Complete the chemical equation for this reaction.

One mole of each of these compounds is dissolved in water. Which will result in the solution with the greatest conductivity?

antiseptic1488 [7]

Answer:

1. NaCl .

Explanation:

Hello there!

In this case, it is necessary to keep in mind that just ionic compounds are able to conduct electricity and therefore, the more ionic the compound is, the more electricity it conducts. In such a way, we may be able to predict how ionic these compounds are, considering that the electronegativity increases from bottom to top and from left to right.

1. NaCl: this is the most ionic compound since it is at the leftmost group and bonded with chlorine, so this is the most conductive one.

2. Mg(CIO3)2: Mg is bonded to O, not to Cl, which makes the compound ionic but not as ionic as NaCl.

3. NiCl: Ni is more electronegative than Na and Mg, so even when this is ionic, it is not as ionic as NaCl.

4. CaCl2: This is similar to NaCl but since Ca is in group 2A, it is more electronegative than Na, which makes CaCl2 conductive but not as much as NaCl.

Best regards!

8 0

3 years ago

The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol.

larisa86 [58]

Answer:

The great jump in ionization energy indicates that the most stable form of the sodium atom- the noble gas configuration, was reached after the removal of the first electron.

Explanation:

Sodium atom has an electronic configuration of 2,8,1. After the first electron has been removed from a sodium atom, the ion formed now has a noble gas configuration which assigns stability to it.

Noble gases have very high ionization energy due to the stability conferred on the by virtue of their completely filled outermost shells. They do not have need to lose electrons to attain stability. Also, because they have the most protons of their period, their atomic radius is reduced as electrons are pulled into the nucleus.

So, the great jump in ionization energy indicates that the most stable form of the sodium atom- the noble gas configuration, was reached after the removal of the first electron.

5 0

4 years ago

Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.660 V when (Zn^2+)=0.22 M and(

yaroslaw [1]

Answer:

pH = 2.059

Explanation:

At the Cathode:

The reduction reaction is:

$2H^+ + 2e^- \to H_2 \ \ \ \mathbf{E^0_{red}= 0.00 \ V}$

At the anode:

At oxidation reaction is:

$Zn \to Zn^{2+} +2e^- \ \ \ \mathbf{E^0_{ox} = 0.76 \ V}$

The overall equation for the reaction is:

$\mathbf{Zn + 2H^+ \to Zn^{2+} + H_2}$

The overall cell potential is:

$\mathbf{E^0_{cell}= E^0_{ox} + E^0_{red}}$

$\mathbf{E^0_{cell}= 0.76 \ V +0.00 \ V}$

$\mathbf{E^0_{cell}= 0.76\ V}$

Using the formula for the Nernst equation:

$E = E^0 - ( \dfrac{0.0591}{n})log (Q)\\$

where;

E = 0.66

(Zn^2+)=0.22 M

Then

$0.66 =0.76- ( \dfrac{0.0591}{2})log \bigg ( \dfrac{[Zn^{2+} ] PH_2}{[H^+]^2} \bigg )$

$0.66 =0.76- 0.02955 * log \bigg ( \dfrac{0.22*0.87}{[H^+]^2} \bigg )$

3.4 = log ( 0.1914) - 2 log [H⁺]

3.4 = -0.7180 - 2 log [H⁺]

3.4 + 0.7180 = - 2 log [H⁺]

4.118 = - 2 log [H⁺]

pH = log [H⁺] = 4.118/2

pH = 2.059

8 0

3 years ago

Write a balanced net ionic equation (include physical states) for the following reaction: HClO2(aq)+NaOH(aq)=H2O(l)+NaClO2(aq)

GuDViN [60]

To write the <span>balanced net ionic equation (include physical states) for the following reaction it should be the below:

</span><span>HClO2(aq) + OH^-(aq) ==> H2O(l) + ClO2^-(aq)
</span>
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3 0

4 years ago

Read 2 more answers

A neutralization reaction between an acid and a metal hydroxide produces

Vikki [24]

Answer:

A neutralization reaction between an acid and a metal hydroxide produces salt and water.

Explanation:

In a neutralization reaction, an acid and a base are combined according to the following example (hydrochloric acid and sodium hydroxide):

HCl + NaOH ---> H20 + NaCl

They are generated as products: water and a salt, in this case sodium chloride.

3 0

4 years ago