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------------------------------------------------ What is the volume of 92.4 g of chlorine gas at a temperature of 46ºC and a pressure of 694 mm Hg, assuming ideal behavior?

Options:
- Option 1: 3.25 L
- Option 2: 4.50 L
- Option 3: 1.67 L
- Option 4: 2.92 L

To calculate the volume of a gas, we use the ideal gas law equation PV = nRT. However, we need more information, such as the number of moles or the molar mass of chlorine gas, to directly calculate the volume.

Explanation:

To calculate the volume of a gas, we can use the ideal gas law equation, which is PV = nRT. In this equation, P represents the pressure, V represents the volume, n represents the number of moles of the gas, R is the gas constant, and T represents the temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin. To do this, we add 273.15 to the Celsius temperature. So, 46ºC + 273.15 = 319.15 K.

We also need to convert the pressure from mm Hg to atm. 1 atm is equivalent to 760 mm Hg. Therefore, 694 mm Hg ÷ 760 mm Hg/atm = 0.91316 atm.

Now we can rearrange the ideal gas law equation to solve for volume. V = (nRT) / P.

Since the question doesn't provide the number of moles of chlorine gas, we cannot directly calculate the volume. We would need more information, such as the number of moles or the molar mass of chlorine gas.

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