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2 years ago

Compared with the energy it takes to separate oxygen and hydrogen from water. How much energy is released when they recombine?.

Chemistry

1 answer:

Stolb23 [73]2 years ago

4 0

The same amount of energy is released when they recombine.

<h3>How to separate oxygen and hydrogen from water?</h3>

Electrolysis is a promising choice for without carbon hydrogen creation from inexhaustible and atomic assets.
Electrolysis is the method involved with utilizing power to part water into hydrogen and oxygen.
This response happens in a unit called an electrolyzer.
Electrolyzers can go in size from little, apparatus size hardware that is appropriate for limited scope dispersed hydrogen creation to huge scope, focal creation offices that could be tied straightforwardly to sustainable or other non-ozone depleting substance radiating types of power creation.

Like energy components, electrolyzers comprise of an anode and a cathode isolated by an electrolyte. Different electrolyzers capability in various ways, fundamentally because of the different kind of electrolyte material included and the ionic species it conducts.

To learn more about electrolysis from the given link

brainly.com/question/24063038

#SPJ4

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Predict the Solubility of the following substances in water.

anyanavicka [17]

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b. AgBr: insoluble
c. NH4OH: soluble
d. Ag2CO3: insoluble
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5 0

3 years ago

I’m not sure how to do this, please help. It’s a mole to mole stoich worksheet.

wlad13 [49]

Answer: 4.05 mol O2, 15.36 mol H2O

Explanation:

I can answer each question individually if you post them individually.

2a. 3.24 mol NH3 * (5 mol O2 / 4 mol NH3) = 4.05 mol O2

2b. 12.8 mol O2 ( 6mol H2O/ 5 mol O2) = 15.36 mol H2O

Essentially what I did was dimensional analysis. Multiplying in a way that the units cancel out so the only thing remains is what each question asks for.

3 0

3 years ago

Which has higher specific heat capacity, iron or brick (Concrete

Dominik [7]

Answer:

Brick

Explanation:

8 0

3 years ago

Read 2 more answers

Balance the following redox reaction in basic solution. Cl â’ (aq) + MnO â’ 4 (aq) â†’ Cl 2 (g) + MnO 2 (s)

FinnZ [79.3K]

$6\; \text{Cl}^{-} \; (aq) + 2\; \text{MnO}_4^{-} \; (aq) + 4 \; \text{H}_2 \text{O} \; (l) \to 3\; \text{Cl}_2 \; (g) + 2\; \text{MnO}_2 \; (s) + 8\; \text{OH}^{-} \; (aq)$

<h3>Explanation</h3>

The oxidation state of the manganese atom $\text{Mn}$ changes from +7 as in $\text{MnO}_4^{-}$ to +4 as in $\text{MnO}_2$ .
There are one $\text{Mn}$ atom in each $\text{MnO}_4$ ion.
Reducing each $\text{MnO}_4^{-}$ ion would thus consume three electrons.

Similarly, the oxidation state of the chlorine atom $\text{Cl}$ changes from -1 as in $\text{Cl}^{-}$ to 0 as in $\text{Cl}_2$ .
It takes two $\text{Cl}^{-}$ ions to produce one $\text{Cl}_2$ molecule.
Oxidizing every two $\text{Cl}^{-}$ would thus produce one $\text{Cl}_2$ while releasing two electrons.

Three $\text{Cl}_2$ molecules contain six chlorine atoms. Three $\text{Cl}_2$ would thus correspond to six $\text{Cl}^{-}$ ions.

Combining six $\text{Cl}^{-}$ , two $\text{MnO}_4^{-}$ ions, three $\text{Cl}_2$ ions, and two $\text{MnO}_2$ would balance the changes in oxidation state.

$6\; \text{Cl}^{-} \; (aq) + 2\; \text{MnO}_4^{-} \; (aq) \to 3\; \text{Cl}_2 \; (g) + 2\; \text{MnO}_2 \; (s)$ (NOT BALANCED)

Still, the product side lacks four oxygen atoms.

In an acidic environment, oxygen atoms would combine with protons to produce water.
In a basic environment (like this one,) there are nearly no protons for oxygen atoms to combine with. Oxygen atoms will likely combine with water to produce hydroxide ions.

Each oxygen atom combine with a water molecule to produce two hydroxide ions. Adding four water molecules and eight hydroxide ions would balance the equation.

5 0

3 years ago

Which unit can be used to express solution concentration

anygoal [31]

mol/dm³, mol/m³, etc

4 0

3 years ago