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Standard X

Chemistry

Electrolytic Cells

An oxidation-...

Question

An oxidation-reduction reaction takes place in chemical cell, and energy for a light bulb, is provided by flow of electrons. Find the true statements for reaction:

The reaction is non-spontaneous and has a positive voltage.

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The reaction is non-spontaneous and has a negative voltage.

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The reaction is at equilibrium and has a voltage of zero.

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The reaction is spontaneous and has a positive voltage.

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The reaction is spontaneous and has a negative voltage.

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Solution

The correct option is D The reaction is spontaneous and has a positive voltage.
Option (D) represents the true statement for reaction.
The reaction is spontaneous and has a positive voltage. This is because a chemical reaction generates electrical energy.

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Similar questions

Q. Statement 1: A synthesis reaction that is non-spontaneous and has a negative value for its heat of reaction will not occur until some heat is added.
Statement 2: Non-spontaneous exothermic reactions need enough activation energy to get them started.

Which of the following is not correct?
(a) $Δ$ G is zero for a reversible reaction.
(b) $Δ$ G is positive for a spontaneous reaction.
(c) $Δ$ G is negative for a spontaneous reaction.
(d) $Δ$ G is positive for a non-spontaneous reaction.

Q. Statement I: A reaction with a positive enthalpy and a negative entropy will be spontaneous
BECAUSE
Statement II: The Gibbs free energy for a spontaneous reaction is negative

Q. Free energy,

G = H - T Δ S

, is a state function that indicates whether a reaction is spontaneous or non-spontaneous. If you think of

T S

as the part of the system`s energy that is disordered already, then

(H - T S)

is the part of the system`s energy that is still ordered and therefore free to cause spontaneous change by becoming disordered.
Also,

Δ G = Δ H - T Δ S

From the second law of Thermodynamics, a reaction is spontaneous if

Δ_{t o t a l} S

is positive, non-spontaneous if

Δ_{t o t a l} S

is negative, and at equilibrium if

Δ_{t o t a l} S

is zero.

Since,

- T Δ S = Δ G

and since

Δ G

and

Δ S

have opposite signs, we can restate the Thermodynamic criterion for the spontaneity of a reaction carried out at a constant temperature and pressure.
If

Δ G < 0

, the reaction is spontaneous
If

Δ G > 0

, the reaction is non-spontaneous
If

Δ G = 0

, the reaction is at equilibrium

Read the above paragraph carefully and answer the following questions based on the above comprehension.

A particular reaction has a negative value for the free energy change. Then at ordinary temperature:

Q. Predict whether the reaction

C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g)

at 300 K is spontaneous & exothermic or non-spontaneous & endothermic, when the standard entropy change is

- 0.094 k J m o l^{- 1} K^{- 1} .

The standard Gibb's free energies of formation for

C O_{2}

and

C O

are

- 394.4 a n d - 137.2 k J m o l^{- 1}

respectively.

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An oxidation-reduction reaction takes place in chemical cell, and energy for a light bulb, is provided by flow of electrons. Find the true statements for reaction:

The correct option is D The reaction is spontaneous and has a positive voltage.Option (D) represents the true statement for reaction. The reaction is spontaneous and has a positive voltage. This is because a chemical reaction generates electrical energy.

The correct option is D The reaction is spontaneous and has a positive voltage.
Option (D) represents the true statement for reaction.
The reaction is spontaneous and has a positive voltage. This is because a chemical reaction generates electrical energy.