A 337.2 g sample of acetone gas with a temperature of 56.0°C is converted to a liquid with a temperature of 56.0°C. How much heat is involved?

What quantity of heat (in J) would be required to convert 6.91 mol of a pure substance from a liquid at 40.0 °C to a gas at 113.0 °C? + Cliquid = 1.45 J/mol °C Tboiling = 88.5 °C Cgas = 0.65 J/mol•°C AHvaporization = 1.23 kJ/mol

How much heat would be required to convert 5.31 mol of a pure substance from a liquid at 40.0°C to a gas at 113.0°C?

Based on the thermodynamic properties provided for methanol (below), select from the following list the equation(s) necessary to calculate the amount of energy needed for 5.0 kg of methanol to go from -64°C to 88°C. Property Value Units Melting point -94 °C Boiling point 65 °C AHfus 3.18 kJ/mol AHvap 37 kJ/mol 615) 48.7 J/mol.°C Cp (1) 81.1 J/mol.°C 5 (8) 43.8 J/mol °C Choose one or more: A. q = n(43.8 J/mol °C)AT, where AT is negative B. q=n(48.7 J/mol ·°C)AT, where AT is negative C. q= n(81.1 J/mol -°C)AT, where A Tis negative D. q = n(43.8 J/mol °C)AT, where A Tis positive E. q=n(-3.18 kJ/mol) F. q- n(37 kJ/mol) G. q=n(-37 kJ/mol) H. q- n(3.18 kJ/mol) 1.q=n(48.7 J/mol °C)AT, where AT is positive J.q=n(81.1 J/mol °C)AT, where A Tis positive