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3 years ago

When the following two solutions are mixed:

Chemistry

2 answers:

Klio2033 [76]3 years ago

6 0

Answer:

For Part A: The spectator ions are $Fe^{3+}\text{ and }CO_3^{2-}$ and the ions that react are $K^+\text{ and }NO_3^-$

For Part B: The net ionic equation is given below.

Explanation:

Net ionic equation of any reaction does not include any spectator ions.

Spectator ions are defined as the ions which does not get involved in a chemical equation. They are found on both the sides of the chemical reaction when it is present in ionic form.

For Part A:

The chemical equation for the reaction of iron (III) nitrate and potassium carbonate is given as:

$2Fe(NO_3)_3(aq.)+3K_2CO_3(aq.)\rightarrow 6KNO_3(aq.) + Fe_2(CO_3)_3(s)$

Ionic form of the above equation follows:

$2Fe^{3+}(aq.)+2NO_3^-(aq.)+3K^+(aq.)+3CO_3^{2-}(aq.)\rightarrow 6K^+(aq.)+6NO_3^+(aq.)+Fe_2(CO_3)_3(s)$

As, potassium and nitrate ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation and are spectator ions.

The net ionic equation for the above reaction follows:

$2Fe^{3+}(aq.)+CO_3^{2-}(aq.)\rightarrow Fe_2(CO_3)_3(s)$

Hence, the spectator ions are $Fe^{3+}\text{ and }CO_3^{2-}$ and the ions that react are $K^+\text{ and }NO_3^-$

For Part B:

The chemical equation for the reaction of sulfuric acid and barium hydroxide is given as:

$Ba(OH)_2(aq.)+H_2SO_4(aq.)\rightarrow BaSO_4(s)+2H_2O(l)$

Ionic form of the above equation follows:

$Ba^{2+}(aq.)+2OH^-(aq.)+2H^+(aq.)+SO_4^{2-}(aq.)\rightarrow BaSO_4(s)+2H_2O(l)$

All the ions are present in this reaction. Thus, no ion is considered as spectator ions.

lyudmila [28]3 years ago

3 0

Answer:

PartA:

spectator ions: K+ and NO3-

ions that react: Fe+ and CO2-3

Explanation:

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nikitadnepr [17]

Answer:

$a)\ 2FeSO4 \xrightarrow{\text{Heat}} SO_3+SO_2+Fe_2O_3\\b)\ Decomposition\ Reaction$

Explanation:

Ferrous Sulphate $(FeSO4)$ is generally found as Lime-Green Crystals. On heating, these crystals almost immediately turn white-yellow. They then, break down to produce an anhydrous mixture of Sulphur Trioxide $(SO_3)$ , Sulphur Dioxide $(SO_2)$ as well as Ferric Oxide $(Fe_2O_3)$ .

We can hence, frame a skeletal equation of this reaction and try to balance it.

Hence,

$FeSO4 \xrightarrow{\text{Heat}} SO_3+SO_2+Fe_2O_3$

Now,

a)In order to balance it through the 'Hit &Trial Method', we'll follow a series of steps:

1. First, lets compare the number of Fe (Iron) atoms on the RHS and LHS. We find that, the no. of Fe Atoms on the RHS is twice the number of Fe Atoms on the LHS. We hence, add a co-effecient 2 beside $FeSO_4$ .

2. Now, Iron atoms, Sulphur Atoms and Oxygen atoms occur 2, 2, 8 respectively on both the sides:

Hence, As all the other elements as well as iron, balance, we've arrived upon our Balanced Equation :

$2FeSO4 \xrightarrow{\text{Heat}} SO_3+SO_2+Fe_2O_3$

b) We know that, decomposition reactions are [generally] endothermic reactions in which Large Compounds decompose into smaller elements and compounds. Here, as Ferrous Sulphate decomposes into Sulphur Dioxide, Sulphur Trioxide and Ferric Oxide, the reaction that occurs here is Decomposition Reaction.

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3 years ago

Determine the rate law, including the values of the orders and rate law constant, for the following reaction using the experimen

murzikaleks [220]

Answer: Rate law is, R= 6.02[A]¹[B]²

Explanation in attached image