When an evacuated glass bulb at 75.0 ml volume is filled with a gas at 25.3 degrees C and 747 mm Hg, the bulb gains 0.0114g. The gas is?

Use PV = nRT and solve for n.

Then n = grams/molar mass. Solve for molar mass. You can identify the gas from the periodic table. By the way, do you know the possibilities? There are not very many gases in the periodic table. H2, N2, O2, F2, Cl2, + noble gases.

the possibilities could be He F2 O2 N2 and NE the correct answer would be F2

I don't think the correct answer is F2.

To determine the gas, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure in atmospheres (convert mm Hg to atm)
V = volume in liters (convert ml to liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin (convert degrees Celsius to Kelvin)

First, let's convert the given values to the appropriate units:

Volume (V) = 75.0 ml = 0.075 L
Pressure (P) = 747 mm Hg = 747/760 atm (since 1 atmosphere = 760 mm Hg)
Temperature (T) = 25.3 + 273.15 = 298.45 K

Now we can rearrange the ideal gas law equation to solve for the number of moles (n):

n = PV / RT

Substituting the values we have:

n = (0.075 L) * (747/760 atm) / (0.0821 L·atm/(mol·K)) * (298.45 K)

Simplifying the equation, we can cancel out units:

n = (0.075) * (747/760) / (0.0821 * 298.45)

n = 0.9204 / 24.4817

n ≈ 0.0376 moles

Now that we have the number of moles, we can find the molar mass of the gas by dividing the mass gained by the number of moles:

Molar mass (g/mol) = mass gained / number of moles

Given that the bulb gains 0.0114 g:

Molar mass ≈ 0.0114 g / 0.0376 moles

Molar mass ≈ 0.303 g/mol

To determine the gas, we need to check the molar mass against the periodic table and look for a gas with a molar mass close to 0.303 g/mol. In this case, the closest match is the gas ammonia (NH₃), which has a molar mass of approximately 17 g/mol.

Therefore, the gas is ammonia (NH₃).