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dangina [55]
2 years ago
10

What is the change in entropy of the lead when 2.0 kg of molten lead at its melting point temperature solidifies.

Chemistry
1 answer:
Rainbow [258]2 years ago
7 0

Answer: The change in entropy of the lead when 2.0 kg of molten lead at its melting point temperature solidifies is 20 cal/K.

Explanation:

Pb(l)\rightleftharpoons Pb(s)

\Delta S=\frac{q}{T}

{\text{Change in entropy}}=\frac{heat}{Temperature}

T is the temperature at which the process is carried out, here the temperature is constant, 327.5°C = (273+327.5)K=600.5K ,because only phase change occurs.

q =  heat given in the process = m\times L_f

m = mass of lead = 2.0 kg

L_f = latent heat of fusion of lead =  5.9 kcal/kg

\Delta S=\frac{2kg\times 5.9kcal/kg}{600.5K}

\Delta S=0.02 kcal/K=20cal/K

Thus the change in entropy of the lead when 2.0 kg of molten lead at its melting point temperature solidifies is 20 cal/K.

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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.

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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+}

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First balance the main element in the reaction.

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

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Now balance hydrogen atom on both side.

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Now balance the charge.

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The balanced chemical equation in acidic medium will be,

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