Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Write a balanced molecular equation describing each of the following chemical reactions.

(a) Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas

(b)Gaseous butane reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor

(c)Aqueous solution of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride

(d) Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.

Short Answer

Expert verified
  1. \(CaC{O_3}\xrightarrow{\Delta }CaO + C{O_2}\)

  2. \(2{C_4}{H_{10}}\left( g \right) + 13{O_2}\left( g \right) \to 8C{O_2}\left( g \right) + 10{H_2}O\left( g \right)\)
  3. \(MgC{l_2}\left( {aq} \right) + 2NaOH\left( {aq} \right) \to Mg{\left( {OH} \right)_2}\left( s \right) + 2NaCl\left( {aq} \right)\)
  4. \(2{H_2}O\left( g \right) + Na\left( s \right) \to 2NaOH\left( s \right) + {H_2}\left( g \right)\)

Step by step solution

01

Consider all the elements in reaction (a)

The reaction has equal numbers of atoms in the reactant and products of the reaction. Hence balancing is not required.

\(CaC{O_3}\xrightarrow{\Delta }CaO + C{O_2}\)


Draw the balancing table to check:

Element

Reactant

Product

Balanced? yes

Ca

1×1

1×1

1=1

C

1×1

1×1

1=1

O

1×3

1×1+1×2

3=3

02

Consider the elements in reaction (b)

Calculate the atoms in the reactants and products of the given reaction. Use small integer coefficients for the formula to balance the equation.

\(2{C_4}{H_{10}}\left( g \right) + 13{O_2}\left( g \right) \to 8C{O_2}\left( g \right) + 10{H_2}O\left( g \right)\)

Draw the balancing table to check: Vary coefficients, not subscripts in the formula.

Element

Reactant

Product

Balanced? yes

C

2×4

8×1

8=8

H

2×10

10×2

20=20

O

13×2

8×2+10×1

26=26

03

Consider the elements in the reaction (c)

Calculate the type and numbers of atoms in the reactants and products of the reaction. Use integer coefficients of the formula; subscripts are kept constant.

\(MgC{l_2}\left( {aq} \right) + 2NaOH\left( {aq} \right) \to Mg{\left( {OH} \right)_2}\left( s \right) + 2NaCl\left( {aq} \right)\)

Draw the balancing table to check: Vary coefficients, not subscripts in the formula

Element

Reactant

Product

Balanced? yes

Mg

1×1

1×1

1=1

Na

2×1

2×1

2=2

Cl

2×1

2×1

2=2

O

2×1

1×2

2=2

H

2×1

1×2

2=2

04

Determine the elements in reaction (d)

Calculate the types and numbers of atoms in the reactants and products of the reaction. Use coefficients of the formula, but subscripts cannot be changed.

\(2{H_2}O\left( g \right) + 2Na\left( s \right) \to 2NaOH\left( s \right) + {H_2}\left( g \right)\)

Draw the balancing table to check:

Element

Reactant

Product

Balanced? yes

Na

2×1

2×1

2=2

H

2×2

2×1+1×2

4=4

O

2×1

2×1

2=2

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.

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

What volume of a 0.00945 M solution of potassium hydroxide would be required to titrate 50.00 mL of a sample of acid rain with a H2SO4 concentration of 1.23×10-4M

\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + 2KO}}{{\rm{H}}_{({\rm{aq}})}}{\rm{ }} \to {\rm{ }}{{\rm{K}}_2}{\rm{S}}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + 2}}{{\rm{H}}_2}{{\rm{O}}_{{\rm{(l)}}}}\)

Identify the atoms that are oxidized and reduced, the change in the oxidation state for each, and the oxidizing and reducing agents in each of the following equations:

(a)\(Mg\left( s \right) + NiC{l_2}\left( {aq} \right) \to MgC{l_2}\left( {aq} \right) + Ni\left( s \right)\)

(b)\(PC{l_3}\left( l \right) + C{l_2}\left( g \right) \to PC{l_5}\left( s \right)\)

(c)\({C_2}{H_4}\left( g \right) + 3{O_2}\left( g \right) \to 2C{O_2}\left( g \right) + 2{H_2}O\left( g \right)\)

(d)\(Zn\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to ZnS{O_4}\left( {aq} \right) + {H_2}\left( g \right)\)

(e) \(2{K_2}{S_2}{O_3}\left( s \right) + {I_2}\left( s \right) \to {K_2}{S_4}{O_6}\left( s \right) + 2KI\left( s \right)\)

(f) \(3Cu\left( s \right) + 8HN{O_3}\left( {aq} \right) \to 3Cu{\left( {N{O_3}} \right)_2}\left( {aq} \right) + 2NO\left( g \right) + 4{H_2}O\left( l \right)\)

Complete and balance each of the following oxidation-reduction reactions,such that it results in the highest possible oxidation state for the oxidized atoms.

(a) \(Al\left( s \right) + {F_2}\left( g \right) \to \)

(b) \(Al\left( s \right) + CuB{r_2}\left( {aq} \right) \to \) (single displacement)

(c) \({P_4}\left( s \right) + {O_2}\left( g \right) \to \)

(d) \(Ca\left( s \right) + {H_2}O\left( l \right) \to \) (products are a strong base and a diatomic gas)

How many moles of Ca(OH)2 are required to react with 1.36 mol of H3PO4 to produce Ca3(PO4)2 according to the equation \(3Ca{\left( {OH} \right)_2} + 2{H_3}P{O_4} \to C{a_3}{\left( {P{O_4}} \right)_2} + 6{H_2}O\)?

What does it mean to say an equation is balanced? Why is it important for an equation to be balanced?

See all solutions

Recommended explanations on Chemistry Textbooks

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