Question

type coefficients in each blank to balance the chemical equation below:
? p₄ + ? o₂ ⟶ ? p₂o₃
once the equation above is balanced, type in the number of each atom below:
reactants
atom amount
p 8
o 12
products
atom amount
p
o 12

Explanation:

Step1: Balance phosphorus atoms

Let the coefficient of \(P_4\) be \(x\), and the coefficient of \(P_2O_3\) be \(y\). For phosphorus atoms, from \(P_4\) and \(P_2O_3\), we have \(4x = 2y\). If we assume \(x = 2\), then \(y=4\).

Step2: Balance oxygen atoms

The coefficient of \(P_4\) is \(2\), the coefficient of \(P_2O_3\) is \(4\). For oxygen atoms, let the coefficient of \(O_2\) be \(z\). From \(O_2\) and \(P_2O_3\), we have \(2z=3\times4\), so \(z = 6\).

Answer:

The balanced equation is \(2P_4+6O_2
ightarrow4P_2O_3\).
For the products:

• The number of \(P\) atoms is \(8\) (since \(4\times2\) in \(P_2O_3\))
• The number of \(O\) atoms is \(12\) (since \(4\times3\) in \(P_2O_3\))