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neonofarm [45]
3 years ago
6

What is the energy change associated with 1.5 mole of D being formed? 

Chemistry
1 answer:
AleksandrR [38]3 years ago
3 0

Answer:

–36 KJ.

Explanation:

The equation for the reaction is given below:

2B + C —› D + E. ΔH = – 24 KJ

From the equation above,

1 mole of D required – 24 KJ of energy.

Now, we shall determine the energy change associated with 1.5 moles of D.

This can be obtained as illustrated below:

From the equation above,

1 mole of D required – 24 KJ of energy

Therefore,

1.5 moles of D will require = 1.5 × – 24 = –36 KJ.

Therefore, –36 KJ of energy is associated with 1.5 moles of D.

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Answer:

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General Formulas and Concepts:

<u>Chemistry - Atomic Structure</u>

  • Reading a Periodic Table
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Explanation:

<u>Step 1: Define</u>

24.75 g H₂O

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

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<u>Step 3: Convert</u>

<u />24.75 \ g \ H_2O(\frac{1 \ mol \ H_2O}{18.02 \ g \ H_2O} ) = 1.37347 mol H₂O

<u>Step 4: Check</u>

<em>We are given 4 sig figs. Follow sig fig rules and round.</em>

1.37347 mol H₂O ≈ 1.373 mol H₂O

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