Chemistry, 21.04.2020 00:03 mrashrafkotkaat

6. Air at 300°C and 130kPa ows through a horizontal 7-cm ID pipe at a velocity of 42.0m/s. (a) Calculate _ Ek W, assuming ideal-gas behavior. (b) If the air is heated to 400°C at constant pressure, what is Δ _ Ek _ Ek 400°C _ Ek 300°C? (c) Why would it be incorrect to say that the rate of transfer of heat to the gas in Part (b) must equal the rate of change of kinetic energy?

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Answer from: carlosd21151

Check the explanation

Explanation:

kindly check the attached image below to see the answer to question A and B

ΔE= ΔU + Δ $E_{k}$

From the above relation, it is clear that some heat energy used to raises the temperature of the air.

Hence, the internal energy is not equal to zero. Therefore, the rate of transfer of heat to air is not equal to the rate of thane in kinetic energy of the air.

That is ΔE ≠ Δ $E_{k}$

6. Air at 300°C and 130kPa ows through a horizontal 7-cm ID pipe at a velocity of 42.0m/s. (a) Calcu

Answer from: Itsyourgirllulu

a) $\delta E_k$ = 112.164 W

b) $\delta E_k$ = 42.567 W

c) From what we've explained in part b; increase in temperature of the system is caused by rate of heat transfer . Therefore, not all heat is used to increase kinetic energy. Hence, since not all the heat is used to increase the kinetic energy . It is not valid and it is incorrect to say that rate of heat transfer is equal to the change in kinetic energy.

Explanation:

The given data include:

Inlet diameter (d_1) = 7 cm = 0.7 m

Inlet velocity (v_1) = 42 m/s

Inlet pressure (P_1) = 130 KPa

Inlet temoerature (T_1) = 300°C = (300 + 273.15) = 573.15 K

a) Assuming Ideal gas behaviour

Inlet Volumetric flowrate (V_1) = Inlet velocity (v_1) × area of the tube

$= v_1*(\frac{\pi}{4})0.07^2\\\\= 0.161635 \ m^3/s$

Using Ideal gas law at Inlet 1

P_1V_1 =nRT_1

where ; n = molar flow rate of steam

making n the subject of the formula; we have:

$n = \frac{P_1V_1}{RT_1}$

$n = \frac{130*42}{8.314*573.15}$

$n= 4.4096*10^{-3} \ Kmol/s$

Moleular weight of air = 28.84 g/mol

The mass flow rate = molar flowrate × molecular weight of air

$= 4.4096*10^{-3} \ * 28.84\\= 0.12717 \ kg/s$

Finally: the kinetic energy at Inlet $(\delta E_k) = \frac{1}{2}*mass \ flowrate *v_1^2$

= 0.5*0.12717*42^2

= 112.164 W

b) If the air is heated to 400°C;

Then temperature at 400°C = (400 + 273.15)K = 673.15 K

Thee pressure is also said to be constant ;

i.e P_1= P_2 = 130 KPa

Therefore; the mass flow rate is also the same ; so as the molar flow rate:

Thus; $n= 4.4096*10^{-3} \ Kmol/s$

Using Ideal gas law at Inlet 2

P_2V_2 = nRT_2

making V_2 the subject of the formula; we have:

$V_2 = \frac{nRT_2}{P_2}$

$V_2 = \frac{4.4906*10^{-3}*8.314*673.15}{130}$

$V_2 = 0.189836 \ m^3/s$

Assuming that the diameter is constant

$d_1 = d_2 = 0.07 \ cm$

Now; the velocity at outlet = $\frac{V_2}{\frac{\pi}{4}d_2^2}$

= $\frac{0.0189836}{\frac{\pi}{4}(0.07)^2}$

= 49.33 m/s

Change in kinetic energy $\delta E_k$ = $\frac{1}{2}*mass \ flowrate * \delta V$

= 0.5*0.12717 *(49.33^2 -42^2)

= 42.567 W

c).

From what we've explained in part b; increase in temperature of the system is caused by rate of heat transfer . Therefore, not all heat is used to increase kinetic energy. Hence, since not all the heat is used to increase the kinetic energy . It is not valid and it is incorrect to say that rate of heat transfer is equal to the change in kinetic energy.

Answer from: Quest

Ch4 is nonpolar and insoluble in water. since all of the hydrogen atoms are evenly spread around the carbon atom even through the c h bond is polar all the poles cancel each other out.

Answer from: Quest

And a) oxygen i believe

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6. Air at 300°C and 130kPa ows through a horizontal 7-cm ID pipe at a velocity of 42.0m/s. (a) Calcu...