Question

2 NO(g) + O2 (g) --> 2 NO2 (g)

What mass of NO2 is produced by the reaction of 2.40 mol NO with excess oxygen?

Answer 1

To find the mass of NO2 produced, we can use stoichiometry and the molar mass of NO2. In this reaction, 2.40 mol of NO will produce 2.40 mol of NO2, and the mass of NO2 produced is 110.42 g.

Step-by-step explanation:

The balanced equation for the reaction is 2 NO(g) + O2(g) → 2 NO2(g). To find the mass of NO2 produced, we first need to convert the number of moles of NO to moles of NO2 using stoichiometry. Since 2 NO is required to produce 2 NO2, the number of moles of NO2 produced will be the same as the number of moles of NO. Therefore, 2.40 mol of NO will produce 2.40 mol of NO2. To find the mass of NO2 produced, we can use the molar mass of NO2:

Molar mass of NO2 = 46.01 g/mol.

Mass of NO2 = Moles of NO2 × Molar mass of NO2

Mass of NO2 = 2.40 mol × 46.01 g/mol = 110.42 g.

Answer 2

2 NO(g) + O2(g) = 2 NO2(g)

2 moles NO ------------ 2 moles NO2
2.40 moles NO ---------- ? ( moles NO2)

moles NO2 = 2.40 x 2 / 2

moles NO2 = 4.8 / 2

= 2.4 moles of NO2

molar mass NO2 = 46.0 g/mol

1 mole ----------- 46.0 g
2.4 moles ------- ( mass NO2)

mass NO2 = 2.4 x 46.0 / 1

mass NO2 = 110.4 / 1

= 110.4 g of NO2