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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) Mn (s) + 2H+ (aq) -> Mn2+ (aq) + H2 (g) b) 2Cr (s) + 6H+ (aq) -> 2Cr3+ (aq) + 3H2 (g) c) Sn (s) + 2H+ (aq) -> Sn2+ (aq) + H2 (g) d) 2Al (s) + 6H+ (aq) -> 2Al3+ (aq) + 3H2 (g)

Step by step solution

01

Identify the reactants and their oxidation states

For each reaction, we need to identify the reactants and their possible oxidation states. They are as follows: a) Manganese (Mn): +2 b) Chromium (Cr): +3 c) Tin (Sn): +2 d) Aluminum (Al): +3
02

Write the balanced molecular equations

Now, let's write the balanced molecular equations for each reaction: a) Manganese with sulfuric acid Mn (s) + H2SO4 (aq) -> MnSO4 (aq) + H2 (g) b) Chromium with hydrobromic acid 2Cr (s) + 6HBr (aq) -> 2CrBr3 (aq) + 3H2 (g) c) Tin with hydrochloric acid Sn (s) + 2HCl (aq) -> SnCl2 (aq) + H2 (g) d) Aluminum with formic acid 2Al (s) + 6HCOOH (aq) -> 2Al(HCOO)3 (aq) + 3H2 (g)
03

Write the balanced net ionic equations

Now, we'll eliminate spectator ions from each balanced equation and write the net ionic equations: a) Manganese with sulfuric acid Mn (s) + 2H+ (aq) + SO42- (aq) -> Mn2+ (aq) + SO42- (aq) + H2 (g) Net ionic equation: Mn (s) + 2H+ (aq) -> Mn2+ (aq) + H2 (g) b) Chromium with hydrobromic acid 2Cr (s) + 6H+ (aq) + 6Br- (aq) -> 2Cr3+ (aq) + 6Br- (aq) + 3H2 (g) Net ionic equation: 2Cr (s) + 6H+ (aq) -> 2Cr3+ (aq) + 3H2 (g) c) Tin with hydrochloric acid Sn (s) + 2H+ (aq) + 2Cl- (aq) -> Sn2+ (aq) + 2Cl- (aq) + H2 (g) Net ionic equation: Sn (s) + 2H+ (aq) -> Sn2+ (aq) + H2 (g) d) Aluminum with formic acid 2Al (s) + 6HCOO- (aq) + 6H+ (aq) -> 2Al3+ (aq) + 6HCOO- (aq) + 3H2 (g) Net ionic equation: 2Al (s) + 6H+ (aq) -> 2Al3+ (aq) + 3H2 (g)

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Most popular questions from this chapter

Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) \(\mathrm{LiClO}_{4}\), (b) \(\mathrm{HClO}\) (c) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\) (propanol), (d) \(\mathrm{HClO}_{3}\), (e) \(\mathrm{CuSO}_{4}\), (f) \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) (sucrose).

Complete and balance the following molecular equations, and then write the net ionic equation for each: (a) \(\mathrm{HBr}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{HClO}_{4}(a q) \longrightarrow\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow\)

As \(\mathrm{K}_{2} \mathrm{O}\) dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. Write the molecular and net ionic equations for this reaction. Based on the definitions of acid and base, what ion is the base in this reaction? What is the acid? What is the spectator ion in the reaction?

Calculate (a) the number of grams of solute in \(0.250 \mathrm{~L}\) of \(0.175 \mathrm{M} \mathrm{KBr},\) (b) the molar concentration of a solution containing \(14.75 \mathrm{~g}\) of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) in \(1.375 \mathrm{~L},\) (c) the volume of \(1.50 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\) in milliliters that contains \(2.50 \mathrm{~g}\) of solute.

Consider the following reagents: zinc, copper, mercury (density \(13.6 \mathrm{~g} / \mathrm{mL}\) ), silver nitrate solution, nitric acid solution. (a) Given a \(500-\mathrm{mL}\) Erlenmeyer flask and a balloon can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon? (b) What is the theoretical yield of the substance that fills the balloon? (c) Can you combine two or more of the foregoing reagents to initiate a chemical reaction that will produce metallic silver? Write a balanced chemical equation to represent this process. What ions are left behind in solution? (d) What is the theoretical yield of silver?
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