2. Identify the oxidation numbers for each element in the following equations. Then determine whether each equation describes a redox reaction. Justify your answer in terms of electron transfer. Describe the oxidation and reduction that occurs.

b. 2KOH + K2Cr2O7 → 2K2CrO4 + H2O

d. 2PbS + 3O2 → 2PbO + 2SO2

PLEASE I REALLY NEED HELP

Question

2. Identify the oxidation numbers for each element in the following equations. Then determine whether each equation describes a redox reaction. Justify your answer in terms of electron transfer. Describe the oxidation and reduction that occurs. 

b. 2KOH + K2Cr2O7 → 2K2CrO4 + H2O

d. 2PbS + 3O2 → 2PbO + 2SO2 

PLEASE I REALLY NEED HELP

chmvijay · Answer

can u find out the oxidation state of Cr on left and right

anonymous · Answer

No I don't know it at all

anonymous · Answer

do you know your rules for assigning oxidation states?

anonymous · Answer

All I know is that a lone element and an element in a diatomic gas have an oxidation state of 0.

jfraser · Answer

you should also remember that the sum of the oxidation states in a neutral compounds must always be zero. In PbO, for example, the lead is a +2, and the oxygen is a -2, adding up to zero.

The polyatomic ions are more difficult, but only because there are more pieces. The general rule is that oxygen ions are always -2. In the $Cr_2O_7$ ion there are seven of them, for a total negative charge of -14. The ion as a whole must have a -2 charge, which means the 2 chromium ions must provide a total charge of +12. There are 2 of them, so what's the easiest way to reach a +12 charge?

anonymous · Answer

Wait so what would be the answer then?