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Mnenie [13.5K]
3 years ago
5

Please help me answer these 3 questions

Chemistry
1 answer:
aleksandr82 [10.1K]3 years ago
3 0

Explanation:

Photosynthesis is the process by which green plants manufacture their food using carbon dioxide and water in the presence of sunlight.

It is expressed using the equation below;

      6CO₂   +   6H₂O     →      C₆H₁₂O₆  +  6O₂

         reactants                      products

1. Compounds consumed are carbon dioxide and water.

2. Product is glucose and oxygen.

3. Most organism obtain their nourishment directly and indirectly from photosynthetic activities.

Plants are the producers of food in the ecosystem. If the process of photosynthesis does not occur, there is no way other organisms will obtain their own nourishment.

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Answer: a) Anode: Cr\rightarrow Cr^{3+}+3e^-

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Cathode : Au

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d) E_{cell}=2.14V

Explanation: - 

a) The element Cr with negative reduction potential will lose electrons undergo oxidation and thus act as anode.The element Au with positive reduction potential will gain electrons undergo reduction and thus acts as cathode.

At cathode: Au{3+}+3e^-\rightarrow Au

At anode: Cr\rightarrow Cr^{3+}+3e^-

b) At cathode which is a positive terminal, reduction occurs which is gain of electrons.

At anode which is a negative terminal, oxidation occurs which is loss of electrons.

Gold acts as cathode ad Chromium acts as anode.

c) Overall balanced equation:

At cathode: Au{3+}+3e^-\rightarrow Au     (1)

At anode: Cr\rightarrow Cr^{3+}+3e^-        (2)

Adding (1) and (2)

Au^{3+}+Cr\rightarrow Au+Cr^{3+}

d)E^0_(Cr^{3+}/Cr)= -0.74 V

E^0_(Au^{3+}/Au)= 1.40 V  

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Using Nernst equation :

E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Au^{3+}]}{[Cr^{3+}]^}

where,

n = number of electrons in oxidation-reduction reaction = 3

E^o_{cell} = standard electrode potential = 2.14 V

E_{cell}=2.14-\frac{0.0592}{3}\log \frac{[1.0}{[1.0]}

E_{cell}=2.14

Thus the standard potential for an electrochemical cell with the cell reaction is 2.14 V.

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