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Dahasolnce [82]
3 years ago
14

Hydrazine reacts with oxygen according to the following equation: N2H4(g) +O2(g) → N2(g) + 2 H2O(l) How many L of N2, measured a

t 34.9 °C and 755.08 torr, will be produced at the same time that 914.894 g of H2O is produced?
Chemistry
1 answer:
mihalych1998 [28]3 years ago
6 0

Answer:

V ≈ 646.50 L

General Formulas and Concepts:

<u>Chemistry - Gas Laws</u>

  • Reading a Periodic Table
  • Stoichiometry
  • Combined Gas Law: PV = nRT
  • R constant - 62.4 (L · torr)/(mol · K)
  • Kelvin Conversion: K = °C + 273.15

Explanation:

<u>Step 1: Define</u>

RxN:   N₂H₄ (g) + O₂ (g) → N₂ (g) + 2H₂O (l)

Given:   34.9 °C, 755.08 torr, 914.894 g H₂O

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

Kelvin Conversion

Molar Mass of H - 1.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol

<u>Step 3: Convert</u>

Stoichiometry:   914.894 \ g \ H_2O(\frac{1 \ mol \ H_2O}{18.02 \ g \ H_2O} )(\frac{1 \ mol \ N_2}{2 \ mol \ H_2O} ) = 25.3955 mol N₂

Temperature:    34.9 + 273.15 = 308.05 K

<u>Step 4: Find Volume</u>

  1. Substitute variables:                                                                             (755.08 torr)V = (25.3955 mol)(62.4 (L · torr)/(mol · K))(308.05 K)
  2. Multiply:                                                                                                      (755.08 torr)V = 488160 L · torr
  3. Isolate <em>V</em>:                                                                                                          V = 646.502 L

<u>Step 5: Check</u>

<em>We are given 5 sig figs as our lowest. Follow sig fig rules and round.</em>

646.502 L ≈ 646.50 L

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