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-i) - The cell in which the following reaction occurs 2Fe+ (aq) +21(aq) 2Fe+2 (aq) +1_) has 0236 V at 298K Calculate the standard Gibbs energy of the cell reaction. (given IF-96500 (molt') How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? ii

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Q1
(a) The cell in which the following reaction occurs:
2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2(s) has E⊝cell=0.236V at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C mol−1)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C mol−1)
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Q2
(a) The cell in which the following reaction occurs:
2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2(s) has E⊝cell=0.236V at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C mol−1)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C mol−1)
View Solution
Q3
The cell in which the following reaction occurs:

2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2(s)

has E∘cell=0.236 V at 298 K.

Calculate the standard Gibbs energy of the cell reaction. (Given : 1 F=96,500 C mol−1)
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Q4
The cell in which the following reaction occurs:

2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2(s)
has E∘cell=0.236 V at 298 K.
Calculate the standard Gibbs energy

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Q5
For the cell reaction
2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2(aq)
EoCell=0.24 V at 298 K.
The standard Gibbs energy (ΔrGo) of the cell reaction is :
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