Final answer:
The question asks for the partial pressure of Cl2 in a gas mixture at specific temperature and total pressure but lacks the necessary information on the composition of the mixture to calculate the partial pressure.
Step-by-step explanation:
The question asks about the partial pressure of Cl2(g) in a gaseous mixture at 1.00°C and 5.00 atm. However, the question seems incomplete, missing the percentage composition of Cl2 in the gaseous mixture, which is essential to calculate its partial pressure. If we had the mole fraction or percentage of Cl2 in the mixture, we could use Dalton's Law of Partial Pressures to calculate the partial pressure of Cl2.
Dalton's Law states that the total pressure of a mixture of gases is equal to the sum of the individual partial pressures of each gas in the mixture. The partial pressure is calculated by multiplying the total pressure by the mole fraction of the gas in the mixture:
Partial Pressure = Total Pressure × Mole Fraction of the Gas
Without additional information, it is not possible to provide the exact value of the partial pressure of Cl2 in the given mixture.