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3 years ago

5. The number of moles of molecules in a 12.0-gram sample of Cl2 is

Chemistry

2 answers:

torisob [31]3 years ago

4 0

Answer:

$\frac{12}{71}$ mole

Explanation:

Given parameters:

Mass = 12g

Molecule = Cl₂

Unknown:

Number of moles of molecules = ?

Solution:

To solve this problem, we use the expression below:

Number of moles = $\frac{mass}{molar mass}$

molar mass of Cl₂ = 2 (35.5) = 71g/mol

Number of moles = $\frac{12}{71}$ mole

Natasha_Volkova [10]3 years ago

4 0

Answer:just tryna get the answer lol

Explanation:

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The answer to this question would be: electron

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4 years ago

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Describe how elements of different electronegativities can share electrons unequally, leading to the formation of a polar covale

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2 years ago

In the following reaction, identify the oxidized species, reduced species, oxidizing agent, and reducing agent. Be sure to answe

gtnhenbr [62]

Answer :

$Cl_2$ is reduced species.

$KI$ is oxidized species.

$Cl_2$ is oxidizing agent.

$KI$ is reducing agent.

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

Reducing agent : It is defined as the agent which helps the other substance to reduce and itself gets oxidized. Thus, it will undergo oxidation reaction.

Oxidizing agent : It is defined as the agent which helps the other substance to oxidize and itself gets reduced. Thus, it will undergo reduction reaction.

The balanced redox reaction is :

$Cl_2(aq)+2KI(aq)\rightarrow 2KCl(aq)+I_2(aq)$

The half oxidation-reduction reactions are:

Oxidation reaction : $2I^-\rightarrow I_2+2e^-$

Reduction reaction : $Cl_2^++2e^-\rightarrow 2Cl^-$

From this we conclude that the $'KI'$ is the reducing agent that loses an electron to another chemical species in a redox chemical reaction and itself gets oxidized and $'Cl_2'$ is the oxidizing agent that gain an electron to another chemical species in a redox chemical reaction and itself gets reduced.