A sample of metallic element X, weighing 4.315 g, combines with 0.4810 L of Cl2 gas (at normal pressure and 20.0¢ªC) to form the metal chloride with the formula XCl. If the density of Cl2 gas under these conditions is 2.948 g/L, what is the mass of the chlorine? The atomic weight of the chlorine is 35.453 amu. What is the atomic weight of X? what is the identity of X
See your post above.
To find the mass of chlorine, we first need to calculate the number of moles of Cl2 gas using the given volume and density.
Step 1: Calculate the mass of Cl2 gas.
Mass of Cl2 gas = density × volume
Mass of Cl2 gas = 2.948 g/L × 0.4810 L
Mass of Cl2 gas = 1.4172 g
Step 2: Calculate the number of moles of Cl2 gas.
Number of moles of Cl2 gas = mass / molar mass
Number of moles of Cl2 gas = 1.4172 g / 35.453 g/mol
Number of moles of Cl2 gas = 0.0400 mol (approximately)
Since the reaction between X and Cl2 gas has a 1:1 mole ratio, this means that the number of moles of X is also 0.0400 mol.
Step 3: Calculate the atomic weight of X.
Atomic weight of X = mass of X / number of moles of X
Atomic weight of X = 4.315 g / 0.0400 mol
Atomic weight of X = 107.875 g/mol
So, the atomic weight of X is approximately 107.875 g/mol.
The identity of X cannot be determined from the given information.