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4 years ago

Balancing Chemical Equations

1 answer:

5 0

Number 1: answer is Zn + 2HCl ----> ZnCl2 + H2
This one was a bit simple
we have:
zn- 1 zn-1
H-1 H-2
Cl-1 Cl-2
After this you can see that both H and Cl need to be multiplied by 2 on the reactants side. By putting 2HCl, you have accomplished this goal
Number 2: 4Fe + 3O2 ----> 2Fe2O3
We have:
Fe- 1 Fe-2
O-2 O-3
So unlucky for us, none of these were already balanced. I started first with Fe and started plugging in numbers. So if i were to put a 2 in front of Fe, it would cause 2-Fe and then 2-Fe on the other side, making it balanced.
The problem is that the O values still need to be balanced. If you notice, both Os have a 3 or a 2. 3 x 2= 6. SO you would need to add the opposite number on each. (3O2).
Number 3: 2H2O2 -----> 2H2O + O2
The answer is balanced as it has
H- 4 H-4
O-4 O-4
To figure this out, you would have to first look at what you need
The H values already look balanced, so we will look at O
There are 2 on the reactant side and 3 on the product
Start by adding a 2 onto H2O2 (2H2O2)
We now have 4 H and 4 O values on that side, but we still need to change the products side
By adding a 2 to H2O, You would then have the number of required values.

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3 years ago

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring

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Answer:

The standard cell potential is 1.40 V. The correct option is the option D (+1.40 V)

Explanation:

Oxide-reduction reactions, also called redox, involve the transfer or transfer of electrons between two or more chemical species. In these reactions two substances interact: the reducing agent and the oxidizing agent.

An oxidizing element or oxidizing agent is one that reaches a stable energy state as a result of which the oxidant is reduced and gains electrons. The oxidizing agent causes oxidation of the reducing agent generating the loss of electrons of the substance and, therefore, oxidizes in the process.

In other words, the oxidizing agent is that chemical species that in a redox process accepts electrons released by the reducing agent and, therefore, is reduced in said process. The oxidizing agent is reduced because, upon receiving electrons from the reducing agent, a decrease in the value of the charge or oxidation number of one of the atoms of the oxidizing agent is induced .

Electrochemical cells, galvanic cells or batteries are called devices that are capable of transforming chemical energy originated in a spontaneous redox process into electrical energy.

The cellular potential is generally in standard conditions, that is, 1 M with respect to solute concentrations in solution and 1 atm for gases.

In this case you have the reaction:

3 Cl₂(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe³⁺(aq)

In this case the following half-reactions occur:

Semi-reaction of oxidation ( an atom or group of atoms loses electrons, or increases its positive charges): Fe³⁺(aq) + 3 e- -->Fe(s); E⁰ = -0.04 V

Semi-reaction of reduction (an atom or group of atoms gains electrons, increasing its negative charges): Cl₂(g) + 2 e- --> 2 Cl-(aq); E⁰=1.36 V

In an electrochemical cell at 25°C the potentials of the semi-reactions are usually measured in the sense of reduction and generally the standard potential between both electrochemical cells will be:

$E^{0} =E^{0} _{reduction} -E^{0} _{oxidation}$

E⁰=1.36 V - (-0.04 V)

E⁰=1.36 V + 0.04 V

<em>E⁰=1.40 V</em>

<em><u>The standard cell potential is 1.40 V. The correct option is the option D (+1.40 V)</u></em>

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3 years ago

Help me please!! I need help with both finding the mistake and the answer and I'll give the brainliest :)

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Answer:

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16Fe(s) + 3S₈(s) => 8Fe₂S₃(s)

Excess | 1.25 mole | ? grams

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Answer:

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