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Hatshy [7]
3 years ago
5

If your boss says you must produce 400 g of ammonia (NH3) in order to keep your job, what mass of nitrogen should you use in thi

s reaction? N2(g) + 3 H2(g) -> 2 NH3(g).
Chemistry
1 answer:
nevsk [136]3 years ago
8 0

Answer:

331 g

Explanation:

Step 1: Write the balanced equation

N₂(g) + 3 H₂(g) → 2 NH₃(g)

Step 2: Calculate the moles corresponding to 400 g of ammonia

The molar mass of ammonia is 17.03 g/mol.

400g \times \frac{1mol}{17.03g} =23.5mol

Step 3: Calculate the moles required of nitrogen

The molar ratio of N₂ to NH₃ is 1:2.

23.5molNH_3 \times \frac{1molN_2}{2molNH_3} =11.8molN_2

Step 4: Calculate the mass corresponding to 11.8 moles of nitrogen

The molar mass of nitrogen is 28.01 g/mol.

11.8 mol \times \frac{28.01g}{mol} =331 g

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<h3>Answer:</h3>

28 mol CaF

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
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<u>Stoichiometry</u>

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<u>Step 1: Define</u>

[Given] 1.7 × 10²⁵ molecules CaF

[Solve] moles CaF

<u>Step 2: Identify Conversions</u>

Avogadro's Number

<u>Step 3: Convert</u>

  1. [DA] Set up:                                                                                                          \displaystyle 1.7 \cdot 10^{25} \ molecules \ CaF(\frac{1 \ mol \ CaF}{6.022 \cdot 10^{23} \ molecules \ CaF})
  2. [DA] Multiply/Divide [Cancel out units]:                                                         \displaystyle 28.2298 \ moles \ CaF

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 2 sig figs.</em>

28.2298 mol CaF ≈ 28 mol CaF

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