[" Q2.Calculate the "E_(" cell ")" of the following reaction at "298K],[2Al(s)+3Cu^(2+)(0.01M)rarr2A^(13+)(0.01M)+3Cu(s)],[" Give "E_(cell)=1.98V]

Calculate E_("cell")^(@) for the following reaction at 298K : 2Al(s)+3Cu^(2+)(0.01M)rarr 2Al^(3+)(0.01M)+3Cu(s) [GIven E_(cell)=1.98V ]

Caculate the E_(cell)^@ for the following reaction at 298K: 2Cr(s)+3Fe^(2+)(0.01M)rarr2Cr^(3+)(0.01M)+3Fe(s) Given E_(cell)=0.261V .

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 |

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: 2AI(s) + 3Cu^(2+)(0.01M) to 2A1^(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 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 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 the equilibrium constant of the following reaction aty 298K. Cu(s)+2Ag^+(aq) rarr Cu^(2+)(aq)2Ag(s)~ Given E_(cell)^Theta=0.46V