Final answer:
According to Dalton's law of partial pressure, the total pressure in a mixture of gases is equal to the sum of the partial pressures of the individual gases. To find the partial pressure of argon gas in the tank, we need to subtract the partial pressure of hydrogen gas from the total pressure. The partial pressure of argon gas in the tank is 522.6 mmHg.
Step-by-step explanation:
According to Dalton's law of partial pressure, the total pressure in a mixture of gases is equal to the sum of the partial pressures of the individual gases. In this case, the total pressure of the gas tank is 745.0 mmHg. To find the partial pressure of argon gas, we need to subtract the partial pressure of hydrogen gas from the total pressure.
To do this, we need to convert the mass of each gas to moles. The molar mass of hydrogen gas (H₂) is approximately 2 g/mol, so the number of moles of hydrogen gas is 0.6048 g / 2 g/mol = 0.3024 mol. The molar mass of argon gas (Ar) is approximately 40 g/mol, so the number of moles of argon gas is 15.9800 g / 40 g/mol = 0.3995 mol.
Now we can calculate the partial pressure of argon gas using the mole fraction of argon gas in the mixture. The mole fraction of argon gas is the number of moles of argon gas divided by the total number of moles of gas (0.3024 mol + 0.3995 mol = 0.7019 mol). The partial pressure of argon gas is the mole fraction of argon gas multiplied by the total pressure of the gas tank: 0.7019 * 745.0 mmHg = 522.6 mmHg. Therefore, the partial pressure of argon gas in the tank is 522.6 mmHg.