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Semenov [28]
3 years ago
11

Calculate the specific volume of Helium using the compressibility factor. 500 kPa, 60 degrees Celsius

Chemistry
1 answer:
IrinaK [193]3 years ago
7 0

Explanation:

Formula for compressibility factor is as follows.

                     z = \frac{P \times V_{m}}{R \times T}

where,     z = compressibility factor for helium = 1.0005

               P = pressure

          V_{m} = molar volume

                R = gas constant = 8.31 J/mol.K

                T = temperature

So, calculate the molar volume as follows.

                V_{m} = \frac{z \times R \times T}{P}

                             = \frac{1.0005 \times 8.314 \times 10^{-3} m^{3}.kPa/mol K \times (60 + 273)K}{500 kPa}

                             = 0.0056 m^{3}/mol

As molar mass of helium is 4 g/mol. Hence, calculate specific volume of helium as follows.

                    V_{sp} = \frac{V_{m}}{M_{w}}

                           = \frac{0.0056 m^{3}/mol}{4 g/mol}

                           = 0.00139 m^{3}/g

                           = 0.00139 m^{3}/g \times \frac{1 g}{10^{-3}kg}

                                 = 1.39 m^{3}/kg

Thus, we can conclude that the specific volume of Helium in given conditions is 1.39 m^{3}/kg.

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I2(g) + Cl2(g)2ICl(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.62 mol
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Answer:

The change in entropy of the surrounding is -146.11 J/K.

Explanation:

Enthalpy of formation of iodine gas = \Delta H_f_{(I_2)}=62.438 kJ/mol

Enthalpy of formation of chlorine gas = \Delta H_f_{(Cl_2)}=0 kJ/mol

Enthalpy of formation of ICl gas = \Delta H_f_{(ICl)}=17.78 kJ/mol

The equation used to calculate enthalpy change is of a reaction is:  

\Delta H_{rxn}=\sum [n\times \Delta H_f(product)]-\sum [n\times \Delta H_f(reactant)]

For the given chemical reaction:

I_2(g)+Cl_2(g)\rightarrow 2ICl(g),\Delta H_{rxn}=?

The equation for the enthalpy change of the above reaction is:

\Delta H_{rxn}=[(2\times \Delta H_f_{(ICl)})]-[(1\times \Delta H_f_{(I_2)})+(1\times \Delta H_f_{(Cl_2)})]

=[2\times 17.78 kJ/mol]-[1\times 0 kJ/mol+1\times 62.436 kJ/mol]=-26.878 kJ/mol

Enthaply change when 1.62 moles of iodine gas recast:

\Delta H= \Delta H_{rxn}\times 1.62 mol=(-26.878 kJ/mol)\times 1.62 mol=-43.542 kJ

Entropy of the surrounding = \Delta S^o_{surr}=\frac{\Delta H}{T}

=\frac{-43.542 kJ}{298 K}=\frac{-43,542 J}{298 K}=-146.11 J/K

1 kJ = 1000 J

The change in entropy of the surrounding is -146.11 J/K.

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Carbon-14 is radioactive and decays by beta decay. That means one of its neutrons spontaneously turns into a proton, an electron, and a neutrino, according to:

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