How to Balance Chemical Equations Using Linear Algebra

Download Article

Explore this Article

Steps

Steps

Other Sections

Related Articles

Expert Interview

Download Article

Balancing chemical equations is typically done by first identifying uncommon elements in compounds and working your way towards hydrogen and oxygen. There is also a slower but more systematic approach using linear algebra.

Steps

Download Article

1. 1
   Identify the equation to balance.

   • ${\begin{aligned}&\mathrm {H} _{3}\mathrm {PO} _{4}+(\mathrm {NH} _{4})_{2}\mathrm {MoO} _{4}+\mathrm {HNO} _{3}\\&\to (\mathrm {NH} _{4})_{3}\mathrm {PO} _{4}\cdot 12\,\mathrm {MoO} _{3}+\mathrm {NH} _{4}\mathrm {NO} _{3}+\mathrm {H} _{2}\mathrm {O} \end{aligned}}$
2. 2
   Identify the elements. The number of elements present in the equation determines how many rows will be in the vectors and matrices that we are going to construct. Below, the order we list corresponds to the order of the rows.

   • $\mathrm {H}$ – Hydrogen
   • $\mathrm {P}$ – Phosphorus
   • $\mathrm {O}$ – Oxygen
   • $\mathrm {N}$ – Nitrogen
   • $\mathrm {Mo}$ – Molybdenum
   Advertisement
3. 3
   Set up the vector equation. The vector equation consists of column vectors corresponding to each compound in the equation. Each vector has a corresponding coefficient, labeled $x_{1}$ to $x_{6},$ for which we are solving for. Make sure you understand how to count the number of atoms in a molecule.

   • $x_{1}{\begin{pmatrix}3\\1\\4\\0\\0\end{pmatrix}}+x_{2}{\begin{pmatrix}8\\0\\4\\2\\1\end{pmatrix}}+x_{3}{\begin{pmatrix}1\\0\\3\\1\\0\end{pmatrix}}=x_{4}{\begin{pmatrix}12\\1\\40\\3\\12\end{pmatrix}}+x_{5}{\begin{pmatrix}4\\0\\3\\2\\0\end{pmatrix}}+x_{6}{\begin{pmatrix}2\\0\\1\\0\\0\end{pmatrix}}$
4. 4
   Set the equation to 0 and obtain the augmented matrix. There are two major points to consider here. First, recognize that a vector equation like the one above has the same solution set as a linear system with its corresponding augmented matrix. This is a fundamental idea in linear algebra. Second, when the augments are all 0, row-reduction does not change the augments. Therefore, we need not write them at all – row-reducing the coefficient matrix is all that is necessary.

   • Note that moving everything to the left side causes the elements on the right side to negate.
   • ${\begin{pmatrix}3&8&1&-12&-4&-2\\1&0&0&-1&0&0\\4&4&3&-40&-3&-1\\0&2&1&-3&-2&0\\0&1&0&-12&0&0\end{pmatrix}}$
5. 5
   Row-reduce to reduced row-echelon form. For such a matrix, it is recommended that you use a calculator, although row-reducing by hand is always an option, albeit slower.

   • ${\begin{pmatrix}1&0&0&0&0&-1/12\\0&1&0&0&0&-1\\0&0&1&0&0&-7/4\\0&0&0&1&0&-1/12\\0&0&0&0&1&-7/4\end{pmatrix}}$
   • It is clear that there is a free variable $x_{6}$ here. Those with sharp minds would've seen this coming, for there are more variables than equations, and hence more columns than rows. This free variable means that $x_{6}$ can take on any value, and the resulting combination of $x_{1}$ to $x_{5}$ would be a valid solution (to our linear system, that is – the chemical equation results in further restrictions in this solution set).
6. 6
   Reparameterize the free variable and solve for the variables. Let's set $x_{6}=t.$ Since for positive values of $t,$ none of the variables become negative, so we are on the right track.

   • $x_{1}=t/12$
   • $x_{2}=t$
   • $x_{3}=7t/4$
   • $x_{4}=t/12$
   • $x_{5}=7t/4$
   • $x_{6}=t$
7. 7
   Substitute an appropriate value for $$ t {\displaystyle t} . Remember that the coefficients in the chemical equation must be integers. Therefore, set $t=12,$ the least common multiple. From our solution set, it is clear that while there are an infinite number of solutions, as we would expect, it is nonetheless a countably infinite set.

   • $x_{1}=1$
   • $x_{2}=12$
   • $x_{3}=21$
   • $x_{4}=1$
   • $x_{5}=21$
   • $x_{6}=12$
8. 8
   Substitute the coefficients into the chemical equation. The equation is now balanced.

   • ${\begin{aligned}&\mathrm {H} _{3}\mathrm {PO} _{4}+12\,(\mathrm {NH} _{4})_{2}\mathrm {MoO} _{4}+21\,\mathrm {HNO} _{3}\\&\to (\mathrm {NH} _{4})_{3}\mathrm {PO} _{4}\cdot 12\,\mathrm {MoO} _{3}+21\,\mathrm {NH} _{4}\mathrm {NO} _{3}+12\,\mathrm {H} _{2}\mathrm {O} \end{aligned}}$
Advertisement

Expert Q&A

Search

Add New Question

Ask a Question

200 characters left

Include your email address to get a message when this question is answered.

Submit

Advertisement

Tips

Submit a Tip

All tip submissions are carefully reviewed before being published

Submit

Thanks for submitting a tip for review!

Expert Interview

Thanks for reading our article! If you’d like to learn more about chemistry, check out our in-depth interview with Anne Schmidt.