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iogann1982 [59]
3 years ago
10

Write the balanced chemical equations, including states, for the neutralization reactions between: HI (aq) and NaOH (aq) H2CO3 (

aq) and Sr(OH)2 (s) *note the strontium compound will be a solid Ca(OH)2 (s) and H2SO4 (aq)
Chemistry
1 answer:
rewona [7]3 years ago
8 0

Answer:

* HI (aq) +NaOH (aq) \rightarrow NaI(aq)+H_2O(l)

* H_2CO_3 (aq) + Sr(OH)_2\rightarrow SrCO_3(s)+2H_2O(l)

* Ca(OH)_2 (s) +H_2SO_4 (aq)\rightarrow CaSO_4(aq)+2H_2O(l)

Explanation:

Hello!

In this case, since neutralization chemical reactions are carried out when an acid and a base react to produce a salt and water, for the first reaction, HI (aq) and NaOH (aq), we can write:

HI (aq) +NaOH (aq) \rightarrow NaI(aq)+H_2O(l)

Whereas the salt, sodium iodide remains aqueous and water liquid. Next, when carbonic acid and strontium hydroxide react, strontium carbonate as the salt precipitates out and water is also produced:

H_2CO_3 (aq) + Sr(OH)_2\rightarrow SrCO_3(s)+2H_2O(l)

Finally, when calcium hydroxide and sulfuric acid react, the compound calcium sulfate as the salt and water are produced as shown below:

Ca(OH)_2 (s) +H_2SO_4 (aq)\rightarrow CaSO_4(aq)+2H_2O(l)

Best regards!

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2 years ago
A 2.20 mol sample of NO 2 ( g ) is added to a 3.50 L vessel and heated to 500 K. N 2 O 4 ( g ) − ⇀ ↽ − 2 NO 2 ( g ) K c = 0.513
igor_vitrenko [27]

Answer:

[NO₂] = 0.434 M

[N₂O₄] = 0.0971 M

Explanation:

The equilibrum is:  N₂O₄(g)  ⇆  2NO₂ (g)

1 moles of nitrogen (IV) oxide is in equilibrium with 2 moles of nitrogen dioxide.

Initally we only have 2.20 moles of NO₂. So let's write the equilibrium again:

              2NO₂ (g)   ⇆   N₂O₄(g)      

Initially   2.20 mol              -

React          x                      x/2

X amount has reacted, and the half has been formed, according to stoichiometry.

Eq       (2.20-x) / 3.50L     (x/2)/ 3.50L

We divide by the volume because we need molar concentrations. Let's make the Kc's expression:

Kc = [N₂O₄] / [NO₂]²

0.513 = ((x/2)/ 3.50L) /  [(2.20-x) / 3.50L]

0.513 = ((x/2)/ 3.50L) / [(2.20-x)² / 3.50L²]

0.513 = ((x/2)/ 3.50L) / [2.20-x)² / 3.50L²]

0.513 = ((x/2)/ 3.50L) / (4.84 - 4.40x + x²) / 12.25)

0.513 / 12.25 (4.84 - 4.40x + x²) = x/2 / 3.50

0.203 - 0.184x + 0.0419x² = x/2 / 3.50

3.50(0.203 - 0.184x + 0.0419x²) = x/2

7 (0.203 - 0.184x + 0.0419x²) - x = 0

1.421 - 2.288x + 0.2933x² = 0  → Quadratic formula

a = 0.2933 ;  b = -2.288 ; c = 1.421

(-b +- √(b²-4ac)) / (2a)

x₁ = 7.12

x₂ = 0.68 → We consider this value, so we can have a (+) concentration.

Concentrations in the equilibrium are:

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[N₂O₄] = (0.68/2) / 3.50  = 0.0971 M

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