When 2 mol of an alkaline earth metal nitrate is decomposed on heating, find the number of gaseous
moles in the product.

To determine the number of gaseous moles produced when 2 moles of an alkaline earth metal nitrate decompose upon heating, we first need to understand the decomposition reaction of alkaline earth metal nitrates. The general formula for an alkaline earth metal nitrate can be represented as M(NO3)2, where M stands for the alkaline earth metal. When these nitrates decompose, they typically break down into the corresponding metal oxide, nitrogen dioxide, and oxygen gas.

The Decomposition Reaction

The decomposition of alkaline earth metal nitrates can be represented by the following balanced chemical equation:

M(NO3)2 (s) → MO (s) + 2 NO2 (g) + 0.5 O2 (g)

Breaking Down the Reaction

From the equation, we can see that one mole of M(NO3)2 produces:

• 1 mole of MO (solid)
• 2 moles of NO2 (gas)
• 0.5 moles of O2 (gas)

Calculating Moles from the Reaction

Now, since we start with 2 moles of M(NO3)2, we can calculate the total moles of gaseous products produced:

• From 2 moles of M(NO3)2, we get:
• 2 moles of MO (solid) - not counted as gas
• 2 moles of M(NO3)2 produce 2 × 2 = 4 moles of NO2 (gas)
• 2 moles of M(NO3)2 produce 2 × 0.5 = 1 mole of O2 (gas)

Summing Up the Gaseous Products

Now, we add the moles of the gaseous products together:

Total gaseous moles = moles of NO2 + moles of O2

Total gaseous moles = 4 moles (NO2) + 1 mole (O2) = 5 moles

Final Result

Therefore, when 2 moles of an alkaline earth metal nitrate decompose upon heating, a total of 5 moles of gaseous products are formed. This includes 4 moles of nitrogen dioxide and 1 mole of oxygen gas.