The isotopes K-37 and K-42 have the same

What can be said about an endothermic reaction with a negative entropy change? View Available Hint(s) The reaction is What can b

REY [17]

Answer: The reaction is spontaneous at low temperatures

Explanation:

Let's first remember the definition of certain terms;

Enthalpy (H) in thermodynamics is defined as the heat content of a reaction. While Entropy (S) in thermodynamics is termed as the quantification of disorder or randomness of a reaction.

Gibb’s free energy change helps to determine the direction of the reaction.

Using the Gibbs free energy equation to solve this question.

∆G = ∆H - T∆S

Where;

∆G = Gibbs free energy

∆H = change in enthalpy

T= temperature of the reaction

∆S = change in entropy.

The question states that it is an exothermic reaction with negative entropy. This means that the change in both enthalpy and entropy will be negative. That is;

∆H = >0 ( it's positive)

∆S = < 0 (negative)

Let's remember that an exothermic reaction generally releases energy to it surroundings. This energy is usually released in the form of heat. Therefore, the change in enthalpy H of an exothermic reaction will always be negative. A negative change in entropy S indicates that there is a decrease in disorder, with respect to the reaction.

Using Gibb’s free energy equation at constant temperature and pressure, we have;

∆G = ∆H - T∆S

Now, the change in enthalpy and change in entropy can be written as follows;

∆H = >0 ( it's positive)

∆S = < 0 (negative)

Substitute these values in the above equation;

∆G = ∆H - T - (∆S)

∆G = ∆H + T∆S

According to the sign convention seen in the equation above,

Change in ∆G will be negative <0 when the value ∆H is greater than T∆S.

This change can occur only at low temperatures. Thus, this reaction is spontaneous at low temperatures.

5 0

3 years ago

Given the partial equation:

Nikolay [14]

Answer : The balanced chemical equation in acidic medium will be,

$IO_3^-(aq)+2Sn^{2+}(aq)+6H^+(aq)\rightarrow I^-(aq)+2Sn^{4+}(aq)+3H_2O(l)$

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

Rules for the balanced chemical equation in acidic solution are :

First we have to write into the two half-reactions.

Now balance the main atoms in the reaction.

Now balance the hydrogen and oxygen atoms on both the sides of the reaction.

If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the less number of oxygen are present.

If the hydrogen atoms are not balanced on both the sides then adding hydrogen ion $(H^+)$ at that side where the less number of hydrogen are present.

Now balance the charge.

The given chemical reaction is,

$IO_3^-(aq)+Sn^{2+}(aq)\rightarrow I^-(aq)+Sn^{4+}(aq)$

The oxidation-reduction half reaction will be :

Oxidation : $Sn^{2+}\rightarrow Sn^{4+}$

Reduction : $IO_3^-\rightarrow I^-$

First balance the main element in the reaction.

Oxidation : $Sn^{2+}\rightarrow Sn^{4+}$

Reduction : $IO_3^-\rightarrow I^-$

Now balance oxygen atom on both side.

Oxidation : $Sn^{2+}\rightarrow Sn^{4+}$

Reduction : $IO_3^-\rightarrow I^-+3H_2O$

Now balance hydrogen atom on both side.

Oxidation : $Sn^{2+}\rightarrow Sn^{4+}$

Reduction : $IO_3^-+6H^+\rightarrow I^-+3H_2O$

Now balance the charge.

Oxidation : $Sn^{2+}\rightarrow Sn^{4+}+2e^-$

Reduction : $IO_3^-+6H^++4e^-\rightarrow I^-+3H_2O$

The charges are not balanced on both side of the reaction. Thus, we are multiplying oxidation reaction by 2 and the adding both equation, we get the balanced redox reaction.

Oxidation : $2Sn^{2+}\rightarrow 2Sn^{4+}+4e^-$

Reduction : $IO_3^-+6H^++4e^-\rightarrow I^-+3H_2O$

The balanced chemical equation in acidic medium will be,

$IO_3^-(aq)+2Sn^{2+}(aq)+6H^+(aq)\rightarrow I^-(aq)+2Sn^{4+}(aq)+3H_2O(l)$

5 0

3 years ago

Which one of these is not a pathogen?

TiliK225 [7]

B, plant

A pathogen is a bacterium, virus, or other microorganisms that can cause disease. A plant does cause a disease

5 0

4 years ago

Why is it necessary for Agricultural student to study home science.

sveta [45]

Answer:

Hope it's help uu.. thankuu

7 0

2 years ago

Luke stirred the water during the experiment. How did this make his results more reliable?

Mama L [17]

Well if anything was mixed in it would make his result different. if not, it could have changed the temperature when he mixed it. which would give him either a lower or higher answer

3 0

3 years ago