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2 years ago

What chemical change occurred in the following reaction? Mg2+(aq)+2OH−(aq)⟶ Mg(OH)2(s)

Chemistry

2 answers:

irina1246 [14]2 years ago

6 0

I think it might be a gas was formed.
Hope I'm right and it helps you out!!

7nadin3 [17]2 years ago

3 0

Answer : When magnesium salts combine with the alkaline water it induces precipitation of solid $Mg(OH)_2$ .

Explanation :

Chemical change : The chemical change occurs when a substance combine with the another substance to form a new substance.

It can not be easily reversible.

The new product is formed or precipitate may be formed.

Physical change : The physical change occurs when a substance combine with the another substance then no new compound is formed.

It can be reversible.

No new product is formed only changes occurs in the state or phase.

As per question, when magnesium salts combine with the alkaline water it induces precipitation of solid $Mg(OH)_2$ .

The balanced chemical reaction is,

$Mg^{2+}(aq)+2OH^-(aq)\rightarrow Mg(OH)_2(s)$

That mean a new compound is formed by this reaction. So, the chemical change occurred in this reaction.

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70 POINTS What type of organic compound contains the following functional group?

andrew-mc [135]

The compound contains an ester functional group.

An ester is a carbonyl (C=O) group with an alkyl (R) group on one side and an alkoxy (OR) group on the other.

We write the condensed structural formula of an ester as R(C=O)OR or RCOOR.

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3 years ago

The heat of fusion for water is the amount of energy that must be absorbed for water to _____.

ivanzaharov [21]

I would say A.evaporate because the water is getting absorbed.

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3 years ago

Select all the species that are ions. HCl NaCl NH4+ H2PO4- CCl4 H3O+

nata0808 [166]

Answer:

NH₄⁺

H₂PO₄⁻

H₃O⁺

Explanation:

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Ion may be positively charged "cation" or negatively charged "anion".

Neutral molecule has a net charge of zero.

So, the species that are ions are:

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4 0

3 years ago

Use the following half-reactions to construct a voltaic cell:

velikii [3]

Answer: The correct answer is $3Ag^+(aq.)+Cr(s)\rightarrow 3Ag(s)+Cr^{3+}(aq.);E^o_{cell}=+1.53V$

Explanation:

We are given:

$Cr^{3+}(aq.)+3e^-\rightarrow Cr(s);E^o=-0.73V\\\\Ag^+(aq.)+e^-\rightarrow Ag(s);E^o=+0.80V$

The substance having highest positive $E^o$ potential will always get reduced and will undergo reduction reaction. Here, silver will always undergo reduction reaction will get reduced.

Chromium will undergo oxidation reaction and will get oxidized.

The half reactions for the above cell is:

Oxidation half reaction: $Cr(s)\rightarrow Cr^{3+}+3e^-;E^o_{Cr^{3+}/Cr}=-0.73V$

Reduction half reaction: $Ag^{+}+e^-\rightarrow Ag(s);E^o_{Ag^{+}/Ag}=0.80V$ ( × 3)

Net equation: $3Ag^+(aq.)+Cr(s)\rightarrow 3Ag(s)+Cr^{3+}(aq.)$

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

Putting values in above equation, we get:

$E^o_{cell}=0.80-(-0.73)=1.53V$

Hence, the correct answer is $3Ag^+(aq.)+Cr(s)\rightarrow 3Ag(s)+Cr^{3+}(aq.);E^o_{cell}=+1.53V$

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2 years ago

Which change favors the products in this reversible reaction n2o4(g)+58 kj 2no2 (g)?

Ksenya-84 [330]

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7 0

3 years ago

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