Question

When 7.00 g of hydrogen react with 70.0 g of nitrogen, hydrogen is considered the limiting reactant because

Answer 1

Answer: A

Explanation: i just took the test and quick answer

Answer 2

Answer:

7.5 mol of hydrogen would be needed to consume the available nitrogen.

Explanation:

• The balanced equation of the reaction of hydrogen with nitrogen is:

3H₂ + N₂ → 2NH₃

it is clear that 3mol of hydrogen react with 1 mol of Nitrogen to give 2 mol of ammonia.

• firstly, we need to calculate the number of moles of both

for H₂:

number of moles = mass / molar mass = (7.00 g) /  (2.00 g/mol) = 3.5 mol.

for N₂:

number of moles = mass / molar mass = (70.00 g) /  (28.00 g/mol) = 2.5 mol.

using cross multiplication

1 mol of  N₂ needs → 3 mol of H₂

2.5 mol of  N₂ needs → ??? mol of H₂

∴ the number of mol of H₂ needed = (3*2.5) / 1 = 7.5 mol

So, the right choice is:

7.5 mol of hydrogen would be needed to consume the available nitrogen.