What is the standard cell potential for the reaction,
`2Cr(s) + 3Sn^(2+)(aq) rightarrow 3Sn(s) + 2Cr^(3+)(aq)`
given the `E^(@)` values shown?

Write Nernst equation for the reaction: (i) 2Cr(s) +3Cd^(2+)(aq) to 2Cr^(3+) (aq) +3Cd(s)

Sn^(4+)(aq) + 2e^(-) rightarrow Sn^(2+)(aq) E^(@) = 0.15V Cr^(3+)(aq) + e^(-) rightarrow Cr^(2+)(aq) E^(@) = 0.41V According to the standard reduction potentials above, what is the value of E^(@) for the reaction below? 2Cr^(3+)(aq) + Sn^(2+)(aq) rightarrow 2Cr^(2+)(aq) + Sn^(4+)(aq)

Write the Nernst equation for the reaction : 2Cr(s)+3Cd^(2+)(aq) to 2Cr^(3+)(aq)+3Cd(s)

Consider a voltaic cell in which the reaction below occurs in two half-cells connected by a salt bridge and an external circuit. 2Cr(s) + 3Sn^(2+)(aq) rightarrow 3Sn(s) + 2Cr^(3+)(aq) E^(@) = 0.603V . Which change will cause the voltage to increase?

Consider the following E^(@) values E^(@) values E_(Fe^(3+)//Fe^(2+))^(@)= 0.77v , E_(Sn^(2+)//Sn)^(@) = -0.14 under standard condition the potential for the reaction Sn_(s)+ 2Fe^(3+)(aq)rightarrow 2Fe^(2+)(aq) + Sn^(2+) (aq) is :

Consider the following E^(@) values E^(@) values E_(Fe^(3+)//Fe^(2+))^(@)= 0.77v , E_(Sn^(2+)//Sn)^(@) = -0.14 under standard condition the potential for the reaction Sn_(s)+ 2Fe^(3+)(aq)rightarrow 2Fe^(2+)(aq) + Sn^(2+) (aq) is :

Given these standard reduction potentials, what is the standard reduction potential for Co^(3+)(aq) + 3e^(-) rightarrow Co(s) ? Co^(3+)(aq) + e^(-) rightarrow Co^(2+)(aq) E^(@) = 1.82V Co^(2+)(aq) + 2e^(-) rightarrow Co(s) E^(@) = -0.28V