Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 56

Using the activity series (Table 4.5 ), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate, (b) a solution of zinc nitrate is added to a solution of magnesium sulfate, (c) hydrochloric acid is added to gold metal, (d) chromium metal is immersed in an aqueous solution of cobalt(II) chloride, (e) hydrogen gas is bubbled

Short Answer

Expert verified
(a) \(Ni(s) + Cu(NO_3)_2(aq) \rightarrow Ni(NO_3)_2(aq) + Cu(s)\) (b) NR (c) NR (d) \(Cr(s) + CoCl_2(aq) \rightarrow CrCl_2(aq) + Co(s)\) (e) NR

Step by step solution

01

Check activity series for Nickel and Copper

Refer to the activity series and find that Nickel (Ni) is more reactive than Copper (Cu). A reaction will occur.
02

Write the balanced chemical equation

The balanced chemical equation for this reaction is: \(Ni(s) + Cu(NO_3)_2(aq) \rightarrow Ni(NO_3)_2(aq) + Cu(s)\) Step 2: Reaction between a solution of zinc nitrate and a solution of magnesium sulfate
03

Check activity series for Zinc and Magnesium

Refer to the activity series and find that Zinc (Zn) is less reactive than Magnesium (Mg). No reaction will occur.
04

Write the balanced chemical equation

Since no reaction occurs, write NR. Step 3: Reaction between hydrochloric acid and gold metal
05

Check activity series for Hydrogen and Gold

Refer to the activity series and find that Hydrogen (H) is more reactive than Gold (Au). No reaction will occur.
06

Write the balanced chemical equation

Since no reaction occurs, write NR. Step 4: Reaction between chromium metal and an aqueous solution of cobalt(II) chloride
07

Check activity series for Chromium and Cobalt

Refer to the activity series and find that Chromium (Cr) is more reactive than Cobalt (Co). A reaction will occur.
08

Write the balanced chemical equation

The balanced chemical equation for this reaction is: \(Cr(s) + CoCl_2(aq) \rightarrow CrCl_2(aq) + Co(s)\) Step 5: Reaction between hydrogen gas and silver nitrate solution
09

Check activity series for Hydrogen and Silver

Refer to the activity series and find that Hydrogen (H) is more reactive than Silver (Ag). No reaction will occur.
10

Write the balanced chemical equation

Since no reaction occurs, write NR.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

(a) Which will have the highest concentration of sodium ions: \(0.25 \mathrm{MNaCl}, 0.15 \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3},\) or \(0.075 \mathrm{MNa}_{3} \mathrm{PO}_{4} ?(\mathbf{b})\) Which will contain the greater number of moles of sodium ion: \(20.0 \mathrm{~mL}\) of \(0.15 \mathrm{M} \mathrm{NaHCO}_{3}\) or $15.0 \mathrm{~mL}\( of \)0.04 \mathrm{M} \mathrm{Na}_{2} \mathrm{~S} ?$

Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, \(\mathrm{BaSO}_{4},\) (b) sulfurous acid, $\mathrm{H}_{2} \mathrm{SO}_{3},(\mathbf{c})\( strontium sulfide, \)\mathrm{Sr} S,(\mathbf{d})$ hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}\). (e) Locate sulfur in the periodic table in Exercise 4.47 what region is it in? (f) Which region(s) of the periodic table contains elements that can adopt both positive and negative oxidation numbers?

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) $3 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Al}(s) \longrightarrow$ $$ 3 \mathrm{Fe}(s)+2 \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q) $$ (c) $\mathrm{Cl}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{NaCl}(a q)$ (d) $\mathrm{PbS}(s)+4 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+4 \mathrm{H}_{2} \mathrm{O}(I)$

When carbon dioxide dissolves in water, it is in equilibrium with carbonic acid \(\mathrm{H}_{2} \mathrm{CO}_{3},\) which is a weak electrolyte. What solutes are present in aqueous solution of this compound? Write the chemical equation for the ionization of \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

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) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free