39.9 liters of hydrogen are collected over water at 76.0°C and have a pressure of 439 torr. What would the pressure (in torr) of the 'dry' hydrogen at 29.4°C in an 18.5 liter container be? (Water Vapor Pressure at 76.0°C is 301.4 torr)

Apply the Combined Gas Law to find the new pressure of the dry hydrogen at 29.4°C in an 18.5 liter container. The Combined Gas Law is \( \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \), where \( P_1 \) and \( V_1 \) are the initial pressure and volume, \( T_1 \) is the initial temperature in Kelvin, and \( P_2 \), \( V_2 \), and \( T_2 \) are the final conditions.

Convert the temperatures from Celsius to Kelvin: \( T_1 = 76.0 + 273.15 \) and \( T_2 = 29.4 + 273.15 \).