Calculate the flask filled with stop is evacuated and weight its mean is found to be 134.567 it is them filled to a pressure of 735 mm at31c with is of UN non molecular mass and then the flask the filled with water and weight again its mass is now 1067.9g a summary that the gas is ideal calculate the molar mass of the gas.
Solution
Sorry, but I can't make sense of the question.
To calculate the molar mass of the gas, we need to use the ideal gas law equation:
PV = nRT,
where:
P = pressure of the gas (735 mmHg),
V = volume of the gas (in liters),
n = number of moles of gas,
R = ideal gas constant (0.0821 L·atm/(mol·K)),
T = temperature of the gas (31°C or 304 K).
First, let's find the number of moles of gas in the flask when it is filled to a pressure of 735 mmHg at 31°C:
To find the volume of gas (V), we need to convert the pressure (P) from mmHg to atm:
1 atm = 760 mmHg
P = 735 mmHg / 760 mmHg/atm = 0.967 atm
Now, rearrange the ideal gas law equation to solve for n:
n = (PV) / (RT)
Substituting the values we have:
n = (0.967 atm * V) / (0.0821 L·atm/(mol·K) * 304 K)
Next, we need to convert the given mass of the gas (134.567 g) to moles. To do this, we have to divide the mass by the molar mass of the gas (M):
n = mass (g) / molar mass (g/mol)
Now, let's consider the second part of the question:
The flask is filled with water and weighed again; its mass is now 1067.9 g. The mass of the gas (134.567 g) is no longer present, so the new mass is the mass of water (mH2O) and the mass of the flask (mFlask) combined.
Thus, the mass of water (mH2O) can be found by subtracting the mass of the empty flask (mFlask) from the new total mass (1067.9 g).
mH2O = 1067.9 g - mFlask
Now, we can calculate the molar mass of water (MH2O), knowing that it is made up of two hydrogen atoms (H) with a molar mass of 1 g/mol each, and one oxygen atom (O) with a molar mass of 16 g/mol:
MH2O = (2 * 1 g/mol) + 16 g/mol = 18 g/mol
Since the water and the gas occupy the same volume, we can equate the moles of the gas to the moles of water:
n = mH2O / MH2O
Now, we have two equations for n, which we can equate:
(mass of the gas) / (molar mass of the gas) = (mass of water) / (molar mass of water)
Plugging in the given values, we have:
134.567 g / (molar mass of the gas) = mH2O / 18 g/mol
Now, rearrange the equation to solve for the molar mass of the gas (molar mass of the gas = (mass of the gas) / (mH2O / 18 g/mol)):
molar mass of the gas = (134.567 g * 18 g/mol) / mH2O
Substituting mH2O = (1067.9 g - mFlask):
molar mass of the gas = (134.567 g * 18 g/mol) / (1067.9 g - mFlask)