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Chapter 4: Problem 53

Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid, (b) chromium with hydrobromic acid, (c) tin with hydrochloric acid, (d) aluminum with formic acid, HCOOH.

Short Answer

Expert verified
\( (a) \) Molecular: \(Mn + H_2SO_4 \rightarrow MnSO_4 + H_2 \) Net ionic: \(Mn + 2H^+ \rightarrow Mn^{2+} + H_2 \) \( (b) \) Molecular: \(2Cr + 6HBr \rightarrow 2CrBr_3 + 3H_2 \) Net ionic: \(2Cr + 6H^+ \rightarrow 2Cr^{3+} + 3H_2 \) \( (c) \) Molecular: \(Sn + 2HCl \rightarrow SnCl_2 + H_2 \) Net ionic: \(Sn + 2H^+ \rightarrow Sn^{2+} + H_2 \) \( (d) \) Molecular: \(2Al + 6HCOOH \rightarrow 2Al(HCOO)_3 + 3H_2 \) Net ionic: \(2Al + 6HCOOH \rightarrow 2Al(HCOO)_3 + 3H_2 \)

Step by step solution

01

(a) Manganese with dilute sulfuric acid: Molecular equation

First, write the unbalanced molecular equation: Mn + H2SO4 -> MnSO4 + H2. Now, balance the equation by ensuring equal numbers of each atom on both sides of the equation. The balanced molecular equation is: Mn + H2SO4 -> MnSO4 + H2.
02

(a) Manganese with dilute sulfuric acid: Net ionic equation

Separate all strong electrolytes into their ions: Mn + 2H^+ + SO4^2- -> Mn^2+ + SO4^2- + H2. Now write the net ionic equation by removing the spectator ions: Mn + 2H^+ -> Mn^2+ + H2.
03

(b) Chromium with hydrobromic acid: Molecular equation

Write the unbalanced molecular equation: Cr + HBr -> CrBr3 + H2. Now, balance the equation by ensuring equal numbers of each atom on both sides of the equation. The balanced molecular equation is: 2Cr + 6HBr -> 2CrBr3 + 3H2.
04

(b) Chromium with hydrobromic acid: Net ionic equation

Separate all strong electrolytes into their ions: 2Cr + 6H^+ + 6Br^- -> 2Cr^3+ + 6Br^- + 3H2. Now write the net ionic equation by removing the spectator ions: 2Cr + 6H^+ -> 2Cr^3+ + 3H2.
05

(c) Tin with hydrochloric acid: Molecular equation

Write the unbalanced molecular equation: Sn + HCl -> SnCl2 + H2. Now, balance the equation by ensuring equal numbers of each atom on both sides of the equation. The balanced molecular equation is: Sn + 2HCl -> SnCl2 + H2.
06

(c) Tin with hydrochloric acid: Net ionic equation

Separate all strong electrolytes into their ions: Sn + 2H^+ + 2Cl^- -> Sn^2+ + 2Cl^- + H2. Now write the net ionic equation by removing the spectator ions: Sn + 2H^+ -> Sn^2+ + H2.
07

(d) Aluminum with formic acid: Molecular equation

Write the unbalanced molecular equation: Al + HCOOH -> Al(HCOO)3 + H2. Now, balance the equation by ensuring equal numbers of each atom on both sides of the equation. The balanced molecular equation is: 2Al + 6HCOOH -> 2Al(HCOO)3 + 3H2.
08

(d) Aluminum with formic acid: Net ionic equation

In this reaction, formic acid does not dissociate completely, so we do not separate it into its ions. The complete ionic equation is the same as the molecular equation: 2Al + 6HCOOH -> 2Al(HCOO)3 + 3H2. The balanced net ionic equation is: 2Al + 6HCOOH -> 2Al(HCOO)3 + 3H2.

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Most popular questions from this chapter

A sample of \(7.75 \mathrm{~g}\) of \(\mathrm{Mg}(\mathrm{OH})_{2}\) is added to \(25.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HNO}_{3}\). (a) Write the chemical equation for the reaction that occurs. (b) Which is the limiting reactant in the reaction? (c) How many moles of \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{HNO}_{3}\), and \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) are present after the reaction is complete?

The metal cadmium tends to form \(\mathrm{Cd}^{2+}\) ions. The following observations are made: (i) When a strip of zinc metal is placed in \(\mathrm{CdCl}_{2}(a q)\), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\), nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the preceding observations. (b) Which elements more closely define the position of cadmium in the activity series? (c) What experiments would you need to perform to locate more precisely the position of cadmium in the activity series?

Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a), how could you distinguish any of the three magnesium substances from the other two?

Which element is oxidized and which is reduced in the following reactions? (a) \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)\) (b) \(3 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Al}(s) \longrightarrow\) (c) \(\mathrm{Cl}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{NaCl}(a q)+2 \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) (d) \(\mathrm{PbS}(\mathrm{s})+4 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{NaCl}(a q)\)

State whether each of the statements below is true or false. Justify your answer in each case. (a) Electrolyte solutions conduct electricity because electrons are moving through the solution. (b) If you add a nonelectrolyte to an aqueous solution that already contains an electrolyte, the electrical conductivity will not change.
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