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3 years ago

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

Chemistry

2 answers:

irina1246 [14]3 years ago

6 0

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

7nadin3 [17]3 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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Answer : The volume of $CO_2$ will be, 514.11 ml

Explanation :

The balanced chemical reaction will be,

$HCO_3^-+HCl\rightarrow Cl^-+H_2O+CO_2$

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As, 1 mole of $HCO_3^-$ react to give 1 mole of $CO_2$

So, 0.0202 mole of $HCO_3^-$ react to give 0.0202 mole of $CO_2$

The moles of $CO_2$ = 0.0202 mole

Now we have to calculate the volume of $CO_2$ by using ideal gas equation.

$PV=nRT$

where,

P = pressure of gas = 1.00 atm

V = volume of gas = ?

T = temperature of gas = $37^oC=273+37=310K$

n = number of moles of gas = 0.0202 mole

R = gas constant = 0.0821 L.atm/mole.K

Now put all the given values in the ideal gas equation, we get :

$(1.00atm)\times V=0.0202 mole\times (0.0821L.atm/mole.K)\times (310K)$

$V=0.51411L=514.11ml$

Therefore, the volume of $CO_2$ will be, 514.11 ml

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