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Bond [772]
3 years ago
11

The pressure in an automobile tire depends on thetemperature of the air in the tire. When the air temperature is25°C, the pressu

re gage reads 210 kPa. If the volume of the tire is 0.025 m3, determine the pressure rise in the tire whenthe air temperature in the tire rises to 50°C. Also, determinethe amount of air that must be bled off to restore pressure toits original value at this temperature. Assume the atmosphericpressure to be 100 kPa.
Engineering
1 answer:
KonstantinChe [14]3 years ago
8 0

Answer:

The pressure rise in the tire when the air temperature in the tire rises to 50°C is 337.43 KPa.

The amount of air that must be bled off to restore pressure 0.007 Kg

Explanation:

Knowing

T1 = 25°C = 298 K

T2 = 50°C = 323 K

volume of the tire = V = 0.025 m^{3}

P = 210 kPa (gage)

Pabs = 210 + 101 = 311 KPa

Before the temperature rise

P1 V1 = m1 R1 T1

m1 = \frac{P1 V1}{R1 T1} = \frac{310 * 10^{3} * 0.25 }{287 - 298} = 0.091 Kg\\ \\

After the temperature rise

P2 = \frac{m2 * R * T2}{V2} = \frac{0.091 *287*323 }{0.025} = 337.43 KPa

after bleeding the pressure and the volume returns  to its first value

P1 = P2 and V1 = V2

then

\frac{m2 * R * T2}{V} = \frac{m1 * R * T1}{V}

m2 = \frac{m1*T1}{T2}

m2 = \frac{0.091*298}{332} = 0.084 Kg\\\\

mbleed = m1 - m2 --> mbleed = 0.91 - 0.84 = 0.007 Kg

P2 = 337.43 KPa

mbleed = 0.007 Kg

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Explanation:

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here, the mean is 9, total numbers are 10.. so the sum will be 9 multiplied by 10, that is 90.

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Answer:

Jordan has more green paints

Explanation:

Given

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Required

Which paint does he have more?

For better understanding, it's better to convert both measurements to decimal.

For the green paint:

Green = \frac{5}{8}

Green = 0.625

For the blue paint:

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How wold you classify the earliest examples of S.T.E.M discoveries provided in this lesson?
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A spring-loaded piston-cylinder contains 1 kg of carbon dioxide. This system is heated from 104 kPa and 25 °C to 1,068 kPa and 3
labwork [276]

Answer:

Q = -68.859 kJ

Explanation:

given details

mass co_2 = 1 kg

initial pressure P_1 = 104 kPa

Temperature T_1 = 25 Degree C = 25+ 273 K = 298 K

final pressure P_2 = 1068 kPa

Temperature T_2 = 311 Degree C = 311+ 273 K = 584 K

we know that

molecular mass of co_2 = 44

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c_v = 0.657 kJ/kgK

from ideal gas equation

PV =mRT

V_1 = \frac{m RT_1}{P_1}

       =\frac{1*0.189*298}{104}

V_1 = 0.5415 m3

V_2 = \frac{m RT_2}{P_2}

     =\frac{1*0.189*584}{1068}

V_1 = 0.1033 m3

WORK DONE

W =P_{avg}*{V_2-V_1}

w = 586*(0.1033 -0.514)

W =256.76 kJ

INTERNAL ENERGY IS

\Delta U  = m *c_v*{V_2-V_1}

\Delta U  = 1*0.657*(584-298)

\Delta U  =187.902 kJ

HEAT TRANSFER

Q = \Delta U  +W

   = 187.902 +(-256.46)

Q = -68.859 kJ

7 0
3 years ago
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