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Brrunno [24]
3 years ago
8

Which ONE of the following is an oxidation–reduction reaction? A) PbCO3(s) + 2 HNO3(aq) ––––> Pb(NO3)2(aq) + CO2(g) + H2O(l)

B) Na2O(s) + H2O(l) –––> 2 NaOH(aq) C) SO3(g) + H2O(l) ––––> H2SO4(aq) D) CO2(g) + H2O(l) ––––> H2CO3(aq) E) C2H4(g) + H2(g) ––––> C2H6(g)
Chemistry
1 answer:
sveta [45]3 years ago
8 0

Answer:

E) C₂H₄(g) + H₂(g) ⇒ C₂H₆(g)

Explanation:

Which ONE of the following is an oxidation–reduction reaction?

A) PbCO₃(s) + 2 HNO₃(aq) ⇒ Pb(NO₃)₂(aq) + CO₂(g) + H₂O(l). NO. All the elements keep the same oxidation numbers.

B) Na₂O(s) + H₂O(l) ⇒ 2 NaOH(aq). NO. All the elements keep the same oxidation numbers.

C) SO₃(g) + H₂O(l) ⇒ H₂SO₄(aq). NO. All the elements keep the same oxidation numbers.

D) CO₂(g) + H₂O(l) ⇒ H₂CO₃(aq). NO. All the elements keep the same oxidation numbers.

E) C₂H₄(g) + H₂(g) ⇒ C₂H₆(g). YES. <u>C is reduced</u> and <u>H is oxidized</u>.

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Answer : The value of \Delta G^o and K is, -180 kJ/mol and 3.6\times 10^{31}

Explanation :

The balanced cell reaction will be,

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The half-cell reactions are:

Oxidation reaction (anode) : Pb(s)\rightarrow Pb^{2+}(aq)+2e^-

Reduction reaction (cathode) : 2Ag^+(aq)+2e^-\rightarrow 2Ag(g)

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\Delta G^o=-2\times 96500\times 0.93

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Now we have to calculate the value of 'K'.

\Delta G^o=-RT\ln K

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\Delta G_^o =  standard Gibbs free energy  = -180 kJ/mol

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-180kJ/mol=-(8.314\times 10^{-3}kJ/mole.K)\times (298K)\times \ln K

K=3.6\times 10^{31}

Therefore, the value of \Delta G^o and K is, -180 kJ/mol and 3.6\times 10^{31}

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