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Sav [38]
3 years ago
6

2HgCl2(aq) + C2O42–(aq) → 2Cl–(aq) +2CO2(g) + Hg2Cl2(s)

Chemistry
1 answer:
alexgriva [62]3 years ago
8 0

Explanation:

Expression for rate of the given reaction is as follows.

             Rate = k[HgCl_{2}]x [C_{2}O^{2-}_{4}]y[/tex]

Therefore, the reaction equations by putting the given values will be as follows.

       1.8 \times 10^{-5} = k[0.105]x [0.15]y ............. (1)

       7.2 \times 10^{-5} = k [0.105]x [0.30]y ........... (2)

       3.6 \times 10^{-5} = k [0.0525]x [0.30]y ............ (3)

Now, solving equations (1) and (2) we get the value of y = 2. Therefore, by solving equation (2) and (3)  we get the value of x = 1.

Therefore, expression for rate of the reaction is as follows.

     Rate = k[HgCl_{2}]x [C_{2}O^{2-}_{4}]y

          Rate = k [HgCl2]1 [C_{2}O^{-2}_{4}]2

Hence, total order = 1 + 2 = 3

According to equation (1),

               1.8 \times 10^{-5} = k[0.105]x [0.15]y  

            1.8 \times 10^{-5} = k [0.105]1 [0.15]2  

                      k = 7.6 \times 10^{-3} M^{-2} min^{-1}  

Thus, we can conclude that rate constant for the given reaction is 7.6 \times 10^{-3} M^{-2} min^{-1}.

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+<br> c)<br> FeCl3 +<br> NH4OH<br> Fe(OH)3<br> NHACI
bixtya [17]

The question is incomplete, the complete question is:

Write the net ionic equation for the below chemical reaction:

(c): FeCl_3+3NH_4OH\rightarrow Fe(OH)_3+3NH_4CI

<u>Answer:</u> The net ionic equation is Fe^{3+}(aq)+3OH^{-}(aq)\rightarrow Fe(OH)_3(s)

<u>Explanation:</u>

Net ionic equation is defined as the equations in which spectator ions are not included.

Spectator ions are the ones that are present equally on the reactant and product sides. They do not participate in the reaction.

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The balanced molecular equation is:

FeCl_3(aq)+3NH_4OH(aq)\rightarrow Fe(OH)_3(s)+3NH_4Cl(aq)

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As ammonium and chloride ions are present on both sides of the reaction. Thus, they are considered spectator ions.

The net ionic equation follows:

Fe^{3+}(aq)+3OH^{-}(aq)\rightarrow Fe(OH)_3(s)

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