Ice (H2O) melting at 273 K and 1 atm has = 6.01 kJ/mol and = 6.01 kJ/mol while water vaporizing under the same conditions has = 37.6 kJ/mol and = 40.7 kJ/mol. Why is there such a large difference between and , but not for and ?

Answers

Answer 1

Answer:

Degree of intermolecular hydrogen bonding

Explanation:

The energy required to melt a solid substance and the temperature at which the solid melts depends on the structure of the solid crystal as also on the magnitude of the intermolecular forces present in the solid.

Ice is less dense than liquid water, there are spaces in the crystal structure of ice. Secondly, the magnitude of hydrogen bonding in ice is lower due to lower intermolecular interaction between the water molecules. Given the lower intermolecular interaction in ice, the heat of fusion is much lower since the intermolecular interactions are easier to break.

In liquid water, hydrogen bonding is much stronger and there is greater intermolecular interaction between the water molecules. It takes more energy to break down these intermolecular interactions, hence the high enthalpy of vaporization of liquid water.

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Answers

Visible light
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Hope this is helpfull! :D
~Korey

According to one acid-base theory, a water molecule acts as an acid when the water molecule(1) accepts an H+ (3) donates an H+
(2) accepts an OH– (4) donates an OH–

Answers

A water molecule acts as an acid when the water molecule donates an H+.

The correct option is 3, donates an H+.

What is the acid-base theory?

The Acid-base theory tells that if a substance produce hydrogen ion is called as an acid.

If the substance accepts, a hydrogen ion is called as base.

This theory is given by Arrhenius.

Thus, the correct option is 3, donates an H+.

Learn more about acids, here:

brainly.com/question/1515003

According to one acid-base theory, a water molecule acts as an acid when the water molecule (3) donates an H+.

Iron in the form of fine wire burns in oxygen to form iron (III) oxide. Write the balanced chemical equation.

Answers

$2Fe+3O_2=2Fe_2O_3$

Rank standard molar entropy without a data table? Without referring to a data table, rank the following compounds by standard molar entropy (highest to lowest). I can do it with a data table but not sure how to proceed without. Thank you for your help. N2(g) H2(g) C2H4(g)

Answers

I think the correct order from most entropy to least entropy is C2H4, N2, and H2. My reasoning is that C2H4 has the biggest number of microstates which means that it will have the most entropy since it. I then based N2 and H2 from there weights (which indicates size) since the larger something is the more microstates it is likely to have. I hope that helps. Let me know if anything is unclear or if you want me to add more detail.

As carbon dioxide sublimes, its entropy
(1) decreases (2) increases (3) remains the same

Answers

Answer: (2) increases

Explanation: Entropy is the measure of randomness or disorder of a system. More is the random arrangement of molecules in a system , more is the entropy of the system. More ordered is the arrangement of molecules in a system, less is the entropy of the system.

When carbon dioxide sublimes, it means solid carbon dioxide is directly changing to gaseous state without undergoing into liquid state, thus the molecules will be more random and thus the entropy will increase.

When something sublimes (Goes straight from solid to gas), it takes in energy, as it is an endothermic process, so its entropy increases

How many molecules of glucose are in a 2.0 mL of a 1.02 mM solution of glucose

Answers

One way of expressing concentration is by molarity. It is the amount of solute per unit volume of the solution. Usually, it takes the unit mol/L. The calculation for this problem is as follows:

1.02 mM = (1.02 mol / mL) (2.0 mL) = 2.04 mol

Thus, the solution has 2.04 mol of glucose.

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