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Gnom [1K]
3 years ago
14

9. Why do areas near large bodies of water tend to not experience large swings in temperature? (2 points)

Chemistry
2 answers:
Maslowich3 years ago
6 0
I think the correct answer from the choices listed above is the third option. Areas  near large bodies of water tend to not experience large swings in temperature because water has a high specific heat. <span>That's because water can take up lots of thermal energy, and thus preven wild swings in temperature. </span>
Serhud [2]3 years ago
4 0

Answer: Water has a high specific heat.

Explanation: Specific heat is the amount of  heat required to raise the temperature of 1 gram of substance through 1^0C.

Water has high value of specific heat as the water molecules are bonded strongly through hydrogen bonds. Thus a large amount of heat is required to break the bonds and increase the kinetic energy of molecules.

This is due to this reason that areas near large bodies of water tend to not experience large swings in temperature.

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A sample of matter was given the following description: The sample of the pure substance is blue in color with an octahedral sha
Alexeev081 [22]

Answer:

A crystalline solid

Explanation:

Most solids form with a regular arrangement of their particles because the overall attractive interactions between particles are maximized, and the total intermolecular energy is minimized, when the particles pack in the most efficient manner. The regular arrangement at an atomic level is often reflected at a macroscopic level.  Liquids dont use to have this kind of arrangements or shapes.

5 0
3 years ago
What are the 5 indicators of a chemical reaction? What are the 5 indicators of a chemical reaction? I only know 3 for sure:2) Ch
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Temperature change, colour change, releasing gas, bubbles and change in odor
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3 years ago
Calculate how many times more soluble Mg(OH)2 is in pure water Based on the given value of the Ksp, 5.61×10−11, calculate the ra
maks197457 [2]

Answer:

molar solubility in water = 2.412 * 10^-4  mol/L

molar solubility of NaOH in 0.130M = 3.32 * 10^-9 mol/L

Mg(OH)2 is a factor 0.73*10^5 more soluble in pure water than in 0.130 M NaOH

Explanation:

The Ksp refers to the partial solubilization of a mostly insoluble salt. This is an equilibrium process.

 

The equation for the solubilization reaction of Mg(OH)2 can be given as:

 

Mg(OH)2 (s) → Mg2+ (aq) + 2OH– (aq)

 Ksp can then be given as followed:

Ksp = [Mg^2+][OH^–]²  

<u>Step 2:</u> Calculate the solubility in water

Mg(OH)2 (s) → Mg2+ (aq) + 2OH– (aq)

The mole ratio Mg^2+ with OH- is 1:2

So there will react X of Mg^2+ and 2X of OH-

The concentration at equilibrium will be XM Mg^2+ and 2X OH-

Ksp = [Mg^2+][OH^–]²  

5.61*10^-11 = X * (2X)² = X *4X² = 4X³

 X = <u>2.412 * 10^-4 mol/L = solubility in water</u>

<u>Step 3</u>: Calculate solubility in 0.130 M NaOH

The initial concentration of Mg^2+  = 0 M

The initial concentration of OH- = 0.130 M

The mole ratio Mg^2+ with OH- is 1:2

So there will react X of Mg^2+ and 2X +0.130 for OH-

The concentration at equilibrium will be XM Mg^2+ and 0.130 + 2X OH-

The value of "[OH–] + 2X" is, because the very small value of X, equal to the value of [OH–] .

Let's consider:

[Mg+2] = X

[OH] = 0.130

Ksp = [Mg^2+][OH^–]²  

5.61*10^-11 = X *(0.130)²  

5.61*10^-11 = X * (0.130)^2

X = <u>3.32*10^-9 = solubility in 0.130 M NaOH </u>

<u>Step 4:</u> Calculate how many times Mg(OH)2 is better soluble in pure water.

(2.412*10^-4)/ (3.32*10^-9) = 0.73 * 10^5

Mg(OH)2 is a factor 0.73*10^5 more soluble in pure water than in 0.130 M NaOH

4 0
3 years ago
What is the overall equation for the covalent bond in H2O . Is it H2 + O2=H2O OR. H2 + O = H2O
AlexFokin [52]

Answer:

The answer is in the photo

Explanation:

I hope that is useful for you :)

4 0
3 years ago
Can you substitute evaporated milk for condensed milk
alex41 [277]
Yes because condensed milk and evaporated milk are similar to one another. However, there won’t be the same sweet flavor but the texture is the same.
3 0
3 years ago
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