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.

a. Ca + 2HCl → CaCl2 + H2

b. 2KOH + K2Cr2O7 → 2K2CrO4 + H2O

c. AgNO3 + KI → AgI + KNO3

d. 2PbS + 3O2 → 2PbO + 2SO2

Question

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. 

a. Ca + 2HCl → CaCl2 + H2 

b. 2KOH + K2Cr2O7 → 2K2CrO4 + H2O 

c. AgNO3 + KI → AgI + KNO3 

d. 2PbS + 3O2 → 2PbO + 2SO2

anonymous · Answer

I already did A but I am confused on the rest

anonymous · Answer

the question marks are arrows

jfraser · Answer

in order for a reaction to be a redox reaction, the $charges$ of the reactants and products must change.

#1 is a redox reaction, because the oxidation state of Ca changes from a 0 (as a neutral atom) to a +2 (as the ion in $CaCl_2$)