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3 years ago

Write a balanced chemical reaction for the dissolution of your copper oxide sample in hydrochloric acid

1 answer:

5 0

Copper oxide reacts with hydrochloric acid to produce copper chloride and water.

So the basic equation that illustrates this reaction is:
CuO + HCl ......> CuCl2 + H2O

Now, we need to balance this equation:
the number of copper and oxygen moles are balanced.
For each of hydrogen and chlorine, we have one mole as a reactant and two moles as product.
Therefore, to balance this, we will add an extra mole of HCl in the reactants.

Based on this, the final balanced equation would be:
CuO + 2HCl ................> CuCl2 + H2O

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jolli1 [7]

Answer:

0.83 g

Explanation:

Step 1: Write the balanced equation

Fe + CuSO₄ ⇒ Cu + FeSO₄

Step 2: Calculate the moles corresponding to 0.75 g of Fe

The molar mass of Fe is 55.85 g/mol.

$0.75g \times \frac{1mol}{55.85g} = 0.013 mol$

Step 3: Calculate the moles of Cu produced from 0.013 moles of Fe

The molar ratio of Fe to Cu is 1:1. The moles of Cu produced are 1/1 × 0.013 mol = 0.013 mol.

Step 4: Calculate the mass corresponding to 0.013 moles of Cu

The molar mass of Cu is 63.55 g/mol.

$0.013mol \times \frac{63.55g}{mol} = 0.83 g$

4 0

4 years ago

Read 2 more answers

Please help me I will give you the brain thing and extra points. 2

oee [108]

I think it’s A but, don’t come at me if I’m wrong. Btw I read over it multiple times so this isn’t a random guess. Good luck tell me if you got it right

7 0

3 years ago

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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

Please can someone help me??!

svp [43]

I believe the correct order of words should be:

Counterclockwise

Crescent

Full

Half

Faces?

Waxing

Right

Waning

Left

I am not sure on faces, but I don't see any other words from the bank that would fit that description. Hope these are correct and hope I helped!

4 0

3 years ago

In order to become stable in an ionic bond, oxygen needs to (A) gain 2 electrons (C) share 2 electrons B) lose 2 electrons

Sedbober [7]

Answer:

gains 2 electrons. In order for the new ionic compound to form a a neutral compound, the oxygens must gain 6 electrons

3 0

3 years ago

Read 2 more answers