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kumpel [21]
3 years ago
8

How much heat is released when 105g of steam at 100.0C is cooled to ice at -15C? Enthalpy of vaporization of water is 40.67kj/mo

l, the enthalpy of fusion of water is 6.01kj/mol, the molar heat capacity of water is 75.4J/(mol.C) and the molar heat capacity of ice is 36.4J/(mol.C)
Chemistry
2 answers:
densk [106]3 years ago
4 0

Answer:

4909.486Kj/mol

Explanation:

the heat would be required to change steam at 100°c to water at 100°c then change the water at that temperature to water at 0°c then change water at 0°c to ice at 0°c then ice at 0°c to ice at -15°c

Anika [276]3 years ago
4 0

Answer : The heat released is, 319.28 kJ

Solution :

The conversions involved in this process are :

(1):H_2O(g)(100^oC)\rightarrow H_2O(l)(100^oC)\\\\(2):H_2O(l)(100^oC)\rightarrow H_2O(l)(0^oC)\\\\(3):H_2O(l)(0^oC)\rightarrow H_2O(s)(100^oC)\\\\(4):H_2O(s)(0^oC)\rightarrow H_2O(s)(-15^oC)

Now we have to calculate the enthalpy change.

\Delta H=n\times \Delta H_{condensation}+[n\times c_{p,l}\times (T_{final}-T_{initial})]+n\times \Delta H_{freezing}+[n\times c_{p,s}\times (T_{final}-T_{initial})]

where,

\Delta H = enthalpy change = ?

Mass of water = 105 g

Moles of water = \frac{\text{Mass of water}}{\text{Molar mass of water}}=\frac{105g}{18g/mole}=5.83mole

c_{p,s} = specific heat of solid water = 36.4J/(mol.^oC)

c_{p,l} = specific heat of liquid water = 75.4J/(mol.^oC)

\Delta H_{freezing} = enthalpy change for freezing = enthalpy change for fusion = - 6.01 KJ/mole = - 6010 J/mole

\Delta H_{condensation} = enthalpy change for condensation = enthalpy change for vaporization = -40.67 KJ/mole = -40670 J/mole

Now put all the given values in the above expression, we get

\Delta H=5.83mole\times -40670J/mole+[5.83mole\times 75.4J/(mol.^oC)\times (0-100)^oC]+5.83mole\times -6010J/mole+[5.83mole\times 36.4J/(mol.^oC)\times (-15-0)^oC]

\Delta H=-319285.78J=-319.28KJ     (1 KJ = 1000 J)

Negative sign indicates that the heat is released during the process.

Therefore, the heat released is, 319.28 KJ

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Answer: (Structure attached).

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Normally, a mixture of <em>ortho-para</em> substituted products would be obtained. However, since both <em>para</em> positions are occupied, only the <em>ortho </em>substituted product is obtained here.

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3 years ago
Three 6−l flasks, fixed with pressure gauges and small valves, each contain 6 g of gas at 276 k. flask a contains ch4, flask b c
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First, please check the missing part in your question in the attachment.

a) So first, the Rank of pressure:

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B) The rank of average molecular kinetic energy:

when K = 3/2 KB T

when K is the average kinetic energy per molecule of gas 

and KB is Boltzmann's constant

and T is the temperature (K)

So from this equation, we can know that K only depends on T value, and when we have the T constant here for A, B, and C So the rank of K will be like the following:

∴ A = B = C

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R2/R1 = √M1/M2

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A > B > C

D) The rank of the Total kinetic energy of the molecules:

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∵ Mw A < Mw B < Mw C 

∴no .of molecules of A > B >C

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e) the rank of density:

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so the density also will be the same, ∴ the rank of the density is:

A = B = C

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we have no.of molecules of A > B > C as Mw A < B < C 

∴the rank of the collision frequency is:

A > B > C 

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A) CH2CHCOOH . Here you have 3 atoms of C but 4 atoms of H. That means this compound is not an isomer.

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