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------------------------------------------------ Determine the limiting reactant and calculate the number of grams of nitrogen dioxide (NO2) that can be formed when 105 g of nitrogen (N2) reacts with 98.5 g of oxygen (O2).

The limiting reactant in the reaction forming Nitrogen Dioxide (NO2) from Nitrogen (N2) and Oxygen (O2) is Oxygen. The quantity of NO2 that can be potentially created from supplied amounts of reactants is 141.68 grams.

Explanation:

In order to determine the limiting reactant and the quantity of NO2 produced, we need to first write a balanced chemical equation. For the formation of Nitrogen Dioxide from Nitrogen and Oxygen, the balanced chemical reaction equation is: N2 + 2O2 -> 2NO2.

Next, we find the number of moles for each reactant. Using molar mass, the number of moles of Nitrogen (N2) is 105g / 28g/mol = 3.75 mol. For Oxygen (O2), it is 98.5g / 32g/mol = 3.08 mol.

Comparing these values, we can see that Oxygen is less in molar quantity and so, is the limiting reactant. Now, we calculate the mass of NO2 produced. Since the stoichiometric ratio of O2 to NO2 is 1:1, the moles of NO2 produced are equal to the moles of O2 present. So, we have 3.08 mol NO2. Considering the molar mass of NO2 (46 g/mol), the mass comes out to be 3.08 mol * 46 g/mol = 141.68 g.

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