Which of the following statements concerning the free energy change ( G) is fals
ID: 101153 • Letter: W
Question
Which of the following statements concerning the free energy change (G) is false?
The energy change for a reaction depends only on the initial and final states, and is independent of the path taken.
The energy change is a function of the concentrations of the products and reactants at reaction start.
The overall energy change for a reaction could be calculated by summing the energy changes for a series of separate reactions that could convert the reactants to the products.
The rate of a reaction cannot be determined from the free energy change.
All of the above answers are true
Biochemists use a modified value for standard G values because
all reagents are not at a 1 molar concentration.
the concentration of water is not at 1 molar concentration.
the reagents are not at one molar concentration and the pH = 7.
All of these justify why biochemists use a special G value.
Which of the following statements are TRUE?
This reaction is exergonic at standard state conditions.
This reaction would require free energy from another reaction in order to go in the direction indicated.
At equilibrium, there will be more [C] and [D] than [A] and [B].
At equilibrium, there will be equal amounts of [A], [B], [C] and [D].
Running this reaction in reverse (i.e. backwards) would result in an endergonic reaction.
This reaction will always be exergonic at any condition.
By definition, a non-spontaneous reaction is one in which
the energy change is zero.
the reaction happens quickly
the enthalpy change is negative
energy is absorbed.
energy is released.
Spontaneous reaction always occurs at a relatively fast rate.
True
False
The second law of thermodynamics can be rephrased as:
absolute zero (0 K) is the absolute minimum temperature of the universe
heat is a measure of the thermal energy of an object
energy can neither be created nor destroyed
non-spontaneous reactions must have slower kinetic rates than spontaneous reactions
any energy transformation increases the entropy of the universe
Consider each of the following scenarios, then choose the scenario(s) in which entropy INCREASES in the described system.
Choose all that apply.
A fertilized frog egg divides into thousands of specialized cells in order to form an embryo.
A fire burns in a fireplace and reduces an oak log to ashes.
You accidentally spill your milk into a fish tank, turning the water a cloudy white.
A double stranded DNA molecule is assembled from individual deoxyribonucleotides.
Your biochemistry professor writes a chemical reaction on the board and says the reaction is "exergonic". What can you conclude from this?
The reaction will have a positive delta H.
The reaction must occur at room temperature (298 K)
The reaction will have a positive delta G.
The reaction will have a negative delta H.
The reaction will have a negative delta G.
The reaction will have a positive delta S.
The energy change for a reaction depends only on the initial and final states, and is independent of the path taken.
The energy change is a function of the concentrations of the products and reactants at reaction start.
The overall energy change for a reaction could be calculated by summing the energy changes for a series of separate reactions that could convert the reactants to the products.
The rate of a reaction cannot be determined from the free energy change.
All of the above answers are true
Explanation / Answer
1. The Gibbs free energy is a thermodynamic potential that can be used to calculate the maximum work performed by a thermodynamic system at a constant temperature and pressure. All the above statements are true regarding free energy change.
2. Standard value of Gibbs free energy is taken at 1molar concentration of reactants and products and at pH=7. The correct answer is option C.
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