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AlekseyPX
3 years ago
13

This chemical equation is balanced.

Chemistry
1 answer:
alina1380 [7]3 years ago
6 0

Answer:

A

Explanation:

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The decomposition of water into hydrogen gas H2 and oxygen gas 02 can be modeled by the balanced chemical equation
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Answer:

2H20 ------> 2H2 + O2

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4 years ago
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Jet001 [13]

Answer:

1 mol SO2 contains 6.0213*10^23 molecules

6.023*10^24 molecules = 10 mol SO2

Equation

S(s) + O2(g) → SO2(g)

1 mol S reacts with 1 mol O2 to prepare 1 mol SO2

To prepare 10 mol SO2 you require : 10 mol S plus 10 mol O2

And that is the answer to the question

If you want a mass :

Molar mass S = 32 g/mol You require 10 mol = 320 g

Molar mass O2 = 32 g/mol :You require 10 mol = 320 g

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Spectator ions when FeSO4 and PbNO32 react
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Explanation:

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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.

Thus, Cl_2 is reduced species.

KI is oxidized species.

Cl_2 is oxidizing agent.

KI is reducing agent.

7 0
4 years ago
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