Home
Class 12
CHEMISTRY
Calculate E(cell)^(@) for the followin...

Calculate `E_(cell)^(@)` for the following reaction at 298 K.
`2Al_((s)) + 3Cu^(2+)(0.01M) rightarrow (0.01M) + 3Cu_((s))`
Given : `E_(cell) = 1.98V` |

Text Solution

AI Generated Solution

To calculate the standard cell potential \( E^\circ_{cell} \) for the reaction: \[ 2 \text{Al}_{(s)} + 3 \text{Cu}^{2+}_{(0.01M)} \rightarrow 2 \text{Al}^{3+}_{(0.01M)} + 3 \text{Cu}_{(s)} \] at 298 K, we can use the Nernst equation: ...
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate E_(cell)^(@) for the following reaction at 298 K: 2Al(s) + 3Cu^(2+)(0.01M) to 2Al^(3+)(0.01M) + 3Cu(s) "Given" : E_(cell) = 1.98V (b) Using the E^(@) values A and B, predict which is better for coating the surface of iron [E^(@)(Fe^(2+)//Fe) = -0.44V] to prevent corrosion and why? "Given" : E^(@)(A^(2+)//A) = 2.37V : E^(@)(B^(2+) //B) = 0.14V

Calculate E_(cell)^(@) for the following reaction at 298 K : 2 Cr (s ) + 3 Fe^(2+) (0.01 M) to 2 Cr^(3+) (0.01 M) + 3 Fe (s) Given : E_(cell) = 0.261 V

Calculate DeltaG^(@) and log K_(c) for the following reaction at 298 K : 2Al(s)+3Cu^(2+)(aq)rarr2Al^(3+)(aq)+3Cu(s) Given E_(cell)^(@) =2.02 V

Calculate emf of the following cell reaction at 2968 K : Ni(s)//Ni^(2+)(0.01 M) || Cu^(2+)(0.1 M)//Cu(s) [Given E_(Ni^(2+)//Ni)^(@)=-0.25" V ",E_(Cu^(2+)//Cu)^(@)=+0.34 " V " ] Write the overall cell reaction.