Balance the redox reaction occurring in an acidic aqueous solution. Au^3+(aq) +
ID: 752476 • Letter: B
Question
Balance the redox reaction occurring in an acidic aqueous solution. Au^3+(aq) + Cr^3+(aq) -->Au(s) +Cr2O7^2-(aq)Explanation / Answer
2) These are right 10) Be careful wiht this one. If a substance increases its oxidation number, then it is LOSING electrons because electrons are negative. Check out this example: Mg + O ---> MgO The oxidation # of Mg increases, going from 0 to 2+; therefore it lost electrons. If it lost electrons it was oxidized, but that means it is the reducing agent. So you have the two answers reversed. This is always confusing for people. Try to remember LEO goes GER; lose electrons oxidized; gain electrons reduced; then the opposite for naming the agents (reducing and oxidizing respectively) Note that if you are adding electrons to a compound, its ox# will get more and more negative, which means it is getting smaller and smaller. So if the ox# is decreasing it is gaining electrons and teh oxidizing agent. 14) Good job! These are right. 24) I can't remember what the oxidation number method is. I think you ust have to make sure the charges are balanced too. This looks right to me, but honestly I am not positive. I need to do some review! 36) Looks good to me. 40) I don't have a table with me, so I am not postive, but these look right by first glance. For D I think it would be the H2, but again, I don't have a table with me, so double check it. 54) Good! Looks right. 60) Perfect! 66) For this they are looking for the net ionic equation, so just put the reaction that occurs between the ions. So split Au(O2CCH3)3 and Hg(O2CCH3)2 into their ions and only include the ions that change in oxidation number for the equation I think. 70) i think this is okay too. You did a great job! It seems like you have a good understanding of electrochem. Don't be too discouraged about struggling with these. I tutor college chemistry and electrochem is hard for a lot people.
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