Question

Heating \( \text{Ba(NO}_3\text{)}_2 \) produces:

• A. \( \text{N}_2 \)
• B. \( \text{BaO} + \text{NO}_2 + \text{O}_2 \)
• C. \( \text{N}_2\text{O} \)
• D. \( \text{NO}_2 \)

Hint:

All alkaline earth metal nitrates decompose on heating to give a metal oxide, brown fumes of \( \text{NO}_2 \), and \( \text{O}_2 \). In contrast, alkali metal nitrates (except \( \text{LiNO}_3 \)) decompose to give metal nitrites and oxygen gas.

Answer 1

The Correct Option is B

Step 1: Place barium.
Barium sits in group 2, the alkaline earth metals. Their nitrates all break down in the same pattern when heated.

Step 2: Write the general decomposition.
For any group 2 nitrate the heated reaction is:
\[ 2M(NO_3)_2 \xrightarrow{\Delta} 2MO + 4NO_2 + O_2 \]

Step 3: Put barium into it.
Replacing M with barium gives:
\[ 2Ba(NO_3)_2 \xrightarrow{\Delta} 2BaO + 4NO_2 + O_2 \]
So we get the oxide, brown nitrogen dioxide fumes and oxygen gas.

Step 4: Match with the options.
The products are $BaO$, $NO_2$ and $O_2$ together.
\[ \boxed{BaO + NO_2 + O_2} \]