The products of the given reaction and its occurrence to any measurable extent are to be predicted. Concept Introduction: Strong acids ionize completely in aqueous solutions to produce hydronium ions and their conjugate base. The conjugate base produced by a stronger acid is very weak, so that it does not recombine with hydronium ions to form acid. Conjugate bases of stronger acids are relatively more stable than the conjugate bases of weaker acids. Thus, a stable conjugate base will have lower affinity for a proton than an unstable conjugate base. Similarly, conjugate acids that are less stable come from weak bases and tend to lose a proton more easily as compared to stable conjugate acids that are derived fromstrong bases and do not lose their proton easily.
The products of the given reaction and its occurrence to any measurable extent are to be predicted. Concept Introduction: Strong acids ionize completely in aqueous solutions to produce hydronium ions and their conjugate base. The conjugate base produced by a stronger acid is very weak, so that it does not recombine with hydronium ions to form acid. Conjugate bases of stronger acids are relatively more stable than the conjugate bases of weaker acids. Thus, a stable conjugate base will have lower affinity for a proton than an unstable conjugate base. Similarly, conjugate acids that are less stable come from weak bases and tend to lose a proton more easily as compared to stable conjugate acids that are derived fromstrong bases and do not lose their proton easily.
Solution Summary: The author explains that strong acids ionize completely in aqueous solutions to produce hydronium ions and their conjugate base, but the reaction does not proceed to any measurable extent.
The products of the given reaction and its occurrence to any measurable extent are to be predicted.
Concept Introduction:
Strong acids ionize completely in aqueous solutions to produce hydronium ions and their conjugate base. The conjugate base produced by a stronger acid is very weak, so that it does not recombine with hydronium ions to form acid.
Conjugate bases of stronger acids are relatively more stable than the conjugate bases of weaker acids. Thus, a stable conjugate base will have lower affinity for a proton than an unstable conjugate base.
Similarly, conjugate acids that are less stable come from weak bases and tend to lose a proton more easily as compared to stable conjugate acids that are derived fromstrong bases and do not lose their proton easily.
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Consider the following reaction:
CH3OH(g)
CO(g) + 2H2(g)
(Note that AG,CH3OH(g) = -162.3 kJ/mol and AG,co(g)=-137.2 kJ/mol.)
Part A
Calculate AG for this reaction at 25 °C under the following conditions:
PCH₂OH
Pco
PH2
0.815 atm
=
0.140 atm
0.170 atm
Express your answer in kilojoules to three significant figures.
Ο ΑΣΦ
AG = -150
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kJ
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Calculate the free energy change under nonstandard conditions (AGrxn) by using the following relationship:
AGrxn = AGrxn + RTInQ,
AGxn+RTInQ,
where AGxn is the standard free energy change, R is the ideal gas constant, T is the temperature in kelvins, a
is the reaction quotient.
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