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mojhsa [17]
2 years ago
8

In a beaker, 300 grams of water at 80°C cools down to 20°C. Assume all the heat from the water is absorbed by 100 cubic meters o

f air, with a mass of 100.000 grams . What is the temperature change in the air?
Chemistry
1 answer:
scZoUnD [109]2 years ago
4 0

Answer:

mass of water, mw = 300g = 0.3kg

∆Tw = (80 - 20) °C

volume of air, va = 100m³

mass of air, ma = 100g = 0.1kg

∆Ta = ?

H = mc∆T

Hw = mwcw∆Tw

Hw = 0.3*4200*60

Hw = 75600J

Hw = 75.6 kJ

All the above heat energy got absorbed by air,

that is; Ha = 75600J

since it's given that the heat was absorbed by a specific amount of volume of air

then specific capacity of volume of air is

then,

ca = <u>Ha</u><u> </u> × <u>density</u><u> </u>

ma temp

then,

Ha = vaca∆Ta

where, ca = volumetric heat capacity of air = 0.012kJ/m³°C

75.6kJ = 100m³ × 0.012kJ/m³°C × ∆Ta

75.6 = 1.2/°C × ∆Ta

∆Ta = 63°C

63°C is the temperature change in air.

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At a constant temperature, 600 mL of an ideal gas is at a pressure of 760 mmHg . If the volume is decreased to 300 mL, the press
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Answer:

1520mmHg

Explanation:

Data obtained from the question include:

V1 (initial volume) = 600 mL

P1 (initial pressure) = 760 mmHg

V2 (final volume) = 300 mL

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Using the Boyle's law equation P1V1 = P2V2, the final pressure of the gas can easily be obtained as shown below:

P1V1 = P2V2

760 x 600 = P2 x 300

Divide both side by 300

P2 = (760 x 600) /300

P2 = 1520mmHg

The final pressure of the gas is 1520mmHg

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g modenr vacuum pumps make it easy to attain pressures of the order of in the laboratory. at a preasusure of 6.75 atm and an ord
Ratling [72]

Answer:

Number of molecules = 1.8267×10^20

Explanation:

From the question, we can deuced that the gases behave ideally, the we can make use of the ideal gas equation, which is expressed below;

PV = nRT

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P =pressure

V =volume

n = the number of moles

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