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Olin [163]
3 years ago
8

Specify whether each compound is soluble in hexane.Classify the appropriate items to their respective category.

Chemistry
1 answer:
igor_vitrenko [27]3 years ago
7 0

Answer:

hydrogen chloride (HC)- insoluble in hexane

hydrogen sulfide (H2S)- insoluble in hexane

water (H2O)- insoluble in hexane

propane (CH3CH2CH3)- soluble in hexane

Explanation:

Generally, it is a principle in chemistry that polar solvents dissolve polar substances while nonpolar solvents dissolve nonpolar substances.

This is because, dissolution of a substance in another substance depends on the kind of intermolecular interaction that is possible between the two substances. Hence, ionic substance dissolve in polar solvents due to dipole interactions and nonpolar substances dissolve in nonpolar solvents due to Vanderwaals interaction between the solute and solvent.

Hydrogen chloride, hydrogen sulphide and water are ionic substances hence they can not dissolve in hexane which is a nonpolar substance. However, propane is a nonpolar solvent hence it dissolves in hexane.

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Under standard-state conditions, which of the following species is the best reducing agent? a. Ag+ b. Pb c. H2 d. Ag e. Mg2+
eimsori [14]

<u>Answer:</u> The correct answer is Option b.

<u>Explanation:</u>

Reducing agents are defined as the agents which help the other substance to get reduced and itself gets oxidized. They undergo oxidation reaction.

X\rightarrow X^{n+}+ne^-

For determination of reducing agents, we will look at the oxidation potentials of the substance. Oxidation potentials can be determined by reversing the standard reduction potentials.

For the given options:

  • <u>Option a:</u>  Ag^+

This ion cannot be further oxidized because +1 is the most stable oxidation state of silver.

  • <u>Option b:</u>  Pb

This metal can easily get oxidized to Pb^{2+} ion and the standard oxidation potential for this is 0.13 V

Pb\rightarrow Pb^{2+}+2e^-;E^o_{(Pb/Pb^{2+})}=+0.13V

  • <u>Option c:</u>  H_2

This metal can easily get oxidized to H^{+} ion and the standard oxidation potential for this is 0.0 V

H_2\rightarrow 2H^++2e^-;E^o_{(H_2/H^{+})}=0.0V

  • <u>Option d:</u>  Ag

This metal can easily get oxidized to Ag^{+} ion and the standard oxidation potential for this is -0.80 V

Ag\rightarrow Ag^{+}+e^-;E^o_{(Ag/Ag^{+})}=-0.80V

  • <u>Option e:</u>  Mg^{2+}

This ion cannot be further oxidized because +2 is the most stable oxidation state of magnesium.

By looking at the standard oxidation potential of the substances, the substance having highest positive E^o potential will always get oxidized and will undergo oxidation reaction. Thus, considered as strong reducing agent.

From the above values, the correct answer is Option b.

8 0
3 years ago
What questions, if we were to answer them, would
Margarita [4]

Answer:

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Explanation:

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7 0
3 years ago
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When temperature of liquid is increased, liquid gets thinner and thinner and hence it's viscosity decreases.

Density = mass/volume.

As we increase the temperature, volume of the liquid starts to increase but mass of the liquid remains constant. As a result, density of liquid decreases.

Hope this helps!
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Answer:

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Explanation:

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