Consider a redox reaction for which E∘ is a negative number. Part A What is the sign of ΔG∘ for the reaction? What is the sign of for the reaction? ΔG∘ > 0 ΔG∘ < 0 Request Answer Part B Will the equilibrium constant for the reaction be larger or smaller than 1? Will the equilibrium constant for the reaction be larger or smaller than 1? K > 1 K < 1 Request Answer Part C Can an electrochemical cell based on this reaction accomplish work on its surroundings? Can an electrochemical cell based on this reaction accomplish work on its surroundings? An electrochemical cell based on this reaction not accomplish work on its surroundings An electrochemical cell based on this reaction accomplish work on its surroundings.

a) ΔG∘ > 0

b) K < 1

c) The electrochemical cell based on this reaction cannot accomplish work on its surroundings.

Explanation:

The Gibb's free energy, ΔG∘, is related to the potential of the cell, E∘ through

ΔG∘ = -nFE∘

where n = number of electrons being gained or lost in the electric cell

F = Amount of Faraday's electricity

a) If E∘ < 0, that is, negative,

ΔG∘ = positive (Since n and F cannot be negative)

That is, ΔG∘ > 0

b) Will the equilibrium constant for the reaction be larger or smaller than 1?

The Gibb's free energy is also related to the equilibrium constant through

ΔG∘ = - nRT In K

where n = number of moles = always positive

R = molar gas constant = always positive

T = absolute temperature in Kelvin = almost always positive too.

Recall that ΔG∘ > 0, that is positive too,

Hence,

- nRT In K = ΔG∘

In K = -(ΔG∘/nRT)

Since all of the quantities on the right hand side are positive parameters,

In K = a negative number

Meaning that K is less than 1.

The equilibrium constant is less than 1.

K < 1

c) Can an electrochemical cell based on this reaction accomplish work on its surroundings?

The Gibb's free energy determines spontaneity.

A process with a negative Gibb's free energy is said to be spontaneous and gives off the free energy as the process proceeds.

A process with a positive Gibb's free energy is said to be non-spontaneous. This one cannot give free energy (work) out to the environment.

For this question, the Gibb's free energy is positive, hence, the electrochemical cell based on this reaction cannot accomplish work on its surroundings.

Hope this Helps!!!

im not exactly sure but i think its b!

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.