A 25-liter sample of steam at 100^circ C and 1.0 atm is cooled to 25^circ C and expanded until the pressure is 19.71 mm Hg. If no water condenses, calculate the final volume of the water vapor. 1.3times 10^-3L 1.0 L 240L 770 L

To solve this problem, we can use the Ideal Gas Law, which is given by: where:- is the pressure,- is the volume,- is the number of moles,- is the ideal gas constant (0.0821 L·atm/(mol·K)),- is the temperature in Kelvin.First, let's convert all the given values to appropriate units and calculate the initial number of moles of steam.Initial conditions:- Volume ( ) = 25 L- Temperature ( ) = = K- Pressure ( ) = 1.0 atmUsing the Ideal Gas Law to find the number of moles ( ): Now, let's use the final conditions to find the final volume ( ):Final conditions:- Temperature ( ) = = K- Pressure ( ) = 19.71 mm Hg = atm = 0.02594 atmUsing the Ideal Gas Law again to find the final volume ( ): Therefore, the final volume of the water vapor is approximately 770 L.The correct answer is:770 L