The change in enthalpy of sublimation has to be calculated. The portion of intermolecular forces in ice that account for the formation of hydrogen bonding has to be estimated. Concept Introduction: Enthalpy is heat content of the system. The value of enthalpy does not depend on the path of a reaction but depend on state of the system. It has a unique value for each state of the system. Thus, enthalpy is a state function. Enthalpy change, denoted by ΔH , refers to heat evolved or absorbed during a reaction. If heat is evolved in the reaction that is exothermic reaction ΔH has negative value. For an endothermic reaction, ΔH has positive value. ΔH can be represented as, ΔH = ΔE + PΔV where, ΔH = Change in enthalpy ΔE = Change in Internal energy ΔV = Change in volume P = Pressure Enthalpy of sublimation is denoted by ΔH sub . It is the enthalpy involved in sublimation process. Internal energy of a system is total energy present in the system. In simple words, it is the sum of kinetic and potential energy of the particles in the system. According to First law of Thermodynamics , Energy of a system is conserved. It is only transferred from one state to another that is from system to surroundings and vice versa. So ΔE can be represented as, ΔE universe = ΔE sys + ΔE surroundings Further, ΔE is also equivalent to sum of either heat gained or lost and either work done on the system or by the system. ΔE = q + w where ΔE = change in internal energy q = quantity of heat gained or heat lost w = work done
The change in enthalpy of sublimation has to be calculated. The portion of intermolecular forces in ice that account for the formation of hydrogen bonding has to be estimated. Concept Introduction: Enthalpy is heat content of the system. The value of enthalpy does not depend on the path of a reaction but depend on state of the system. It has a unique value for each state of the system. Thus, enthalpy is a state function. Enthalpy change, denoted by ΔH , refers to heat evolved or absorbed during a reaction. If heat is evolved in the reaction that is exothermic reaction ΔH has negative value. For an endothermic reaction, ΔH has positive value. ΔH can be represented as, ΔH = ΔE + PΔV where, ΔH = Change in enthalpy ΔE = Change in Internal energy ΔV = Change in volume P = Pressure Enthalpy of sublimation is denoted by ΔH sub . It is the enthalpy involved in sublimation process. Internal energy of a system is total energy present in the system. In simple words, it is the sum of kinetic and potential energy of the particles in the system. According to First law of Thermodynamics , Energy of a system is conserved. It is only transferred from one state to another that is from system to surroundings and vice versa. So ΔE can be represented as, ΔE universe = ΔE sys + ΔE surroundings Further, ΔE is also equivalent to sum of either heat gained or lost and either work done on the system or by the system. ΔE = q + w where ΔE = change in internal energy q = quantity of heat gained or heat lost w = work done
Solution Summary: The author explains that the change in enthalpy of sublimation has to be calculated and the portion of intermolecular forces that account for the formation of hydrogen bonding is estimated.
Science that deals with the amount of energy transferred from one equilibrium state to another equilibrium state.
Chapter 10, Problem 143CP
Interpretation Introduction
Interpretation:
The change in enthalpy of sublimation has to be calculated.
The portion of intermolecular forces in ice that account for the formation of hydrogen bonding has to be estimated.
Concept Introduction:
Enthalpy is heat content of the system. The value of enthalpy does not depend on the path of a reaction but depend on state of the system. It has a unique value for each state of the system. Thus, enthalpy is a state function.
Enthalpy change, denoted by
ΔH, refers to heat evolved or absorbed during a reaction. If heat is evolved in the reaction that is exothermic reaction
ΔH has negative value. For an endothermic reaction,
ΔH has positive value.
ΔH can be represented as,
Enthalpy of sublimation is denoted by
ΔHsub. It is the enthalpy involved in sublimation process.
Internal energy of a system is total energy present in the system. In simple words, it is the sum of kinetic and potential energy of the particles in the system. According to First law of Thermodynamics, Energy of a system is conserved. It is only transferred from one state to another that is from system to surroundings and vice versa. So
ΔE can be represented as,
ΔEuniverse=ΔEsys+ΔEsurroundings
Further,
ΔE is also equivalent to sum of either heat gained or lost and either work done on the system or by the system.
1) a) Give the dominant Intermolecular Force (IMF) in a sample of each of the following
compounds. Please show your work. (8) SF2, CH,OH, C₂H₂
b) Based on your answers given above, list the compounds in order of their Boiling Point
from low to high. (8)
19.78 Write the products of the following sequences of reactions. Refer to your reaction road-
maps to see how the combined reactions allow you to "navigate" between the different
functional groups. Note that you will need your old Chapters 6-11 and Chapters 15-18
roadmaps along with your new Chapter 19 roadmap for these.
(a)
1. BHS
2. H₂O₂
3. H₂CrO4
4. SOCI₂
(b)
1. Cl₂/hv
2. KOLBU
3. H₂O, catalytic H₂SO4
4. H₂CrO4
Reaction
Roadmap
An alkene 5. EtOH
6.0.5 Equiv. NaOEt/EtOH
7. Mild H₂O
An alkane
1.0
2. (CH3)₂S
3. H₂CrO
(d)
(c)
4. Excess EtOH, catalytic H₂SO
OH
4. Mild H₂O*
5.0.5 Equiv. NaOEt/EtOH
An alkene 6. Mild H₂O*
A carboxylic
acid
7. Mild H₂O*
1. SOC₁₂
2. EtOH
3.0.5 Equiv. NaOEt/E:OH
5.1.0 Equiv. NaOEt
6.
NH₂
(e)
1. 0.5 Equiv. NaOEt/EtOH
2. Mild H₂O*
Br
(f)
i
H
An aldehyde
1. Catalytic NaOE/EtOH
2. H₂O*, heat
3. (CH,CH₂)₂Culi
4. Mild H₂O*
5.1.0 Equiv. LDA
Br
An ester
4. NaOH, H₂O
5. Mild H₂O*
6. Heat
7.
MgBr
8. Mild H₂O*
7. Mild H₂O+
Li+ is a hard acid. With this in mind, which if the following compounds should be most soluble in water?
Group of answer choices
LiBr
LiI
LiF
LiCl
Chapter 10 Solutions
WebAssign for Zumdahl/Zumdahl/DeCoste's Chemistry, 10th Edition [Instant Access], Single-Term
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