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Chapter 8: Problem 2

How does a coefficient in front of a formula affect the number of each type of atom in the formula?

Short Answer

Expert verified
A coefficient in front of a chemical formula multiplies the number of each type of atom in the formula by the coefficient. So in an example like '2 \(H_2O\)', we would end up with 4 Hydrogen atoms and 2 Oxygen atoms.

Step by step solution

01

Understanding the basic concept of a chemical formula

Consider any chemical formula, for instance \( H_2O \), which represents water. In this formula, the subscript after each element represents the number of atoms of that element in one molecule of the substance. These subscripts are not affected by the coefficient in front.
02

Identifying the effect of coefficient

If a coefficient is placed before the formula, say '2 \(H_2O\)', that coefficient applies to the entire molecule including all the atoms present in that molecule. So this means we now have 2 water molecules, which corresponds to 4 Hydrogen atoms (\(2*2H\)) and 2 Oxygen atoms (\(2*1O\)).
03

Generalizing the principle

In general, a coefficient, say 'n', in front of a formula multiplies the entire formula, thereby multiplying the quantity of each individual atom by n.

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Most popular questions from this chapter

Evaporating ocean water leaves a mixture of salts. Is this a chemical change? Explain.

Identify the type of reaction for each of the following. Then, predict products for the reaction and balance the equation. If no reaction occurs, write "no reaction." $$ \begin{array}{l}{\text { a. } \mathrm{C}_{2} \mathrm{H}_{6}+\mathrm{O}_{2} \rightarrow} \\ {\text { b. } \mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{Al} \rightarrow} \\ {\text { c. } \mathrm{N}_{2}+\mathrm{Mg} \rightarrow} \\\ {\text { d. } \mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow} \\ {\text { e. } \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{SO}_{4} \longrightarrow}\end{array} $$

Write an unbalanced chemical equation for each of the following. $$\begin{array}{l}{\text { a. Aluminum reacts with oxygen to produce }} \\\ {\text { aluminum oxide. }} \\ {\text { b. Phosphoric acid, } \mathrm{H}_{3} \mathrm{PO}_{4} \text { , is produced }} \\ {\text { through the reaction between tetraphosphorus}} \\ {\text { decoxide and water. }}\end{array}$$

How do total and net ionic equations differ?

Complete and balance the equation for the complete combustion of each of the following. $$ \begin{array}{ll}{\text { a. } C_{3} \mathrm{H}_{6}} & {\text { c. } C \mathrm{H}_{3} \mathrm{OH}} \\ {\text { b. } C_{5} \mathrm{H}_{12}} & {\text { d. } C_{12} \mathrm{H}_{22} \mathrm{O}_{11}}\end{array} $$
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