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Chapter 18: Q97 E (page 1047)

Write two balanced chemical equations in which sulfuric acid acts as an oxidizing agent.

Short Answer

Expert verified

The two balanced chemical equations are:

\(\begin{array}{l}{\rm{1) Sn}}(s) + 2{{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}(aq) \to {\rm{S}}{{\rm{O}}_2}(g) + 2{{\rm{H}}_2}{\rm{O}}(l) + S{\rm{O}}_4^{2 - }(aq) + {\rm{S}}{{\rm{n}}^{2 + }}(aq).\\2)C(s) + 2{H_2}{\rm{S}}{{\rm{O}}_4}(aq) \to {\rm{C}}{{\rm{O}}_2}(g) + 2{\rm{S}}{{\rm{O}}_2}(g) + 2{{\rm{H}}_2}{\rm{O}}(l).\end{array}\)

Step by step solution

01

To write the two balanced chemical equations in which the sulfuric acid acts as an oxidizing agent.

The two balanced chemical equations are:

\(\begin{array}{l}{\rm{1) Sn}}(s) + 2{{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}(aq) \to {\rm{S}}{{\rm{O}}_2}(g) + 2{{\rm{H}}_2}{\rm{O}}(l) + S{\rm{O}}_4^{2 - }(aq) + {\rm{S}}{{\rm{n}}^{2 + }}(aq).\\2)C(s) + 2{H_2}{\rm{S}}{{\rm{O}}_4}(aq) \to {\rm{C}}{{\rm{O}}_2}(g) + 2{\rm{S}}{{\rm{O}}_2}(g) + 2{{\rm{H}}_2}{\rm{O}}(l).\end{array}\)

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Most popular questions from this chapter

Write balanced chemical equations for the following reactions:

(a) cadmium burned in air

(b) elemental cadmium added to a solution of hydrochloric acid

(c) cadmium hydroxide added to a solution of acetic acid, \({\rm{C}}{{\rm{H}}_3}{\rm{C}}{{\rm{O}}_2}{\rm{H}}\)

Why is it necessary to keep the chlorine and sodium, resulting from the electrolysis of sodium chloride, separate during the production of sodium metal?

What mass of magnesium forms when \({\bf{100}},{\bf{000}}{\rm{ }}{\bf{A}}\) is passed through a \({\bf{MgC}}{{\bf{l}}_2}\)melt for \({\bf{1}}.{\bf{00}}{\rm{ }}{\bf{h}}\) if the yield of magnesium is \({\bf{85}}\% \) of the theoretical yield?

Why does white phosphorus consist of tetrahedral \({P_4}\)molecules while nitrogen consists of diatomic \({N_2}\) molecules?

Why does phosphorous acid form only two series of salts, even though the molecule contains three hydrogen atoms?
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