The vapor pressure of ethanol is 115 torr at 34.9°C. If the [tex]\Delta H_{\text{vap}}[/tex] of ethanol is 38.6 kJ/mol, calculate the temperature (°C) when the vapor pressure is 760 torr.

The Clausius-Clapeyron Equation is used to find the temperature when the vapour pressure of ethanol is 760 torr. By substituting known quantities into the equation, we can derive that the temperature is around 78.51°C.

Explanation:

You can use the Clausius-Clapeyron Equation which is ln(P2/P1) = −ΔHvap/R * (1/T2 - 1/T1), where P1 and T1 are the known pressure and temperature, P2 is the pressure when we want to find the corresponding temperature (T2, which is what we want to find), and ΔHvap is the heat of vaporization. R equals 8.3145 J/(mol K) or 62.36 L torr / (mol K).

Plugging the known values into Clausius-Clapeyron Equation, ln(760/115) = -38600J/(8.3145 J/(molK) * (1/T2 - 1/(34.9 + 273.15)), after solving it algebraically, we get T2 = 351.66K, or T2 = 78.51°C approx.

Learn more about Clausius-Clapeyron Equation here:

https://brainly.com/question/33369944

#SPJ11