Question

For each pair below, select the sample that contains the largest number of moles. Pair A 2.50 g O2 2.50 g N2

Answer 1

Answer:

Pair A : 2.50 g N2    Pair B : 21.5 g n2    Pair C : 0.081 CO2

Explanation:

Answer 2

Answer:

Explanation:

Pair  2.50g of O₂ and 2.50g of  N₂

The atoms sample with the largest number of moles since the masses are the same would be the one with lowest molar mass according the the equation below:

Number of moles = $\frac{mass }{molarmass}$

Atomic mass of O = 16g and N = 14g

Molar mass of O₂ = 16 x 2 = 32gmol⁻¹

Molar mass of N₂ = 14 x 2 = 28gmol⁻¹

Number of moles of O₂ = $\frac{2.5}{32}$ = 0.078mole

Number of moles of N₂ = $\frac{2.5}{28}$ =  0.089mole

We see that N₂ has the largest number of moles