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Sagot :
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
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