To identify a diatomic gas (X_2), a researcher carried out the following experiment: She weighed an empty 1.00-L bulb, then filled it with the gas at 1.10atm and 23.0 degrees celsius and weighed it again. The difference in mass was 1.27g . Identify the gas.
Express your answer as a chemical formula.
Sorry about that.
Use the equation I gave you before for calculating the density of a gas. You have the density given as 1.27 g/L. Calculate molar mass and divide by 2. Post your work if you need additional assistance.
I got C2H4?
How did you get C2H4? Show your work and I'll try to find the error.
jus give us the damn answer u stupid head!
The answer is N2, but your rude behavior is uncalled for.
No problem! To identify the gas, we need to calculate its molar mass and then determine its chemical formula.
First, we need to convert the mass difference to moles of the gas. The ideal gas law can be used for this calculation:
PV = nRT
Where:
P = pressure in atm
V = volume in liters
n = number of moles
R = ideal gas constant (0.08206 L·atm/K·mol)
T = temperature in Kelvin
Let's convert the given values:
P = 1.10 atm
V = 1.00 L
R = 0.08206 L·atm/K·mol
T = (23.0 + 273.15) K (converting Celsius to Kelvin)
Now we can solve for n:
n = PV / RT
Substituting the values:
n = (1.10 atm * 1.00 L) / (0.08206 L·atm/K·mol * (23.0 + 273.15) K)
Calculating this, we find:
n ≈ 0.046 mol
Next, we need to calculate the molar mass of the gas. We do this by dividing the mass difference by the moles:
Molar mass = mass difference (g) / moles
Substituting the values:
Molar mass = 1.27 g / 0.046 mol
Calculating this, we find:
Molar mass ≈ 27.6 g/mol
Now, we need to find the diatomic gas whose molar mass is approximately 27.6 g/mol. Checking the periodic table, we can see that the only diatomic gas with a molar mass close to this value is oxygen gas (O2).
Therefore, the identity of the gas is oxygen gas, which is represented by the chemical formula O2.