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3. (a) Derive the integrated form of Clausius-Clapeyron equation applicable to vaporization, lnleft(frac{p_2}{p_1} ight) = frac{Delta H_{ ext{vap}}}{R}left(frac{1}{T_1} - frac{1}{T_2} ight), (this equation relates the vapor pressures of liquid p1 and p2 at temperatures T1 and T2, respectively) by starting from the differential form that we obtained in class: frac{dln p}{dT} = frac{Delta H_{ ext{vap}}}{RT^2} (b) The vapor pressure of a substance at 20 °C is 58.0 kPa and its enthalpy of vaporization is 32.7 kJ mol?¹. Estimate the temperature at which its vapor pressure is 66.0 kPa. NOTE: Do not confuse the vapor pressure with the atmospheric pressure. If at temperature T the vapor pressure is p then the liquid and vapor are in equilibrium at those temperature and pressure. If the atmospheric pressure p_atm is greater than the vapor pressure p then the liquid will not be boiling. Only when p_atm = p, the liquid will be at its boiling point.

          3. (a) Derive the integrated form of Clausius-Clapeyron equation applicable to vaporization,
lnleft(frac{p_2}{p_1}
ight) = frac{Delta H_{	ext{vap}}}{R}left(frac{1}{T_1} - frac{1}{T_2}
ight),
(this equation relates the vapor pressures of liquid p1 and p2 at temperatures T1 and T2, respectively) by starting from the differential form that we obtained in class:
frac{dln p}{dT} = frac{Delta H_{	ext{vap}}}{RT^2}
(b) The vapor pressure of a substance at 20 °C is 58.0 kPa and its enthalpy of vaporization is 32.7 kJ mol?¹. Estimate the temperature at which its vapor pressure is 66.0 kPa. NOTE: Do not confuse the vapor pressure with the atmospheric pressure. If at temperature T the vapor pressure is p then the liquid and vapor are in equilibrium at those temperature and pressure. If the atmospheric pressure p_atm is greater than the vapor pressure p then the liquid will not be boiling. Only when p_atm = p, the liquid will be at its boiling point.

$3. (a) Derive the integrated form of Clausius-Clapeyron equation applicable to vaporization, lnleft(fracp2p1 ight) = fracDelta H extvapRleft(frac1T1 - frac1T2 ight), (this equation relates the vapor pressures of liquid p1 and p2 at temperatures T1 and T2, respectively) by starting from the differential form that we obtained in class: fracdln pdT = fracDelta H extvapRT^2 (b) The vapor pressure of a substance at 20 °C is 58.0 kPa and its enthalpy of vaporization is 32.7 kJ mol?¹. Estimate the temperature at which its vapor pressure is 66.0 kPa. NOTE: Do not confuse the vapor pressure with the atmospheric pressure. If at temperature T the vapor pressure is p then the liquid and vapor are in equilibrium at those temperature and pressure. If the atmospheric pressure patm is greater than the vapor pressure p then the liquid will not be boiling. Only when patm = p, the liquid will be at its boiling point.$

Added by Catalina R.

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