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In each of the following, identify the reactant that is oxidized and the reactant that is reduced:
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Chapter 8 Solutions
EP BASIC CHEMISTRY-MODIFIED MASTERING
- For each reaction, indicate which elements are oxidized and which are reduced: a.2Al+3CU2+2Al3++3Cub.2H++NiNi2++H2c.2I-+Cl2I2+2Cl-arrow_forwardIdentify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in each of the following equations: (a) Mg(s)+NiCl2(aq)MgCl2(aq)+Ni(s) (b) PCl3(l)+Cl2(g)PCl5(s) (c) C2H4(g)+3O2(g)2CO2(g)+2H2O(g) (d) Zn(s)+H2SO4(aq)ZnSO4(aq)+H2(g) (e) 2K2S2O3(s)+I2(s)K2S4O6(s)+2KI(s) (f) 3Cu(s)+8HNO3(aq)3Cu( NO3)2(aq)+2NO(g)+4H2O(l)arrow_forwardWrite equations for respiration and photosynthesis. For each reaction, label the substances that are oxidized and reduced. Why are these reactions important?arrow_forward
- Bromine is obtained from sea water by the following redox reaction: Cl2(g) + 2 NaBr(aq) 2 NaCl(aq) + Br2() (a) What has been oxidized? What has been reduced? (b) Identify the oxidizing and reducing agents.arrow_forward4.3 Explain the difference between complete and incomplete combustion.arrow_forwardConsider the reaction between oxygen (O2) gas and magnesium metal to form magnesium oxide. Using oxidation states, how many electrons would each oxygen atom gain, and how many electrons would each magnesium atom lose? How many magnesium atoms are needed to react with one oxygen molecule? Write a balanced equation for this reaction.arrow_forward
- Oxidation of 1.00 g of carbon monoxide, CO, produces 1.57 g of carbon dioxide, CO2. How many grams of oxygen were required in this reaction?arrow_forward10 Consider the reaction: H2(g) + Cl2(g) → 2HCl(g) Hydrogen is getting ______________. Group of answer choices oxidized reducedarrow_forwardFor each of the following reactions, identify the elements that are oxidized and reduced, the oxidizing and reducing agents, and how many moles of electrons are transferred in the overall reaction. a. 4Fe(s) + 302(g) → 2Fe2O3(s) b. 2Ag(s) + H2S(g) → Ag2S(s) + H2(g) c. 2 Al(s) + 3 CuCl2(aq) → 2 AlCl3(aq) + 3 Cu(s) d. 2NaHCO3(s) → Na2CO3(s) + H20(1) + CO2(g) e. CH4(g) + 2 02(g) → CO2(g) + 2H2O(1)arrow_forward
- H2.arrow_forwardWhich substance is oxidized in each reaction? a) 2Zn(s) + O2(g) = 2ZnO(g) b) CH4(g) + 2 O2(g) = CO2(g) + H2O(g) c) Sr(s) + F2(g) = SrF2(s)arrow_forwardIdentify the reactant that is being reduced, the reactant that is being oxidized, the reducing agent, the oxidizing agent, and determine how many electrons have been transferred from one atom to another in the following equation. Al + P → AlP Aluminum: Phosphorus: Determine the oxidation number of each element in aluminum phosphide. Al: P:arrow_forward
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