Final answer:
The decomposition of RbNO3 can result in different products depending on the reaction conditions, and alkali metal nitrates typically decompose into their metal oxides, nitrogen dioxide, and oxygen. For an accurate balanced equation, specific details regarding the decomposition conditions are necessary.
Step-by-step explanation:
The decomposition of RbNO3 (rubidium nitrate) would lead to the formation of rubidium nitrite (RbNO2) and oxygen (O2). However, typical nitrates of alkali metals like rubidium do not decompose into nitrites and oxygen as do nitrates of heavier metals; instead, they usually decompose into the nitrate's corresponding metal oxide, nitrogen dioxide, and oxygen. Therefore, since this behavior can be complex and context-dependent, I would need more specific information about the conditions of the decomposition to provide a precise equation.
Let's take a more generic example for illustrative purposes:
- Decomposition of potassium chlorate: 2 KClO3 → 3 O2 + 2 KCl.
In case of RbNO3, if we were to speculate a similar simple decomposition, a balanced chemical equation might be:
2 RbNO3 → 2 RbNO2 + O2.
However, this is just a hypothetical example and should not be taken as the actual decomposition of rubidium nitrate. Understanding the decomposition of such compounds requires knowledge of the specific conditions under which the reaction occurs.