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ArbitrLikvidat [17]
3 years ago
9

Which waves move by replacing one particle with another? A) light waves B) sound waves C) electrostatic waves D) electromagnetic

waves
Chemistry
2 answers:
ANEK [815]3 years ago
8 0
<span>Answer: B) sound waves</span>

<span> There are 2 classifications of waves according to the media of propagation.</span>

<span> <span>Mechanical Waves – needs a medium, an example is sound waves. Sound waves do not travel through a vacuum. Sound waves move by replacing one particle with another. Particles vibrate and that is why we hear the sounds.</span> <span>Electromagnetic Waves and electrostatic waves are one but the same. They do<span> not require a medium.  – an example is light waves.</span></span> </span>
Bumek [7]3 years ago
7 0

i think it is B) because Sound waves move by replacing one particle with another. Sound waves require a medium to propagate, or move. Light and electromagnetic waves do not require a medium. Electrostatic are not a type of wave.

hope this helps

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Why is it important to use low flame when evaporating water from a recovered filtrate?
goldfiish [28.3K]

It is important to use low flame when evaporating water from a recovered filtrate because then the water and filtrate will not spatter and the filtrate can also be recovered after evaporating water.

If flame is not low then water as well as got spatter so it is important to use low flame so that   the water and filtrate will not spatter.


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3 0
2 years ago
A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both sol
Reika [66]

Answer : The enthalpy change for the process is 52.5 kJ/mole.

Explanation :

Heat released by the reaction = Heat absorbed by the calorimeter + Heat absorbed by the solution

q=[q_1+q_2]

q=[c_1\times \Delta T+m_2\times c_2\times \Delta T]

where,

q = heat released by the reaction

q_1 = heat absorbed by the calorimeter

q_2 = heat absorbed by the solution

c_1 = specific heat of calorimeter = 12.1J/^oC

c_2 = specific heat of water = 4.18J/g^oC

m_2 = mass of water or solution = Density\times Volume=1/mL\times 100.0mL=100.0g

\Delta T = change in temperature = T_2-T_1=(26.3-20.2)^oC=6.1^oC

Now put all the given values in the above formula, we get:

q=[(12.1J/^oC\times 6.1^oC)+(100.0g\times 4.18J/g^oC\times 6.1^oC)]

q=2623.61J

Now we have to calculate the enthalpy change for the process.

\Delta H=\frac{q}{n}

where,

\Delta H = enthalpy change = ?

q = heat released = 2626.61 J

n = number of moles of copper sulfate used = Concentration\times Volume=1M\times 0.050L=0.050mole

\Delta H=\frac{2623.61J}{0.050mole}=52472.2J/mole=52.5kJ/mole

Therefore, the enthalpy change for the process is 52.5 kJ/mole.

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3 years ago
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