Concept explainers
(a)
Interpretation:
The value of
Concept introduction:
The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.
Heat is one form of energy.
The amount of energy required to break a
(b)
Interpretation:
The value of
Concept introduction:
The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.
Heat is one form of energy.
The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.
(c)
Interpretation:
It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exothermic or endothermic in nature.
Concept introduction:
The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction. Heat is given off when bonds are formed and heat is consumed when bonds are broken.
Heat is one form of energy.
The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.
A reaction with a negative
A reaction with a positive
(d)
Interpretation: It should be identified that whether the given reactions (addition of HCl to ethene and addition of dihydrogen to ethene) are exergonic or endergonic in nature.
Concept introduction:
The amount of heat consumed or given off during the course of a reaction is known as enthalpy of reaction (H). Heat is given off when bonds are formed and heat is consumed when bonds are broken.
Heat is one form of energy.
The amount of energy required to break a chemical bond is referred to as bond dissociation enthalpy.
The mathematical relationship between enthalpy (H) and free energy (G) is,
In an exergonic reaction the products have a lower free energy than it consumes.
In an endergonic reaction the product have a higher free energy than it consumes.
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Chapter 5 Solutions
Organic Chemistry
- 2) The equilibrium constant Ke for the reaction A B is 1 x 105 at room temperature (25°C). a) You make a solution containing compound A at a concentration of 1 M and compound B at a concentration of 1 mM of B, and let the reaction proceed to equilibrium. What are the equilibrium concentrations of A and B? b) Calculate the standard free-energy change (AG) for this reaction. c) What is the standard free-energy change (AG) for the inverse reaction (BA)?arrow_forwardWhat is the name of the process shown below and how does it work (be specific about what happens to the molecules involved)? Which class of biomolecules (protein, lipid, carbohydrate, nucleic acid) are involved in this particular reaction example? List at least 2 types of functions this class of macromolecules might be involved in biologically. CH₂OH CH₂OH CH2OH CH₂OH НО ОН он ОН н ОН OH ОН Н + H2O → HO ОН ОН н OH + НО ОН ОН Н ОНarrow_forwardN-benzylethanamide Draw the molecule on the canvas by choosing buttons from the Tools (for bonds), Atoms, and Adv toolbars. The single bond is active by default. DC H 12D EXP. CONT. Gl · [1] A ZI CH3 H с N S CI Br I P Farrow_forward
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- a. Find the delta(H) for the equation above b. State the molar heat of combustion of C2H2 c. State whether the reaction is endothermic or exothermic and why.arrow_forwardFormation of ammonia from nitrogen and hydrogen is an exothermic process. Which of the following statements is true about the bonds that are broken and formed during this reaction? N2(g) + 3H2(g) ---> 2NH3(g) a.) products have lower PE because product bonds are weaker than reactants b.) products have higher PE because product bonds are stronger than reactants c.) products have higher PE because product bonds are weaker than reactants d.) products have lower PE because product bonds are stronger than reactantsarrow_forwardCH,(9) + 2 O,(g) AH = -809.0 kJ/mol rxn Co,(9) + 2 H,0(g) ΔΗ. = -81.3 kJ 'cond 2 H,0U) Given the energy diagram above, what is AH when two moles of methane are combusted? -401.15 kJ +1604.6 kJ -802.3 kJ +802.3 kJ +401.15 kJ O -1604.6 kJarrow_forward
- Calculate A,H for the following reaction: 5C(s) + 6H2(9) → C5H12(1) Use the following reactions and given ArH's. C5H12 (1) + 8 O2(g) → 5CO2(g) + 6H2O(g), A;H = -3505.8 kJ mol C(s) + 02(g) → CO2(g), ArH = -393.5 kJ mol1 2H2(g) + O2(9) → 2H2O(g) , A¡H = -483.5 kJ molarrow_forward19. For the following reaction, 2H2S (g) + O2 (g) = 25 (s) + 2H2O (g) Explain what happen to a. [02] if H2S is added. b. [H2S] if Oz is added. c. (H2O] if O2 is removed.arrow_forwardTo a test tube containing 5.0 ml of 1.00 M NaOH at 27°C in a calorimeter, 5.0 ml of 2.00 M HNO3 at the same temperature was added, the heat generated by the reaction was monitored. Which of the following is TRUE? a.Reaction is exothermic; solution will turn pink upon addition of phenolphthalein. b.Heat is absorbed by the system; no color change will be observed upon addition of phenolphthalein. c.Heat is released by the system; no color change will be observed upon addition of phenolphthalein. d.Reaction is endothermic; solution will turn pink upon addition of phenolphthalein.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning