Answer:
56.5J
Explanation:
<em>To </em><em>find</em><em> </em><em>the </em><em>heat </em><em>energy</em><em> </em><em>required</em><em> </em><em>use </em><em>the </em><em>formula</em><em> </em><em>for </em><em>the </em><em>specific</em><em> </em><em>heat </em><em>capacity</em><em> </em><em>which </em><em>is </em>
<em>c=</em><em>quantity</em><em> of</em><em> </em><em>heat/</em><em>mass×</em><em>c</em><em>h</em><em>a</em><em>n</em><em>g</em><em>e</em><em> </em><em>in </em><em>temperature</em>
<em>in </em><em>this </em><em>question</em><em> </em><em>c </em><em>is </em><em>0</em><em>.</em><em>2</em><em>2</em><em>6</em><em>j</em><em>/</em><em>g,</em><em>the </em><em>mass </em><em>is </em><em>5</em><em>0</em><em>g</em><em> </em><em>and </em><em>the </em><em>change </em><em>in </em><em>temperature</em><em> </em><em>is </em><em>3</em><em>0</em><em>-</em><em>2</em><em>5</em><em>=</em><em>5</em>
<em>therefore</em>
<em>0</em><em>.</em><em>2</em><em>2</em><em>6</em><em>=</em><em>Q/</em><em>5</em><em>0</em><em>×</em><em>5</em>
<em>Q=</em><em>0</em><em>.</em><em>2</em><em>2</em><em>6</em><em>×</em><em>2</em><em>5</em><em>0</em>
<em> </em><em> </em><em> </em><em>=</em><em>56.5J</em>
<em>I </em><em>hope </em><em>this</em><em> helps</em>
A reduced element (which gains electrons) and an oxidized element are required for redox reactions (gives electrons). It is not a redox reaction if we lack both of them (an element can not receive electrons if no element gives electrons and vice versa).
A reduced half and an oxidized half, which always occur together, make up redox processes. While the oxidized half experiences electron loss and an increase in oxidation number, the reduced half obtains electrons and the oxidation number declines. The mnemonic devices OIL RIG, which stand for "oxidation is loss" and "reduction is gain," are simple ways to memorize this. In a redox process, the total number of electrons stays constant. In the reduction half reaction, another species absorbs those that were released in the oxidation half reaction.
In a redox reaction, two species exchange electrons, and they are given unique names:
- The ion or molecule that accepts electrons is called the oxidizing agent - by accepting electrons it oxidizes other species.
- The ion or molecule that donates electrons is called the reducing agent - by giving electrons it reduces the other species.
Hence, what is oxidized is the reducing agent and what is reduced is the oxidizing agent.
<h3>
What is the purpose of oxidizing agents and reducing agents?</h3>
By reducing other compounds and shedding electrons, a reducing agent raises its oxidation state. An oxidizing agent gets electrons by oxidizing other compounds; as a result, its oxidation state lowers.
<h3>
What is a redox reaction?</h3>
Oxidation-reduction (or "redox") reactions are chemical processes in which electrons are exchanged between two substances. An oxidation-reduction reaction is any chemical process in which a molecule, atom, or ion alters the number of electrons it has, hence increasing or decreasing its oxidation state.
Learn more about redox reaction: brainly.com/question/13293425
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Answer:
Explanation: Zn (s) + 2 AgCl (s) ⇒ ZnCl2 (s) + 2 Ag(s)
Less noble Zinc reduces more noble Silver
Answer and Explanation:
Find enclosed the Lewis diagrams for ozone (O₃) resonance structures. The diagram shows the two main contributing structures (I and II) with their formal charges.
The formal charge (FC) is determined as follows:
FC= number of valence electrons in free atom - 1/2 (number of bonding electrons) - number of non bonding electrons
The O central atom has the formal charge +1:
FC= 6 - 1/2(6) - 2= +1
The O atom on the right in structure I and on the left in structure II has the formal charge -1:
FC= 6 - 1/2(2) - 6= 6 - 1 - 6 = -1
The O atom on the left in structure I and on the right in structure II has the formal charge 0:
FC= 6- 1/2(4) - 4= 6 - 2 - 4= 0
