8.2 grams of calcium nitrate is decomposed by heating according to the equation $2 \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}$ $\_\_\_\_$ $\rightarrow 2 \mathrm{CaO}+4 \mathrm{NO}_{2}+\mathrm{O}_{2}$ Calculate the following: Mass of CaO formed [Atomic weights: $\mathrm{Ca}-40, \mathrm{~N}-14, \mathrm{O}-16$ ]
Explanation
First, we need to calculate the number of moles of calcium nitrate decomposed. The molar mass of calcium nitrate is 164 g/mol. So, the number of moles of calcium nitrate is 8.2 g / 164 g/mol = 0.05 mol. According to the equation, 2 moles of calcium nitrate produce 2 moles of calcium oxide. So, the number of moles of calcium oxide produced is 0.05 mol * 2 = 0.1 mol. The molar mass of calcium oxide is 56 g/mol. So, the mass of calcium oxide formed is 0.1 mol * 56 g/mol = 5.6 g. However, since the question asks for the mass of CaO formed from 8.2 grams of calcium nitrate, we need to consider the mass of CaO formed from 8.2 grams of calcium nitrate. The mass of CaO formed from 8.2 grams of calcium nitrate is 5.6 g * (8.2 g / 164 g) = 16.8 g.
⬆ Related Topic
📘 Syllabus
📝 Practice Questions
Practice Previous Year Questions →
🤖 Practice with AI
Generate Practice Question Paper →