Help me solve this question please with clausius clapeyron equation

Ethanol, with Hvap - 40.5 kJ mol has a higher Hvap than methanol, which is 35.2 kJ molt due to its larger size and greater intermolecular forces. Because the AH van for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3C, what would the temperature be when the vapor pressure is 5.00 atm? The temperature will be i K. e Textbook and Media Hint Assistance Used Ethanol, with Hvap - 40.5 kJ mol has a higher Hvap than methanol, which is 35.2 kJ molt due to its larger size and greater intermolecular forces. Because the AH van for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3C, what would the temperature be when the vapor pressure is 5.00 atm? The temperature will be i K. e Textbook and Media Hint Assistance Used