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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

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Most popular questions from this chapter

Diatomic chlorine and sodium hydroxide(lye) are commodity chemicals produced in large quantities, along with diatomic hydrogen via the electrolysis of brine according to the following unbalanced equation:

\[NaCl\left( {aq} \right) + {H_2}O\left( l \right) \to NaOH\left( {aq} \right) + {H_2}\left( g \right) + C{l_2}\left( g \right).\]

Write balanced molecular, complete ionic, and net ionic equations for this process.

What is the percent yield of a reaction that produces 12.5g of the gas freon CF2Cl2 from 32.9 g of CCl4 and excess HF.

\(CC{l_4} + 2HF \to C{F_2}\)

Colourful fireworks often involve the decomposition of barium nitrate and potassium chlorate and the reaction of metals magnesium, aluminium, and iron with oxygen.

(a)Write the formulae of barium nitrate and potassium chlorate.

(b)The decomposition of solid potassium chlorate leads to the formation of solid potassium chloride and diatomic oxygen gas. Write an equation for the reaction.

(c) The decomposition of solid barium nitrate leads to the formation of solid barium oxide, diatomic nitrogen gas and diatomic oxygen gas. Write an equation for the reaction.

(d)Write separate equations for the reactions of the solid metals magnesium, aluminium and iron and oxygen gas to yield the corresponding metal oxides.(Assume the iron oxide contains \(F{e^{3 + }}\)ions.)

Complete and balance each of the following oxidation-reduction reactions, such that it results in the highest possible oxidation states for the oxidizing atoms:

(a)\(K\left( s \right) + {H_2}O\left( l \right) \to \)

(b)\(Ba\left( s \right) + HBr\left( {aq} \right) \to \)

(c) \(Sn\left( s \right) + {I_2}\left( s \right) \to \)

What volume of 0.0105-M HBr solution is required to titrate 125 mL of a 0.0100-MCa(OH)2 solution?

Ca(OH)2(aq) + 2HBr(aq)⟶CaBr2(aq) + 2H2 O(l)

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