Given that 4NH₃(g) + 50₂(g) - 4NO(g) + 6H₂0(g), if 4.5 moles of NH₃ react with sufficient oxygen, how many moles of H₂O should form?
O 4.0
O 4.5
O 6.0
O 6.8
O 5.5



Answer :

Answer:

6.8 mol

Explanation:

Pre-Solving

We are given the following chemical reaction:

4NH₃(g) + 5O₂(g) -> 4NO(g) + 6H₂O(g)

We want to know how much water (H₂O) would form if 4.5 moles of NH₃ reacts with enough oxygen to completely react all 4.5 moles.

Solving

This can be solved with stoichiometry. We want to convert from NH₃ to H₂O.

[tex]4.5 mol NH_3 * \frac{6 mol H_2O}{4 mol NH3} = 6.8 mol H_2O[/tex] (rounded to two sig figs)

When 4.5 moles of NH₃ react, they produce approximately d. 6.8 moles of H₂O.

To determine how many moles of H₂O are produced when 4.5 moles of NH₃ react, we need to look at the balanced chemical equation:

4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g)

The equation shows that 4 moles of NH₃ produce 6 moles of H₂O.

If 4 moles of NH₃ produce 6 moles of H₂O, then 1 mole of NH₃ would produce (6/4) or 1.5 moles of H₂O.

So, for 4.5 moles of NH₃:

4.5 moles NH₃ × (1.5 moles H₂O / 1 mole NH₃) = 6.75 moles of H₂O

Hence, 4.5 moles of NH₃ will produce approximately 6.75 moles of H₂O. None of the answer options exactly fit this, but 6.8 is the closest. The correct answer is d. 6.8,

The complete question is:

Given that 4NH₃(g) + 50₂(g) - 4NO(g) + 6H₂0(g), if 4.5 moles of NH₃ react with sufficient oxygen, how many moles of H₂O should form?

a. 4.0

b. 4.5

c. 6.0

d. 6.8

e. 5.5