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Vlad1618 [11]
3 years ago
15

Which of the following happens during an endothermic chemical change? Heat is released. Net energy decreases. Products have a hi

gher total potential energy than the reactants. Products have the same total potential energy as the reactants.
Chemistry
1 answer:
frutty [35]3 years ago
7 0

Answer:

Products have a higher total potential energy than the reactants

Explanation:

<em>-absorbs heat not released </em>

<em>-there is no net energy change</em>

<em>-In an endothermic reaction, the reaction mixture absorbs heat from the surroundings. Therefore, the products will have a higher energy than the reactants</em>

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<h3>1</h3>

Species shown in bold are precipitates.

  • Ca(NO₃)₂ + 2 KOH → Ca(OH)₂ + 2 KNO₃
  • Ca(NO₃)₂ + Na₂C₂O₄ → CaC₂O₄ + 2 NaNO₃
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  • Ni(NO₃)₂ + 2 KOH → Ni(OH)₂ + 2 KNO₃
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  • Zn(NO₃)₂ + 2 KOH → Zn(OH)₂ + 2 KNO₃
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<h3>2</h3>

A double replacement reaction takes place only if it reduces in the concentration of ions in the solution. For example, the reaction between Ca(NO₃)₂ and KOH produces Ca(OH)₂. Ca(OH)₂ barely dissolves. The reaction has removed Ca²⁺ and OH⁻ ions from the solution.

Some of the reactions lead to neither precipitates nor gases. They will not take place since they are not energetically favored.


<h3>3</h3>

Compare the first and last row:

Both Ca(NO₃)₂ and Zn(NO₃)₂ react with KOH. However, between the two precipitates formed, Ca(OH)₂ is more soluble than Zn(OH)₂.

As a result, add the same amount of KOH to two Ca(NO₃)₂ and Zn(NO₃)₂ of equal concentration. The solution that end up with more precipitate shall belong to Zn(NO₃)₂.


<h3>4</h3>

Compare the second and third row:

Cu(NO₃)₂ reacts with KI, but Ni(NO₃)₂ does not. Thus, add equal amount of KI to the two unknowns. The solution that forms precipitate shall belong to Cu(NO₃)₂.

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