!
To determine the molar mass, we need to 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 ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the given conditions to the appropriate units. The volume is already in liters, the temperature needs to be converted to Kelvin, and the pressure needs to be converted to atm.
Given:
Mass of gas = 0.94 g
Volume of gas (V) = 500 L
Temperature (T) = 0 degrees Celsius = 273.15 K (conversion: K = °C + 273.15)
Pressure (P) = 1.00 atm
Now, we can rearrange the equation to find the number of moles (n):
n = PV / RT
Rearranging again, we can solve for the molar mass (M):
M = m / n
where m is the mass of the gas and n is the number of moles.
First, let's calculate the number of moles (n):
n = (P * V) / (R * T)
n = (1.00 atm * 500 L) / (0.0821 L * atm/(mol * K) * 273.15 K)
n ≈ 22.6 moles
Next, we can calculate the molar mass (M):
M = m / n
M = 0.94 g / 22.6 mol
M ≈ 0.0416 g/mol
Therefore, the molar mass of the gas is approximately 0.0416 g/mol, not 32 g/mol.