nitrous acid oxidises I- to I2 in acidic medium balance the equation balance the equation
Answers
+5 ......... Oxidation
+5 ......... OxidationFor N +5 to +4 Net change = -1 ..........Reduction
+5 ......... OxidationFor N +5 to +4 Net change = -1 ..........ReductionStep 5
+5 ......... OxidationFor N +5 to +4 Net change = -1 ..........ReductionStep 5Determine a ratio of oxidized to reduced atoms that would yield a net increase in oxidation number equal to the net decrease in oxidation number.
+5 ......... OxidationFor N +5 to +4 Net change = -1 ..........ReductionStep 5Determine a ratio of oxidized to reduced atoms that would yield a net increase in oxidation number equal to the net decrease in oxidation number.I atoms would yield a net increase in oxidation number of +5. (five electrons would be lost by five I atoms.). 1 N atom would yield a net decrease of -1. (One N atom would gain three electrons.)
number of +5. (five electrons would be lost by five I atoms.). 1 N atom would yield a net decrease of -1. (One N atom would gain three electrons.)Thus the ratio of I atoms to N atoms is 5:1.But we have I2 as a reactant then the ratio becomes 10:1
number of +5. (five electrons would be lost by five I atoms.). 1 N atom would yield a net decrease of -1. (One N atom would gain three electrons.)Thus the ratio of I atoms to N atoms is 5:1.But we have I2 as a reactant then the ratio becomes 10:1Step 6
number of +5. (five electrons would be lost by five I atoms.). 1 N atom would yield a net decrease of -1. (One N atom would gain three electrons.)Thus the ratio of I atoms to N atoms is 5:1.But we have I2 as a reactant then the ratio becomes 10:1Step 6To get the ratio identified in Step 5, add coefficients to the formulas which contain the elements whose oxidation number is changing.
and we will get the balanced equation,
and we will get the balanced equation,I2 + 10 HNO3 → 2HIO3 + 10NO2 + 4H2O
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