Homework #1 Based on the type or types of intermolecular force, predict the substance in each...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅K respectively. A) How much heat is required to convert 30.5 g of ethanol at 30 ∘C to the vapor phase at 78 ∘C? Q=______kJ B)How much heat is required to convert 30.5 g of ethanol at -167 ∘C...
10. (14 pts) For the compounds below: a. Identify the strongest intermolecular force present in each molecule. b. Arrange the following molecules in order of lowest vapor pressure to highest vapor pressure. c. Briefly justify your answer to part b using your knowledge of intermolecular forces. Molecule * HH * Strongest Intermolecular Force: Lowest vapor pressure: < < Highest vapor pressure 11.(12 pts) Ethanol (CH-OH, FW-46.08 g/mol) melts at -114 °C and boils at 78 °C. How much heat is...
Ethanol melts at 159K and boils at 351K. The enthalpy of fusion is 5.02 kJ/mol, the enthalpy of vaporization is 35.56 kJ/mol, and the molar mass is 46.07 g/mol. The specific heats of solid ethanol is 0.97 J/g-K, for liquid ethanol it is 2.3 J/g-K, and for gaseous ethanol it is 1.9 J/g-K. How much heat (kJ) is needed to convert 215 g of liquid ethanol at 160 K to gaseous ethanol at 713 K?
What are the differences between liquids and solids? b. What are the differences between liquids and gases? Define briefly: boiling point melting point What is the difference between a nomadic liquid crystal and a sematic A liquid crystal? Ethanol (C_2H_5OH) Delta H_vap =38.56 kJ/mol. Delta H_fus= 5.02kJ/mol, Boiling point = 78degree C, melting point = -114 degree C Specific heat of solid ethanol = 0.97J/g-K, specific heat of liquid ethanol = 2.3J/g-K How much heat does it take to convert...
6. Shown below is the heating curve for a substance. The five segments of the heating curve are labeled A-E 130 100 T (°C) heat added (kJ) I. ndicate the phases of matter present when the substance is at each point (A-E) on the heating curve For this substance, which phase of matter has the largest heat capacity? How can you tell? In what state of matter would this substance exist at room temperature? How can you tell? IV. In...
1. Rank these substances in order of increasing noncovalent intermolecular attractions. For each substance, name the types of intermolecular attractions that occur. A) CH.CH2CHCH B) CH.CH C) CH,CH2CH2OH D) CH,CHOCH 2. The chlorofluorocarbon CC13F has a vaporization enthalpy of 24.8 kJ/mol. Calculate the heat energy transfer required to vaporize 1.0 kg of the compound.