Cyanogen (C2N2 Hvap=23.3 kJ/mol) has a normal boiling point of -21.2C. At what temperature in C, will the vapor pressure of liquid cyanogen be 0.1000atm?
a. -294
b. -21.1
c. 44.6
d. -272
e. -64.3
Cyanogen (C2N2 Hvap=23.3 kJ/mol) has a normal boiling point of -21.2C. At what temperature in C,...
Chloroform has a normal boiling point of 61°C and a Hvap of 29.6 kJ/mol. Determine the vapor pressure (in atm) of chloroform at 35°C. Give you answer to decimal places
The normal boiling point of a liquid is 282 °C. At what temperature (in °C) would the vapor pressure be 0.4 atm? (∆Hvap = 28.5 kJ/mol)
Acetic acid has a normal boiling point of 118 ?Cand a ?Hvap of 23.4 kJ/mol. Part A What is the vapor pressure (in mmHg) of acetic acid at 35 ?C? Express your answer using three significant figures.
Methanol has a normal boiling point of 64.6 °C at 760 torr. The △Hvap = 35.2 kJ/mol. What is the vapor pressure of methanol at 12.0 °C? ln (P2P1) = −△HvapR (1T2 − 1T1)R = 8.314 J /mol⋅K
HI has a normal boiling point of −36°C, and its ∆Hvap is 22.18 kJ/mol. Calculate the molar entropy of vaporization (∆Svap).
What is the vapor pressure of a liquid at 319.93 K if its ∆Hvap = 28.9 kJ/mol and its normal boiling point is 341.88 K?
The molar enthalpy of vaporization of NH3 is 23.3 kJ/mol at its normal boiling point of -33.3 °C. How much energy is required to evaporate 2.03 kg of ammonia at -33.3 °C?
The molar enthalpy of vaporization of liquid nh4 is 23.5 kJ/mol, and it’s normal boiling point is -33.4 C. What is the vapor pressure of ammonia at-21.5C
The normal boiling point of ammonia is -33.3°C, and its enthalpy of vaporization is 23.35 kJ/mol. Calculate the temperature in °C required to double the vapor pressure of ammonia.
A liquid has a ΔH o vap of 31.1 kJ/mol and a boiling point of 135°C at 1 atm. What is its vapor pressure at 106°C?