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3 years ago

Which is an example of an exothermic process?

Chemistry

2 answers:

Diano4ka-milaya [45]3 years ago

7 0

<h3>Question 1</h3>

An example of an exothermic process is, A hot pack feels warm when chemicals in it combine.

<h2>Further Explanation;</h2><h3>Energy changes in chemical reactions</h3>

Chemical reactions are accompanied by energy changes, as energy is either absorbed to break chemical bonds or released when bonds are formed.
Chemical reactions are therefore classified as endothermic reactions or exothermic reactions.

<h3>Exothermic reactions </h3>

Exothermic reactions are types of reaction that release energy to the surrounding.
In these reactions energy is released when new bonds are formed during the reactions. More energy is released when bonds are formed in the products than is used to break bonds in the reactants.
Therefore exothermic reactions have a negative (-) enthalpy change (ΔH).

<h3>Endothermic reactions </h3>

Endothermic reactions are type of reactions that absorb energy from the surroundings.
In these type of reactions more energy is absorbed when bonds of the reactants are broken than the energy released when bonds of the products are formed.
Endothermic reactions have a positive (+) enthalpy change (ΔH).

Keywords: Chemical reactions, energy changes in chemical reactions, exothermic reactions, endothermic reactions.

<h2>Question 2</h2>

The statement that describes the reaction;

N2(g) + 3H2(g)---> 2NH3(g) + 93 kJ is

The reaction is an endothermic reaction because energy is absorbed

<h2>Further Explanation;</h2><h3>Enthalpy of a reaction (ΔH)</h3>

Enthalpy chnage of a reaction or heat change is the difference between the enthalpy of products and the enthalpy of reactants.
Enthalpy change can be used to determine whether a reaction is exothermic or endothermic.
ΔH = energy used in bond breaking of reactant + energy released in bond formation of product.

<h3>Endothermic reactions</h3>

Endothermic reactions have a positive (+) enthalpy change (ΔH) because less energy is released when the products are formed compared to the energy used to break up the bonds in reactants.

<h3>Exothermic reactions </h3>

Exothermic reactions have a negative(-) enthalpy change (ΔH) since more energy released when the products are formed compared to energy used to break bonds in reactants.

Keywords: Enthalpy change, heat change, exothermic reactions, endothermic reactions.

<h3>Learn more about</h3>

Energy changes in chemical reactions: brainly.com/question/2217125
Ethalpy change; brainly.com/question/1127247
Endothermic reactions: brainly.com/question/1127247
Exothermic reactions: brainly.com/question/1831889

Level: High school

Subject: Chemistry

Topic: Chemical reactions

Sub-topic: Energy changes in chemical reactions

Gwar [14]3 years ago

5 0

1) Answer: A hot pack feels warm when chemicals in it combine.

Explanation: Reactions or process in which heat is released(produced) are known as exothermic reactions or process and those in which the heat is absorbed are known as endothermic reactions or process.

If a beaker feels cools when chemical in it react then it means the chemicals have absorbed the heat energy from its surroundings and so it is an example of an endothermic process.

A hot pack feels warm when chemicals in it combine means the energy is released in the chemical reaction and so it is an example of an exothermic process.

Plants use the sun's energy for photosynthesis which is a process of forming food for the plants. Energy acts as a reactant in this process and so it is an example of endothermic process.

Frying an egg by heating it on a stove is an example of an endothermic process as the heat is required to fry the egg.

So, the only exothermic process is the second one, "A hot pack feels warm when chemicals in it combine."

2) In the given equation, heat is written as a product means the heat is released in the equation and so it is an example of an exothermic reaction.

So, the correct choice is the last one " It is exothermic because energy is released."

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3 years ago

Read 2 more answers

If a lab group were using hydrochloric acid to perform a substitution reaction, which precaution would not be a concern?

Pie

The question is incomplete. Complete question is attached below:
...............................................................................................................................

Correct Answer: Option A i.e Flammability

Reason:

Hydrochloric acid is a strong acid. It has a high value of dissociation constant. Following equilibrium is established with HCl is dissolved in water

HCl + H2O ↔ Cl- + H3O+

Above, reaction is highly exothermic in nature. So care must be taken while preparing HCl solution of desired concentration. HCl must be added in beaker containing water. Reversed, i.e. adding water in HCl, must never be done. This is because when acid is poured into water, it flows down the flask and mixes much efficiently and no boiling occurs. On other hand, <span> when water is added to acid, the very first drop of water will react with acid. The heat generated during this event might be high enough to boil the water instantly, which could spray acid out of the container.

The physical contact with concentration HCl will result in skin burn. As well, inhaling</span><span> HCl vapors can cause burns to body tissues, lung damage and even death in extreme cases. Also, since HCl is a strong acid, it would undergoes reaction almost spontaneously, which would inturn favour substitution reaction. However, HCl is not a flammable gas. Hence, it is of no concern while performing substitution reaction. </span>