Chlourine monoxide reacts with flourine gas to give a new unknown gas that contains Cl, O and F. In an experiment you find that 0.15476 g of the new gas has a preasure of 17mmHg ina 1850 mo flak at 21ºC. What is thd identity of the unknown gas?
To determine the identity of the unknown gas, we need to calculate the number of moles present. We can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure (17 mmHg)
V = volume (1850 mL or 1.85 L)
n = number of moles
R = Ideal Gas Constant (0.0821 L·atm/(K·mol))
T = temperature in Kelvin (21ºC + 273.15 = 294.15 K)
Rearranging the equation to solve for n, we have:
n = PV / RT
Substituting the given values:
n = (17 mmHg * 1.85 L) / (0.0821 L·atm/(K·mol) * 294.15 K)
n ≈ 0.1426 moles
Now that we know the number of moles, we can calculate the molar mass of the unknown gas using the given mass of 0.15476 g:
Molar mass = mass / moles
Molar mass ≈ 0.15476 g / 0.1426 moles
Molar mass ≈ 1.085 g/mol
The molar mass approximately equals 1.085 g/mol. Now, we need to determine the possible constituents of the gas. Since the unknown gas is formed from the reaction of chlorine monoxide (Cl2O) and fluorine gas (F2), we need to determine which combination of elements can yield a molar mass close to 1.085 g/mol.
By analyzing the possible combinations, we find that the only plausible combination is ClOF, which has a molar mass of approximately 1.085 g/mol. Therefore, the identity of the unknown gas is ClOF (chlorine monoxide fluoride).