Question

type the correct answer in each box. balance the chemical equation. □ n₂o₃ → □ n₂ + □ o₂

Explanation:

Step1: Analyze nitrogen atoms

On the left side, each \( \ce{N2O3} \) has 2 N atoms. On the right side, \( \ce{N2} \) has 2 N atoms. So the coefficient for \( \ce{N2O3} \) and \( \ce{N2} \) related to N should be balanced first. Let's assume the coefficient of \( \ce{N2O3} \) is \( x \), \( \ce{N2} \) is \( y \), then \( 2x = 2y \), so \( x = y \) for now.

Step2: Analyze oxygen atoms

On the left side, each \( \ce{N2O3} \) has 3 O atoms. On the right side, \( \ce{O2} \) has 2 O atoms. Let the coefficient of \( \ce{O2} \) be \( z \). So the number of O atoms: \( 3x = 2z \). We need to find the least common multiple of 3 and 2, which is 6. So if \( 3x = 6 \), then \( x = 2 \); and \( 2z = 6 \), then \( z = 3 \). And since \( x = y \), \( y = 2 \).

Step3: Verify the equation

Putting the coefficients: \( 2\ce{N2O3}
ightarrow 2\ce{N2} + 3\ce{O2} \). Check N: left \( 2\times2 = 4 \), right \( 2\times2 = 4 \). Check O: left \( 2\times3 = 6 \), right \( 3\times2 = 6 \). Balanced.

Answer:

2, 2, 3 (in the order of \( \ce{N2O3} \), \( \ce{N2} \), \( \ce{O2} \) coefficients)