here reaction is occurring when Sn and I2 are refluxed together reduction and oxidation is takes place(called redox ) he would ask the oxidation potential &its reduction potential is asking . Sn + 2I2------>SnI4 here Sn oxidised to Sn2+ ,iodine reduced ,means reduction potential of tin(Sn) is E0= -0.136, I2 reduction potential is =+0.53 ,its indicates reduction potential of iodine is more so it can oxidise the Sn & it can be reduced. Zn(s) + I2(s) -----> Zn2+ (aq) + 2I- (aq) here Zn oxidised to Zn2+ ,iodine reduced ,means reduction potential of tin(Sn) is E0=-0.763 I2 reduction potential is =+0.53 ,its indicates reduction potential of iodine is more so it can oxidise the Zn & it can be reduced Sn(s)+2HCl (aq) -----> Sn2+ (aq) +2Cl- (aq) + H2 (g) here Sn oxidised to Sn2+ ,chlorine reduced ,means reduction potential of tin(Sn) is E0=- 0.136here Sn oxidised to Sn2+ ,chlorine reduced ,means reduction potential of tin(Sn) is E0=- 0.136, cl- reduction potential is =+1.36 ,its indicates reduction potential of chlorine is more so it can oxidise the Sn & it(Cl) can be reduced. Sn2+ (aq) + 2I- (aq) -----> SnI2 (s) I2 reduction potential is =+0.53 ,its indicates reduction potential of iodine is less than the Sn2+ so it can reduce the Sn2+ & it(I-) can be oxidised. Solution here reaction is occurring when Sn and I2 are refluxed together reduction and oxidation is takes place(called redox ) he would ask the oxidation potential &its reduction potential is asking . Sn + 2I2------>SnI4 here Sn oxidised to Sn2+ ,iodine reduced ,means reduction potential of tin(Sn) is E0= -0.136, I2 reduction potential is =+0.53 ,its indicates reduction potential of iodine is more so it can oxidise the Sn & it can be reduced. Zn(s) + I2(s) -----> Zn2+ (aq) + 2I- (aq) here Zn oxidised to Zn2+ ,iodine reduced ,means reduction potential of tin(Sn) is E0=-0.763 I2 reduction potential is =+0.53 ,its indicates reduction potential of iodine is more so it can oxidise the Zn & it can be reduced Sn(s)+2HCl (aq) -----> Sn2+ (aq) +2Cl- (aq) + H2 (g) here Sn oxidised to Sn2+ ,chlorine reduced ,means reduction potential of tin(Sn) is E0=- 0.136here Sn oxidised to Sn2+ ,chlorine reduced ,means reduction potential of tin(Sn) is E0=- 0.136, cl- reduction potential is =+1.36 ,its indicates reduction potential of chlorine is more so it can oxidise the Sn & it(Cl) can be reduced. Sn2+ (aq) + 2I- (aq) -----> SnI2 (s) I2 reduction potential is =+0.53 ,its indicates reduction potential of iodine is less than the Sn2+ so it can reduce the Sn2+ & it(I-) can be oxidised..