8) Sn¹2(aq) + Zn(s) Sn(s) + Zn¹2(aq) MOMO E-0.2V [Sn2] (M) [Zn] [sn] [Zn¹2] (M) 1 1 0.3 0.6 0.3-x S 0.6+x 0.6V For a reaction of tin (II) ions with zinc to form tin and zinc ions determine the unknown values. The concentrations of zinc and tin solids are not used. a) b) Ecell a) The Ecell with 1M concentrations is just the Eºcell calculated using potentials from a table. b) You will need to use the Nernst equation to adjust the Ecell to concentrations other than 1M. c) Use the Nernst equation backwards with the given Ecell to calculate how much Sn*2 has been converted (the variable x). Report [Sn*2] and [Zn*²] at this value.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![8) Sn¹2(aq) + Zn(s) Sn(s) + Zn+2 (aq)
MO ³ - 3eMO E-0.2V
[Sn+2] (M)
[Zn]
[sn]
[Zn+²] (M) Ecell
a)
1
1
b)
0.3
0.6
c)
0.3-x
S
0.6+x
0.6V
For a reaction of tin (II) ions with zinc to form tin and zinc ions determine the unknown values. The
concentrations of zinc and tin solids are not used.
a) The Ecell with 1M concentrations is just the Eºcel calculated using potentials from a table.
b) You will need to use the Nernst equation to adjust the Ecell to concentrations other than 1M.
c) Use the Nernst equation backwards with the given Ecell to calculate how much Sn2 has been
converted (the variable x). Report [Sn*2] and [Zn2] at this value.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2dbed1da-3f32-4254-ad4d-67b595b99f21%2F6143559a-32be-4a46-bcf4-5f1d01708c49%2Fspre9rn_processed.jpeg&w=3840&q=75)
Answer:
Galvanic cell is the type of cell that converts chemical energy into electrical energy via spontaneous cell reaction. In the Galvanic cell oxidation always occurs at anode and reduction always occurs at cathode.
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