Which of the following redox reactions are spontaneous --
SN2+(aq)+BA(s)->Sn(s)+Ba2+(aq)
2AG+(ag)+2Cl-(aq)->2Ag(s)+C12(g)
ZN(s)+F2(g)->2F-(aq)+Zn2+(aq)
2LI(s)+Co2+->(aq)->2Li+(aq)+Co(s)
2I-(aq)+K+(aq)->I2(s)+K(s)
I believe it is A, C & E
I don't know and you can look up (and probably have) the E values. If Ecell is +, the cell is spontaneous. Note that AG, ZN and SN don't mean anything.
To determine whether the redox reactions are spontaneous, we need to compare the reduction potentials (also known as standard electrode potentials) of the reactants and products involved.
In general, a redox reaction will be spontaneous if the reduction potential of the product is greater than the reduction potential of the reactant. If the opposite is true, and the reduction potential of the reactant is greater, the reaction will not be spontaneous.
Let's go through each reaction and compare the reduction potentials:
A) SN2+(aq) + BA(s) -> Sn(s) + Ba2+(aq)
To find the reduction potential, we can refer to a table of standard reduction potentials. Comparing the reduction potentials of Sn2+ (+0.15 V) and Ba2+ (-2.90 V), we can see that Ba2+ has a more negative (lower) reduction potential, which means it is more likely to be reduced. Therefore, this reaction is not spontaneous.
B) 2Ag+(aq) + 2Cl-(aq) -> 2Ag(s) + Cl2(g)
Comparing the reduction potentials of Ag+ (+0.80 V) and Cl2 (+1.36 V), we can see that Cl2 has a higher reduction potential. This indicates that Cl2 is more likely to be reduced. Therefore, this reaction is spontaneous.
C) Zn(s) + F2(g) -> 2F-(aq) + Zn2+(aq)
Comparing the reduction potentials of F2 (+2.87 V) and Zn2+ (-0.76 V), we can see that F2 has a higher reduction potential. This indicates that F2 is more likely to be reduced. Therefore, this reaction is spontaneous.
D) 2Li(s) + Co2+(aq) -> 2Li+(aq) + Co(s)
Comparing the reduction potentials of Co2+ (-0.28 V) and Li+ (-3.04 V), we can see that Co2+ has a more negative (lower) reduction potential. This means Co2+ is more likely to be reduced. Therefore, this reaction is not spontaneous.
E) 2I-(aq) + 2K+(aq) -> I2(s) + 2K(s)
Comparing the reduction potentials of I- (-0.54 V) and K+ (-2.92 V), we can see that I- has a higher reduction potential. This indicates that I- is more likely to be reduced. Therefore, this reaction is spontaneous.
Based on the analysis above, the spontaneous redox reactions are B, C, and E.