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quester [9]
2 years ago
11

NAME the four phases of matter and DESCRIBE how the intermolecular forces and kinetic energy change as you change phases.

Chemistry
1 answer:
weqwewe [10]2 years ago
5 0

Answer: Substances on Earth can exist in one of four phases, but mostly, they exist in one of three: solid, liquid or gas. Learn the six changes of phase: freezing, melting, condensation, vaporization, sublimation and deposition. Intermolecular forces are forces between molecules that determine the physical properties of liquids and solids. 11.2 Vaporization and Vapor Pressure— vaporization is the conversion of a liquid to a gas (vapor), and the quantity of heat associated with this phase change is known as the enthalpy (heat) of vaporization. When kinetic energy is increasing molecules are simply moving faster. However, when the potential energy is increasing molecules are changing phases. Therefore, when the potential energy is increasing is when the molecule is changing phases. Phase changes require either the addition of heat energy (melting, evaporation, and sublimation) or subtraction of heat energy (condensation and freezing). ... Changing the amount of heat energy usually causes a temperature change.

HOpe this helps..... Stay safe and have a Merry Christmas!!!!!!!!!! :D

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How does a scientist explain something when a controlled experiment cannot be carried out
Romashka [77]
<span> We look for evidence. There are numerous natural phenomenon that we can't observe happening in real-time because they happen over large time scales, or large spatial scales. But we can observe the effects of these phenomenon and make predictions about what other effects we should see. </span>
7 0
3 years ago
A 0.45-g sample of aspirin is decomposed into its constituent elements and found to contain 0.27 g C, 0.020 g H, and 0.16 g O. C
slamgirl [31]

Answer:

Explanation:

mass % of C = 0.27/0.45*100 = 60%

mass % of H = 0.02/0.45*100 = 4.4%

mass % of O = 0.16/0.45*100 = 35.6%

Total = 60%+4.4%+ 35.6% = 100%

3 0
3 years ago
At a certain temperature the vapor pressure of pure benzene is measured to be . Suppose a solution is prepared by mixing of benz
Marianna [84]

Answer:

P(C₆H₆) = 0.2961 atm

Explanation:

I found an exercise pretty similar to this, so i'm gonna use the data of this exercise to show you how to do it, and then, replace your data in the procedure so you can have an accurate result:

<em>"At a certain temperature the vapor pressure of pure benzene (C6H6) is measured to be 0.63 atm. Suppose a solution is prepared by mixing 79.2 g of benzene and 115. g of heptane (C7H16) Calculate the partial pressure of benzene vapor above this solution. Round your answer to 2 significant digits. Note for advanced students: you may assume the solution is ideal".</em>

<em />

Now, according to the data, we want partial pressure of benzene, so we need to use Raoul's law which is:

P = Xₐ * P°    (1)

Where:

P: Partial pressure

Xₐ: molar fraction

P°: Vapour pressure

We only have the vapour pressure of benzene in the mixture. We need to determine the molar fraction first. To do this, we need the moles of each compound in the mixture.

To get the moles:   n = m / MM

To get the molar mass of benzene (C₆H₆) and heptane (C₇H₁₆), we need the atomic weights of Carbon and hydrogen, which are 12 g/mol and 1 g/mol:

MM(C₆H₆) = (12*6) + (6*1) = 78 g/mol

MM(C₇H₁₆) = (7*12) + (16*1) = 100 g/mol

Let's determine the moles of each compound:

moles (C₆H₆) = 79.2 / 78 = 1.02 moles

moles (C₇H₁₆) = 115 / 100 = 1.15 moles

moles in solution = 1.02 + 1.15 = 2.17 moles

To get the molar fractions, we use the following expression:

Xₐ = moles(C₆H₆) / moles in solution

Xₐ = 1.02 / 2.17 = 0.47

Finally, the partial pressure is:

P(C₆H₆) = 0.47 * 0.63

<h2>P(C₆H₆) = 0.2961 atm</h2>

Hope this helps

7 0
3 years ago
Convert .004569g to mg
algol [13]

Answer:

4.569 mg

:)))))))))))))))

4 0
3 years ago
Read 2 more answers
The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. 2A(g)
monitta

Answer:

The value of the missing equilibrium constant ( of the first equation) is 1.72

Explanation:

First equation: 2A + B ↔ A2B   Kc = TO BE DETERMINED

 ⇒ The equilibrium expression for this equation is written as: [A2B]/[A]²[B]

Second equation: A2B + B ↔ A2B2   Kc= 16.4

⇒ The equilibrium expression is written as: [A2B2]/[A2B][B]

Third equation:  2A + 2B ↔ A2B2     Kc = 28.2

⇒ The equilibrium expression is written as: [A2B2]/ [A]²[B]²

If we add the first to the second equation

2A + B + B ↔ A2B2   the equilibrium constant Kc will be X(16.4)

But the sum of these 2 equations, is the same as the third equation ( 2A + 2B ↔ A2B2)   with Kc = 28.2

So this means: 28.2 = X(16.4)

or X = 28.2/16.4

X = 1.72

with X = Kc of the first equation

The value of the missing equilibrium constant ( of the first equation) is 1.72

7 0
3 years ago
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