Use the balanced equation, 2NO + O2 - 2NO2, to answer the following questions.
Part 1 of 3
Determine the limiting reactant. Select the single best answer.
5.00 mol NO
4.50 mol O2
Part: 1 / 3
Part 2 of 3
How many moles of the product NO2 form? Be sure your answer has the correct number of significant figures.
mol NO2
Copilot
To determine the limiting reactant, we need to compare the mole ratio of the reactants with the coefficients in the balanced chemical equation. The balanced equation is:
2
𝑁
𝑂
+
𝑂
2
→
2
𝑁
𝑂
2
2NO+O2→2NO2
This indicates that 2 moles of NO react with 1 mole of O2 to produce 2 moles of NO2.
Given:
5.00 mol NO
4.50 mol O2
We can calculate the amount of NO that would react with the given amount of O2:
4.50
mol O
2
×
2
mol NO
1
mol O
2
=
9.00
mol NO
4.50 mol O2×1 mol O22 mol NO=9.00 mol NO
Since only 5.00 mol of NO is available, which is less than the 9.00 mol required to react with all of the O2, NO is the limiting reactant.
Part 2 of 3:
To find out how many moles of NO2 form, we use the stoichiometry of the reaction based on the limiting reactant, which is NO:
5.00
mol NO
×
2
mol NO
2
2
mol NO
=
5.00
mol NO
2
Calculate the number of grams of the product NO2 that form. Be sure your answer has the correct number of significant figures.
g NO2
To calculate the number of grams of NO2 that form, we need to use the molar mass of NO2, which is 46.0055 g/mol.
5.00 mol NO2 x 46.0055 g/mol = 230.03 g NO2
Therefore, 230.03 grams of NO2 will form.