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earnstyle [38]
2 years ago
12

What did Thomson’s and Rutherford’s experiments have in common?

Chemistry
1 answer:
Alchen [17]2 years ago
8 0

Answer:

The answer is A.

Explanation:

They both used charged particles in their experiments.

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Give three examples of environmental, industrial and bio-chemistry.
JulsSmile [24]

Three examples of environmental, industrial and bio-chemistry are listed below:

  • Environmental chemistry: Contamination, Atmospheric Deposition, and Soil Pollution.
  • industrial chemistry:  industrial inorganic chemicals, industrial organic chemicals, and agricultural chemicals
  • bio-chemistry: genetic, immunology, and enzymology

<h3>Meaning of Chemistry</h3>

Chemistry can be defined as a branch of science which is concerned with the substances matter is composed of, their properties and reactions,

Chemistry also deals with the use of such reactions to form new substances.

In conclusion, Three examples of environmental, industrial and bio-chemistry are listed anove

Learn more about chemistry: brainly.com/question/24419453

#SPJ1

4 0
2 years ago
What is meant by the octet rule? What electrons are involved? How does this affect how elements bond?
FromTheMoon [43]

Answer:

The octet rule is a chemical rule of thumb that reflects the observation that main group elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas

Explanation:

4 0
2 years ago
The reaction for the combustion of methane is shown below. If 28.70g of methane
antiseptic1488 [7]
Omg hard question but it’s also amazing imma think about that question
8 0
2 years ago
Complete combustion of 3.20g of a hydrocarbon produced 9.69g of CO2 and 4.96g of H2O. What is the empirical formula for the hydr
vlabodo [156]

Let empirical formula for hydrocarbon is CxHy

it will undergo combustion as

CxHy + (x + y/4) O2  ---> xCO2 + (y/2 )H2O

Given that mass of CO2 produced = 9.69 g

So moles of CO2 produced = 9.69 / 44 = 0.22 moles

So moles of carbon present = 0.22 moles

mass of H2O produced = 4.96 g

Moles of H2O produced = mass / molar mass = 4.96 / 18 = 0.28 moles

So moles of H present = 2 X 0.28 = 0.56 moles

Let us divided the moles of each with lowest value of moles

Moles of Carbon = 0.22 / 0.22 = 1 moles

moles of H = 0.56 / 0.22 = 2.55

Multiplying with two to get whole number

the ratio of carbon and hydrogen will be : C:H = 2:5

empirical formula : C2H5


4 0
2 years ago
Read 2 more answers
A 2.5 g sample of french fries is placed in a calorimeter with 500.0 g of water at an initial temperature of 21 °C. After combus
SIZIF [17.4K]
Q=m°C<span>ΔT
=(500g) x (1 cal/g.</span>°C) x (48°C-21°C) = 13500 cal
13500 cal / 1000 = 13.5 kcal

<span>"What is the caloric value (kcal/g) of the french fries?"
13.5 kcal/ 2.5 g = 5.4 kcal/g</span>
8 0
3 years ago
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