Organic Chemistry
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Predict the entropy change (ΔS > 0, ΔS = 0, or ΔS < 0) of the following elimination step:
In which of the following reactions will ∆S° be the greatest and positive? Assume that all the species are gases.
Identify whether the standard entropy change, ΔS°, is positive, negative, zero, or impossible to predict for the reaction below:
Predict whether the ∆S° for the given reaction is expected to be less than, greater than, or equal to 0. Explain.
At room temperature the reaction between propene (CH2=CH−CH3) and hydrogen gas (H2) to form propane (CH3−CH2−CH3) goes to completion when a platinum catalyst is present in the reaction mixture.Determine the signs of ΔH° and ΔS° for this addition reaction based on the information given above. Explain these signs in terms of freedom of motion and bonding.CH2=CH−CH3 + H2 (Pt catalyst) → CH3−CH2−CH3
The hydrogenation of 2-butene to produce butane is shown below:
In terms of entropy, is the reaction favored or disfavored?
From the given reactions, determine which one has a greater ∆S°. Also, is the value positive or negative?
Consider the following equilibrium reaction:
Which direction is favored by ΔH, ΔG, and ΔS?
Predict the sign of ΔS° for the following reaction.
Use the bond-dissociation energies to estimate the equilibrium constant of the reaction given below at 298 K.
The dehydrogenation of ethane (CH3−CH3) to ethene (CH2=CH2) has ΔH° = +136 kJ/mol (+32.5 kcal/mol) and ΔS° = +120 J/kelvin-mol (+28.7 cal/kelvin-mol). Calculate the value of ΔG° for the reaction at room temperature. Is the reaction favored or disfavored?
Determine whether the standard entropy change, ΔS°, is positive, negative, zero, or impossible to predict for the following reaction:
Determine the value of the entropy change ((ΔS > 0, ΔS = 0, or ΔS < 0) in the following reaction:
Provide the temperature at which any value of the entropy change of a process becomes negligible in determining its spontaneity.
Determine if the ∆S° for the given reaction is expected to be less than, greater than, or equal to 0. Justify.
In the given reaction, if the temperature is increased, which side of the reaction, if any, would be favored?
Predict whether the ∆S° of sublimation of dry ice is less than, equal to, or greater than 0. Justify your answer.
Determine whether the ∆S° is less than, greater than, or equal to zero in the reaction shown below.
Consider the following ring-opening reaction of an epoxide:
What is the sign of ∆S°?
A reaction with an equilibrium constant of 2.00 × 10–5 is conducted at 25°C. To increase the equilibrium constant by a factor of 100, what is the required change in each of the following?
(i) ΔG°
(ii) ΔH°, if ΔS° = 0
(iii) ΔS°, if ΔH° = 0