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Novosadov [1.4K]
2 years ago
7

SHOW ALL WORK AND INCLUDE UNITS

Chemistry
1 answer:
Sliva [168]2 years ago
6 0

Answer:

+375.2 KJ.

Explanation:

The balanced equation for the reaction is given below:

H₂ + F₂ —> 2HF ΔH = +536 KJ

From the balanced equation above,

2 moles of HF required +536 KJ .

Finally, we shall determine the heat required to produce 1.4 mol of hydrogen fluoride, HF. This is illustrated below:

From the balanced equation above,

2 moles of HF required +536 KJ .

Therefore, 1.4 moles of HF will require = (1.4 × 536)/2 = +375.2 KJ

Thus, +375.2 KJ of heat energy is required.

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asambeis [7]
<h3>Answer:</h3>

5.00 mol O₂

<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
  • Left to Right<u> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

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<u>Stoichiometry</u>

  • Using Dimensional Analysis
<h3>Explanation:</h3>

<u>Step 1: Define</u>

3.01 × 10²⁴ atoms O₂

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

Avogadro's Number

<u>Step 3: Convert</u>

  1. Set up:                              \displaystyle 3.01 \cdot 10^{24} \ atoms \ O_2(\frac{1 \ mol \ O_2}{6.022 \cdot 10^{23} \ atoms \ O_2})
  2. Multiply/Divide:                \displaystyle 4.99834 \ mol \ O_2

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 3 sig figs.</em>

4.99834 mol O₂ ≈ 5.00 mol O₂

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Answer: -

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Explanation: -

A reaction involves change of the reactants into products.

Initially there is only reactants. So the rate if reaction is high.

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Reactions involve collisions of reactant molecules. As the reactant amount decreases, collisions between the reactants decreases. As such the rate of reaction decreases with the progress of the reaction.

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