Which of the following is best described as an oxidation-reduction reaction? Sol

Question

Which of the following is best described as an oxidation-reduction reaction?

Explanation / Answer

let us consider example Co(OH)2(s) + 2HCl(aq) ® CoCl2(aq) + 2H2O(l) Ca(s) + 2HCl(aq) ® CaCl2(aq) + H2(g) Fe(s) + 2AgNO3(aq) ® Fe(NO3)2(aq) + 2Ag(s) NH3(aq) + H2O(l) ® NH4+(aq) + OH-(aq) Cl2(g) + H2O(l) ® H+(aq) + Cl-(aq) + HOCl(aq) ans) A redox reaction is one in which two or more elements change oxidation states. In order to identify a redox reaction, start by assigning oxidation numbers to each element and see if any change. Co(OH)2(s) + 2HCl(aq) --> CoCl2(aq) + 2H2O(l) .... Not redox, no oxidation number changes. This one is double replacement, or acid-base. Take your pick. Acid-base neutralization reactions are a type of double replacement. Ca(s) + 2HCl(aq) -->CaCl2(aq) + H2(g) Fe(s) + 2AgNO3(aq) --> Fe(NO3)2(aq) + 2Ag(s) Both of these are redox. Calcium and iron metals are initially in the zero oxidation state and they are each oxidized to the +2 oxidation state, while hydrogen and silver are reduced to the elemental form. NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) ... not redox. Not even much of a reaction. The equilibrium will lie far to the left. Only a very few molecules of ammonia will actually react with water. Cl2(g) + H2O(l) --> H+(aq) + Cl-(aq) + HOCl(aq) ... redox. Cl2 undergoes a disproportionation reaction in which chlorine in Cl2 is both oxidized to +1 in HOCl, and reduced to Cl- where the oxidation number is -1.

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