Balancing redox reactions?
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How do you balance this: S2O3^-2 + I2 -----> I^- + S4O6^-2 (in acidic solution) PLEASE give all steps!!
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Answer:
S2O3^-2 + I2 -----> I^- + S4O6^-2 (in acidic solution) I2 -----> I- NOT ENOUGHT IODINE I2 -----> 2I- NOT ENOUGH ELECTRONS 2e- + I2 -----> 2I- BALENCED HALF RXN S2O3^-2 -----> S4O6^-2 NOT ENOUGH S OR O 2S2O3^-2 -----> S4O6^-2 NOT ENOUGH ELECTRONS 2S2O3^-2 -----> S4O6^-2 + 2e- BALANCED HALF RXN 2S2O3^-2 -----> S4O6^-2 + 2e- AND 2e- + I2 -----> 2I- 2e- + I2 + 2S2O3^-2 -----> 2I- + S4O6^-2 + 2e- EXTRA e- s I2 + 2S2O3^-2 -----> 2I- + S4O6^-2
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