What is the volume of 0.100 g of C2H2F4
vapor at 1.09 atm and 43.9◦C?
Answer in units of L
YES(:
V=nRT/P
change 0.100g of C2H2F4 to moles n
change temp to kelvins
pressure units ok.
R=22.4L*1atm/1mole*273K=0.082 L*atm/mole*K
so then would it be (22.4)(.0821)(316.0) divided by 1.09? which is ultimately 534.671
it said that it was wrong
T is wrong. What's the 22.4? It doesn't belong there. Where is n? It belongs there. No surprise the data base gave you a thumbs down.
To find the volume of a gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles of the gas
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature of the gas (in Kelvin)
First, let's convert the given temperature from degrees Celsius (°C) to Kelvin (K). The conversion formula is:
T(K) = T(°C) + 273.15
Substituting the values, we get:
T(K) = 43.9 + 273.15 = 317.05 K
Next, calculate the number of moles (n) of the gas using the given mass and the molar mass of C2H2F4 (112.05 g/mol):
n = mass / molar mass
n = 0.100 g / 112.05 g/mol
Divide the mass by the molar mass of C2H2F4 to get the number of moles.
Once you have the number of moles, you can rearrange the ideal gas law equation to solve for volume (V):
V = (nRT) / P
Substitute the known values:
V = (n * R * T) / P
Calculate the volume using the given values: P = 1.09 atm, T = 317.05 K, and n from the previous step.
Finally, express the volume in liters (L) as required in the question.