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Allushta [10]
2 years ago
10

You are doing a peer review of a science experiment. The paper claims that an increase of pressure requires a greater addition o

f thermal energy to change a liquid to a gas. Why is this true?
Chemistry
1 answer:
Rus_ich [418]2 years ago
3 0

This is true because as thermal energy increases, molecules move faster and liquids are turned into gas.

States of matter is determined by the amount of energy possessed by the particles. Particles of a solid has the least amount of energy, liquid particles have more energy than solid particles while gas particles possess the highest amount of energy.

To increase the pressure of a substance, greater thermal energy is added to the substance by heating it up. This heat causes the molecules of the liquid to become more energetic and move faster .

As this occurs, intermolecular forces between the substance is broken as the liquid is converted to gas. The pressure. The energetic gas particles collide faster with the walls of the container thereby increasing the pressure.

Learn more: brainly.com/question/18124975

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A patient in need of treatment for the correction of a malocclusion would visit a/an
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4 0
3 years ago
How do you do part B?
galina1969 [7]
I cannot see the whole equation.Therefore I shall not answer

7 0
2 years ago
What volume of 1.10 M SrCl2 is needed to prepare 525 mL of 5.00 mM SrCl2?
grigory [225]

Answer:- 2.39 mL are required.

Solution:- It's a dilution problem and to solve this type of problems we use the dilution equation:

M_1V_1=M_2V_2

Where, M_1 and M_2 are molarities of concentrated and diluted solutions and V_1 and V_2 are their respective volumes.

M_1 = 1.10M

M_2 = 5.00mM = 0.005M    (since, mM stands for milli molar and M stands for molar. 1M = 1000mM)

V_1 = ?

V_2 = 525 mL

Let's plug in the given values in the formula:

1.10M(V_1)=0.005M(525mL)

V_1=(\frac{0.005M*525mL}{1.10M})

V_1=2.39mL

So, 2.39 mL of 1.10M are needed to make 525 mL of 5.00mM solution.

7 0
2 years ago
If 1 kg of fuel is used in the above fusion reaction (2 1H + 3 1H--&gt; 4 2He+1 0N) , the resulting helium has a mass of 0.993 k
enot [183]
Δmc
2

For one reaction:
Mass Defect =Δm
=2(m
H
​
)−m
He
​
−m
n
​

=2(2.015)−3.017−1.009
=0.004 amu
1 amu=931.5 MeV/c
2

Hence,
E=0.004×931.5 MeV=3.724 MeV
E=3.726×1.6×10
−13
J=5.96×10
−13
J

For 1 kg of Deuterium available,
moles=
2g
1000g
​
=500
N=500N
A
​
=3.01×10
26

Energy released =
2
N
​
×5.95×10
−13
J
=8.95×10
13
6 0
2 years ago
A balloon is filled with 0.250 mole of air at 35°C. If the volume of the balloon is 6.23 liters, what is the absolute pressure
lord [1]

Answer is:  the absolute pressure of the air in the balloon is 1.015 atm (102.84 kPa).

n = 0.250 mol; amount of substance.

V = 6.23 L; volume of the balloon.

T = 35°C = 308.15 K; temperature.

R = 0.08206 L·atm/mol·K, universal gas constant.

Ideal gas law: p·V = n·R·T.

p = n·R·T / V.

p = 0.250 mol · 0.08206 L·atm/mol·K · 308.15 K / 6.23 L.

p = 1.015 atm; presure of the air.

6 0
3 years ago
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