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andriy [413]
3 years ago
13

In 1887, Albert A. Michelson and Edward W. Morley conducted an experiment to measure the speed at which the Earth moves through

the ether. Their experiment was so refined that it should have finally detected the luminiferous ether. But it didn't. Repeated trials verified the surprising result that the ether did not exist. How did the failure of the Michelson-Morley experiment change scientific theories of light? A. The Michelson-Morley experiment provided a new theory that fit the data better than the theory of the luminiferous ether did. B. The results of the Michelson-Morley experiment had to be rejected because the theory of the luminiferous ether was so well established. C. The results of the Michelson-Morley experiment did not fit the theory of the luminiferous ether, so the theory had to be rejected. D. The Michelson-Morley experiment proved that the luminiferous ether moved at the exact same speed as the Earth during all seasons of the year.
Chemistry
2 answers:
vichka [17]3 years ago
7 0
<span> C.The results of the Michelson-Morley experiment did not fit the theory of the luminiferous ether, so the theory had to be rejected. </span>
frutty [35]3 years ago
3 0

Answer:

The correct answer is option C. "The results of the Michelson-Morley experiment did not fit the theory of the luminiferous ether, so the theory had to be rejected".

Explanation:

The notorious Michelson-Morley experiment changed the way empty spaces were perceived at their time. Before 1887, the scientific community believed the existence of the luminiferous ether, a substance that supposedly was in empty spaces and allowed electromagnetic waves propagation. The results of the Michelson-Morley experiment did not fit the theory of the luminiferous ether, and the experiment was so refined that the theory had to be rejected.

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Which of the following is not a part of every scientific investigation?
Dmitry_Shevchenko [17]

Answer:

the correct answer is Group of answer choices

6 0
3 years ago
S
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Answer:

B

Explanation:

B

4 0
3 years ago
Why do gases diffuse more quickly than liquids?
Alborosie

Answer:

D)Gas particles move rapidly and have space between them.

Explanation:

Matter exists in three states namely: solids, liquids and gases. The particles contained in these three states are different from one another. In the gaseous state, the particles are FAR APART from one another i.e. space exists and they move at a very fast rate in contrast to the particles of a liquid, which have less space and move slower.

This rapid movement of gas particles within a less restricted space accounts for the reason why gaseous substances DIFFUSE more quickly than liquids.

5 0
3 years ago
A 1.00 g sample of octane (C8H18) is burned in a bomb calorimeter with a heat capacity of 837J∘C that holds 1200. g of water at
lubasha [3.4K]

Answer:

The heat of combustion for 1.00 mol of octane is  -5485.7 kJ/mol

Explanation:

<u>Step 1:</u> Data given

Mass of octane = 1.00 grams

Heat capacity of calorimeter = 837 J/°C

Mass of water = 1200 grams

Temperature of water = 25.0°C

Final temperature : 33.2 °C

<u> Step 2:</u> Calculate heat absorbed by the calorimeter

q = c*ΔT

⇒ with c = the heat capacity of the calorimeter = 837 J/°C

⇒ with ΔT = The change of temperature = T2 - T1 = 33.2 - 25.0 : 8.2 °C

q = 837 * 8.2 = 6863.4 J

<u>Step 3:</u> Calculate heat absorbed by the water

q = m*c*ΔT

⇒ m = the mass of the water = 1200 grams

⇒ c = the specific heat of water = 4.184 J/g°C

⇒ ΔT = The change in temperature = T2 - T1 = 33.2 - 25  = 8.2 °C

q = 1200 * 4.184 * 8.2 =  41170.56 J

<u>Step 4</u>: Calculate the total heat

qcalorimeter + qwater = 6863.4 + 41170. 56 = 48033.96 J  = 48 kJ

Since this is an exothermic reaction, there is heat released. q is positive but ΔH is negative.

<u>Step 5</u>: Calculate moles of octane

Moles octane = 1.00 gram / 114.23 g/mol

Moles octane = 0.00875 moles

<u>Step 6:</u> Calculate heat combustion for 1.00 mol of octane

ΔH = -48 kJ / 0.00875 moles

ΔH = -5485.7 kJ/mol

The heat of combustion for 1.00 mol of octane is  -5485.7 kJ/mol

8 0
3 years ago
4Cr(s)+3O2(g)→2Cr2O3(s) calculate how many grams of the product form when 21.4 g of O2 completely reacts
weqwewe [10]

Answer:

= 67.79 g

Explanation:

The equation for the reaction is;

4Cr(s)+3O2(g)→2Cr2O3(s)

The mass of O2 is 21.4 g, therefore, we find the number of moles of O2;

moles O2 = 21.4 g / 32 g/mol

                =0.669 moles

Using mole ratio, we get the moles of Cr2O3;

moles Cr2O3 = 0.669 x 2/3

                       =0.446 moles

but molar mass of Cr2O3 is 151.99 g/mol

Hence,

The mass Cr2O3 = 0.446 mol x 151.99 g/mol

                            <u> = 67.79 g </u>

6 0
3 years ago
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