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Balance the following redox reaction and enter the correct coefficients for all of the species in the balanced reaction. Cr2​O72−​(aq)+H2​CO→H2​CO2​+Cr3+(aq) This reaction takes place in an acidic solution H2​COCr2​O72−​(aq)H+H2​CO2​Cr3+(aq)H2​O​
For the reaction, shown below, determine which statements are True and which are False. 3Fe(s)+Cr2​O72−​(aq)+14H+(aq)→3Fe2+(aq)+2Cr3+(aq)+7H2​O(l)ξ∘=1.77 V The oxidation state of chromium in dichromate is +2. The iron half-reaction takes place in an acidic solution. The oxidation state of hydrogen changes from 0 to +1. The reducing agent is Fe(s) The oxidizing agent is Cr3+(aq) The highest oxidation state for chromium in this reaction is +6