Equation Number Balanced Equation 2 ZnS(s) + 3 0,(g) → 2 ZnO(s) + 2 SO, (g) Ag*(aq) + Br¯(aq) 1 AgBr(s) | 3 10 H*(aq) + SO, (aq) + 8I¬(aq) 4L, (s) + H, S(g) + 4 H,O(1) Classify each reactant in the chemical equations as an oxidizing agent, a reducing agent, or neither. Oxidizing agent Reducing agent Neither Answer Bank so;- Ag* H+ Br ZnS

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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Equation
Number
Balanced Equation
1
2 ZnS(s) + 3 O,(g)
2 ZnO(s) + 2 S0,(g)
Ag*(aq) + Br¯(aq)
10 H*(aq) + SO (aq) + 8 I¬(aq)
→ AgBr(s)
3
4 L, (s) + H, S(g) + 4 H, O(1)
Classify each reactant in the chemical equations as an oxidizing agent, a reducing agent, or neither.
Oxidizing agent
Reducing agent
Neither
Answer Bank
SO
Ag*
Br
ZnS
H+
Transcribed Image Text:Equation Number Balanced Equation 1 2 ZnS(s) + 3 O,(g) 2 ZnO(s) + 2 S0,(g) Ag*(aq) + Br¯(aq) 10 H*(aq) + SO (aq) + 8 I¬(aq) → AgBr(s) 3 4 L, (s) + H, S(g) + 4 H, O(1) Classify each reactant in the chemical equations as an oxidizing agent, a reducing agent, or neither. Oxidizing agent Reducing agent Neither Answer Bank SO Ag* Br ZnS H+
<>
so?-
Ag*
H+
I-
Br
ZnS
O2
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.
sulfur, beginning in the reactant ZnS
bromine, beginning in the reactant Br
iodine, beginning in the reactant I-
sulfur, beginning in the reactant SO
Transcribed Image Text:<> so?- Ag* H+ I- Br ZnS O2 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. sulfur, beginning in the reactant ZnS bromine, beginning in the reactant Br iodine, beginning in the reactant I- sulfur, beginning in the reactant SO
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