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masya89 [10]
3 years ago
12

In parts of England during the 19th century, the peppered moth was widespread. This kind of moth comes in two color variations,

cream and gray. Prior to the Industrial Revolution, cream-colored moths were more common. However, after the Industrial Revolution, the population of gray-colored moths was found to be larger than that of cream-colored moths. What was most likely the reason for the increase in the number of gray moths? A. Cream moths were resistant to environmental changes during the Industrial Revolution. B. Gray moths were not affected by the Industrial Revolution. C. Changes during the Industrial Revolution increased the chance of survival and reproduction for gray-colored moths. D. Changes during the Industrial Revolution increased the chance of survival and reproduction for cream-colored moths.
Chemistry
2 answers:
snow_lady [41]3 years ago
8 0

Answer:

C

Explanation:

the gray moths were able to hide better in the smoky air then cream colored moth and were able to stay alive.

klio [65]3 years ago
3 0

Answer:

C

Explanation:

During the industrial revolution the grey moths could blend in more and have more camouflaged then the crème colored moths, that being said they had a better chance of reproduction and became more populated afterwards. hope this helps! :)

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According to the first law of thermodynamics, what quantity is conserved?.
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Answer:

energy

Explanation:

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How many milliliters of nitrogen, N2, would have to be collected at 99.19 kPa and 28oC to have a sample containing 0.015 moles o
Semmy [17]

Answer:

378mL

Explanation:

The following data were obtained from the question:

Pressure (P) = 99.19 kPa

Temperature (T) = 28°C

Number of mole (n) = 0.015 mole

Volume (V) =...?

Next, we shall convert the pressure and temperature to appropriate units. This is illustrated below:

For Pressure:

101.325 KPa = 1 atm

Therefore, 99.19 kPa = 99.19/101.325 = 0.98 atm

For Temperature:

T(K) = T(°C) + 273

T(°C) = 28°C

T(K) = 28°C + 273 = 301K.

Next we shall determine the volume of N2. The volume of N2 can be obtained by using the ideal gas equation as shown below:

PV = nRT

Pressure (P) = 0.98 atm

Temperature (T) = 301K

Number of mole (n) = 0.015 mole

Gas constant (R) = 0.0821atm.L/Kmol.

Volume (V) =...?

0.98 x V = 0.015 x 0.0821 x 301

Divide both side by 0.98

V = (0.015 x 0.0821 x 301) /0.98

V = 0.378 L

Finally, we shall convert 0.378 L to millilitres (mL). This is illustrated below:

1L = 1000mL

Therefore, 0.378L = 0.378 x 1000 = 378mL

Therefore, the volume of N2 collected is 378mL

4 0
3 years ago
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