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saw5 [17]
2 years ago
11

Find the potentials of the following electrochemical cell:

Chemistry
1 answer:
melomori [17]2 years ago
6 0

Answer: 0.18 V

Explanation:-

Cd/Cd^{2+}(0.10M)//Ni^{2+}(0.50M)?Ni

Here Cd undergoes oxidation by loss of electrons, thus act as anode. nickel undergoes reduction by gain of electrons and thus act as cathode.

E^0_(Cd^{2+}/Cd)=-0.40V[/tex]

E^0_(Ni^{2+}/Ni)=-0.24V[/tex]

Cd+Ni^{2+}\rightarrow Cd^{2+}+Ni

Here Cd undergoes oxidation by loss of electrons, thus act as anode. nickel undergoes reduction by gain of electrons and thus act as cathode.

E^0=E^0_{cathode}- E^0_{anode}

Where both E^0 are standard reduction potentials.

E^0=E^0_{[Ni^{2+}/Ni]}- E^0_{[Cd^{2+}/Cd]}

E^0=-0.24-(-0.40)=0.16V

Using Nernst equation :

E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Cd^{2+}]}{[Ni^{2+]}

where,

n = number of electrons in oxidation-reduction reaction = 2

E^o_{cell} = standard electrode potential = 0.16 V

E_{cell}=0.16-\frac{0.0592}{2}\log \frac{[0.10]}{[0.5]}

E_{cell}=0.18V

Thus the potential of the following electrochemical cell is 0.18 V.

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reaction B is the best one I would choose

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3 years ago
Calculate the mass (in grams) of 250mL of ether at 25 oC. The density of
leonid [27]
  • Volume=250mL
  • Density=0.71g/ml

\boxed{\sf Density=\dfrac{Mass}{Volume}}

\\ \sf{:}\implies Mass=Density(Volume)

\\ \sf{:}\implies Mass=0.71(250)

\\ \sf{:}\implies Mass=177.5g

6 0
2 years ago
My car is 10.4 feet long. how many inches is that​
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Answer:

124.8 inches

Explanation:

7 0
3 years ago
Read 2 more answers
This is the process where fossil fuels, forests, or other carbon-containing substances are burned, adding more carbon dioxide to
sattari [20]
The process where fossil fuels, forests, or other carbon-containing substances are burned, addin more carbon dioxide to the air is the combustion.

Some examples of combustion are:

Fossil fuel:

Carbon + O2

C + O2 -> CO2

Forests (wood)

Wood = cellulose = [C6H10O5]n

[C6H10O5]n + 6nO2 = 6n CO2 + 5n H2O

So, in general the combustion of organic matter produces CO2 and water.


4 0
2 years ago
Does any solid Ag₂CrO₄ form when 2.7x10⁻⁵g of AgNO₃ is dissolved in 15.0 mL of 4.0x10⁻⁴MK₂CrO₄?
e-lub [12.9K]

Molarity of Ag+ is less than the molar solubility thus ppt will not occur.

Balanced reaction-:

<h3>2AgNO3(aq)+K2CrO4(aq)→Ag2CrO4(s)+2KNO3(aq)</h3>

Moles of AgNO3=mass(g)molar mass (g/mol) =2.7×10−5g / 169.86 gmol

=1.589⋅10^−7 mol

Molarity of Ag+=moles of solute(L)=1.589⋅10−7 mol0.015 L=1.059⋅10−5M

Ksp of Ag2CrO4

=[Ag+]2[CrO42−]

1.2⋅10−12=[2s]2[s]

4s3=1.2⋅10−12

s=6.69⋅10−5 M

Molarity of Ag+ is less than the molar solubility thus ppt will not occur.

<h3>What is the molarity calculation formula?</h3>

The volume of solvent required to dissolve the provided solute is multiplied by the ratio of the moles of the solute whose molarity has to be computed. (M=frac{n}{V}) The molality of the solution that needs to be computed in this case is M. n is the solute's molecular weight in moles.

Learn more about Molarity:

brainly.com/question/8732513

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3 0
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