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3 years ago

A racoon has 8 levels of classification. In which level would you find an organism more closely related to a racoon?

Chemistry

2 answers:

disa [49]3 years ago

8 0

Answer:

class

Explanation:

leva [86]3 years ago

3 0

Answer:

b. same class

Explanation:

because domain is sort of like a different species but same classification means it is in the FAMILY of raccoons.

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How many moles are in 15.94g of water?

Semmy [17]

Your answer would be 0,8856 mol H2O.

Molar mass of H2O is approximately 18 g/mol

15.94/18 = 0,8856 mol H2O

8 0

4 years ago

Write a transmutation nuclear equation that represents an example of fission

morpeh [17]

Answer:

²³⁸₉₂U → ²³⁴₉₀Th + ⁴₂He

Explanation:

Nuclei higher than Bi - 92 naturally are radioactive.

In a transmutation reaction, a new element is produced from an existing one due to radioactivity.

Nuclear fission is the radioactive process by which a heavy nucleus spontaneously decays into lighter ones with the release of a large amount of energy.

One example is the transmutation of uranium into thorium;

²³⁸₉₂U → ²³⁴₉₀Th + ⁴₂He

4 0

3 years ago

Which statement is true? Postively charged objects attract other positively charged objects negatively charged objects attract o

ANEK [815]

Answer:

Explanation:one is true because if it is positiveit would not be attracting it would be sepperating

8 0

3 years ago

3. Besides the major types of radioactive decay, there are two others: positron emission and electron capture.

Vanyuwa [196]

Answer 1: The electron is a subatomic particle that has a negative charge. Electron cannot be sub-divided further. An electron has a mass that ia ~ 1/1836 that of the proton.
The positron is also refereed as an antielectron. The positron has the charge of +1e, a spin of 1⁄2. The similarity between positron and electron is that they have same mass.

Answer 2: Positron decay occurs in nuclei having heavy mass. Positron emission decreases proton number relative to the neutron number. Positron also exhibits nuclear transmutation thereby producing an atom of a different element, as compared to parent element,. Them atomic number of daughter element is less as compared to parent element by 1.

Example: 23 12Mg → 23 11Na + e+ + energy

Answer 3: Electron capture is also referred as K-electron capture. It involves absorption of energy, thereby resulting in loss of electron usually from K or L shell. In this process,following thing occurs simultaneously
i) a nuclear proton present in nuclei changes to a neutron, after reacting with an electron which falls into the nucleus from one of its orbitals (preferentially from K or L)
2) Emission of an electron neutrino.
Following is an example of K-electron capture.
7 4Be + 0 -1e → 7 3Li + energy

Answer 4: Following are the distinct features of transmutations caused by positron emissions and electron capture.
i) Positron: A proton get converted into neutron due to radio-active process. This process results in the emission of positron and neutrino. The process results in decrease in atomic number by one unit, and however atomic mass number remains unchanged.
ii) Electron capture: A electron from the low energy level (K-shell or L-shell) falls into the nucleus. Due to this proton is converted into neutron. During this process, neutrino is emitted from the nucleus. As seen in positron emission, the atomic number goes down by one unit, but atomic mass number remains unchanged.

4 0

3 years ago

Excess oxygen gas (O2) reacts with 244g of Iron (Fe) to produce 332 g of Fe2O3. What is the percent yield?

Andru [333]

Answer:

95.15%

Explanation:

To calculate the percent yield, we need the following formula:

$\% yield=\dfrac{actual yield}{theoreticalyield}\times100\%$

Solving for the theoretical yied, you need to predict how much of the product will be produced if we USE up the given.

Our given is 224g of Fe and we to get the theoretical yield, we need to figure out how much product will Fe produce supposing that we use up all the reactant.

First thing we do is get the balance equation of this chemical reaction:

4Fe + 3O₂ → 2Fe₂O₃

We get the ratio between Fe and the the product, Fe₂O₃

$\dfrac{4moles of Fe}{2molesofFe_{2}O_{3}}=\dfrac{2moles of Fe}{1moleofFe_{2}O_{3}}$

This basically means that we need 2 moles of Fe to produce 1 mole of Fe₂O₃. We'll use this later.

Now we let's use our given:

We need to first convert our given to moles. To do this, we need to determine how many grams there are of the reactant for every mole. We need to first get the atomic mass of the elements involved in the substance:

Iron(1)

Fe = 55.845(1) = 55.845g/mole(1)

Then we use this to convert grams to moles

$244g\times\dfrac{1mole}{55.845g}=4.369moles$

This means that there are 4.396moles of Fe in 244g of Fe.

This we will use to see how many moles of product we can produce given the moles of reactant by using the reactant:rproduct ratio.

$4.369moles of Fe\times\dfrac{1moleofFe_{2}O_{3}}{2molesofFe}=2.185 moles of Fe_{2}O_{3}$

So given 4.693 moles of Fe we can produce 2.185 moles of Fe₂O₃

The next step is to get how many grams of product there are given our calculation. We do this again by getting how many grams of Fe₂O₃ there are in 1 mole.

Fe(2) O(3)

Fe₂O₃=55.845(2) + 15.999(3)

= 111.69 + 47.997 =159.687g/mol

We then use this to solve for how many grams of product there are in 2.185 moles.

$2.185moles\times\dfrac{159.687g}{1mole}=348.92g$

This is our theoretical yield 348.92g of Fe₂O₃.

We can finally use our percent yield equation. Our actual yield is given by the probelm, 332g of Fe₂O₃ and we solved for our theoretical yield which is 348.92g of Fe₂O₃. We plug this in our formula and solve.

$\%yield=\dfrac{actual yield}{theoreticalyield}\times100\%$

$\%yield=\dfrac{332gofFe_{2}O_{3}}{348gofFe_{2}O_{3}}\times100\%=95.15\%$

So the answer is 95.15%

3 0

3 years ago