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Chapter 8: Problem 13

How does the process of balancing an equation illustrate the law of conservation of mass?

Short Answer

Expert verified
Balancing a chemical equation illustrates the law of conservation of mass by ensuring that the number of atoms for each element in the reactants (before the reaction) is the same as in the products (after the reaction). This shows that in a closed system, matter is neither created nor destroyed, but only changes form, in accordance with this fundamental law.

Step by step solution

01

Understand the Law of Conservation of Mass

This law, sometimes also called the principle of mass or matter conservation, states that the mass of a closed system will remain constant over time, regardless of the processes happening within. It basically means that in an isolated system, matter cannot be created or destroyed but only transformed.
02

Examining a Chemical Equation

A chemical equation is a symbolic representation of a chemical reaction in terms of chemical formulas. It includes reactants (substances before the reaction) on the left hand and products (substances after the reaction) on the right hand. An arrow in between symbolizes the transition from reactants to products.
03

Balancing a Chemical Equation

Balancing a chemical equation means making sure that the number of atoms of each element is the same on both sides of the equation. This is done by putting coefficients (the numbers in front of the compounds) to adjust the number of atoms.
04

Connection to the Law of Conservation of Mass

The process of balancing the equation is a clear illustration of the law of conservation of mass. When a chemical equation is balanced, the mass of the reactants (the initial substances) equals the mass of the product (the resulting substances). No atoms are lost or created during a chemical reaction, they are just rearranged, which exactly matches the postulates of the law of conservation of mass.

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Most popular questions from this chapter

Write a balanced equation for each of the following: a. iron(III) oxide + magnesium \(\rightarrow\) magnesium oxide + iron b. nitrogen dioxide + water \(\longrightarrow\) nitric acid + nitrogen monoxide c. silicon tetrachloride + water \(\rightarrow\) silicon dioxide + hydrochloric acid

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." $$ \begin{array}{l}{\text { a. } \mathrm{C}_{2} \mathrm{H}_{6}+\mathrm{O}_{2} \rightarrow} \\ {\text { b. } \mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{Al} \rightarrow} \\ {\text { c. } \mathrm{N}_{2}+\mathrm{Mg} \rightarrow} \\\ {\text { d. } \mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow} \\ {\text { e. } \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{SO}_{4} \longrightarrow}\end{array} $$

Use the activity series to predict whether the following reactions are possible. Explain your answers. $$\text {a}.\mathrm{Ni}(s)+\mathrm{MgSO}_{4}(a q) \longrightarrow{\mathrm{NiSO}_{4}(a q)+\mathrm{Mg}(s)}$$ $$\begin{array}{r}{\text { b. } 3 \mathrm{Mg}(s)+\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q) \longrightarrow} {3 \mathrm{MgSO}_{4}(a q)+2 \mathrm{Al}(s)}\end{array}$$ $$\text{c} \cdot \mathrm{Pb}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow{\mathrm{Pb}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{2}(g)} $$

Write a balanced equation for each of the following: $$\begin{array}{c}{\text { a. copper(II) sulfate }+\text { ammonium sulfide } \rightarrow} \\ {\text { copper(II) sulfide + ammonium sulfate }} \\ {\text { b. nitric acid + barium hydroxide } \rightarrow} \\ {\text { water + barium nitrate }}\end{array}$$ $$ \begin{array}{c}{\text { c. barium chloride + phosphoric acid } \rightarrow} \\\ {\text { barium phosphate + hydrochloric acid }}\end{array} $$

Describe the trend in bond length as you move down the elements in Group 17 on the periodic table.
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