tudy the chemical equations in the table. Equation Number Balanced Equation 1 2Al(s)+3Cl2(g)⟶2Al3+(aq)+6Cl−(aq) 2 Ag+(aq)+Br−(aq)⟶AgBr(s) 3 4H+(aq)+2Cl−(aq)+MnO2(s)⟶Mn2+(aq)+Cl2(g)+2H2O(l) Classify each reactant in the chemical equations as an oxidizing agent, a reducing agent, or neither.   Br-, Cl-, Ag+, Cl2. MnO2, H+, and Al   Calculate the increase or decrease in the oxidation state for each element listed as it changes from a reactant to a product. Use a negative sign to show a decrease in oxidation state.   aluminum, beginning in the reactant Al     bromine, beginning in the reactant Br−     chlorine, beginning in the reactant Cl−     manganese, beginning in the reactant MnO

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Study the chemical equations in the table.

Equation Number Balanced Equation
1 2Al(s)+3Cl2(g)⟶2Al3+(aq)+6Cl−(aq)
2 Ag+(aq)+Br−(aq)⟶AgBr(s)
3 4H+(aq)+2Cl−(aq)+MnO2(s)⟶Mn2+(aq)+Cl2(g)+2H2O(l)
Classify each reactant in the chemical equations as an oxidizing agent, a reducing agent, or neither.
 
Br-, Cl-, Ag+, Cl2. MnO2, H+, and Al
 
Calculate the increase or decrease in the oxidation state for each element listed as it changes from a reactant to a product. Use a negative sign to show a decrease in oxidation state.
 
aluminum, beginning in the reactant Al
 
 
bromine, beginning in the reactant Br−
 
 
chlorine, beginning in the reactant Cl−
 
 
manganese, beginning in the reactant MnO2
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