High color saturation produces gray tones.
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Related Questions
What is the percentage of nitrogen in N2O
Which the following accurately describes a trade-off of using nuclear energy to produce electricity?A. The energy source is renewable, but the power plant disturbs natural ecosystems by stopping the flow of rivers B. This energy source causes no pollution, but the fuel is a nonrenewable resourceC. Very little fuel is necessary to produce a large amount of energy but the waste materials are harmful to the environment. D. The fuel is inexpensive , but using the energy produces air pollution.
Mixtures have strong chemical bonds true or false ?
Calculate the percentage of iron in iron (III) sulphate
B. similar to other minerals
C. variable depending on where its found
D. influenced by heat and light
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The chemical compositions of minerals is very necessary in order to define or describe a certain mineral. Some minerals can be written in simple chemical formula while others are also written in complicated chemical formulas.
b. 16 g
c. 32 g
d. 1.204 × 1024
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The correct answer is B.
1 mol O2 x 15.999 O2/ 1 mol O2 = 15.999 O2
16 O2 when rounded.
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Now we can solve using the Mole Ratio:
4.54 mol N2 × 2 / 1 × 17.04 g/mol NH3
= 154.72 g
If you need further clarification, feel free to comment.
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The empirical formula is No2 and molecular formula is N2O4
empirical formula calculation
find the moles of each reactant
=% composition/molar mass
molar mass of oxygen=16 g/mol ,while hat of nitrogen= 14 g/mol from periodic table
moles is therefore=
nitrogen= 30.43/14=2.174 moles
oxygen= 69.57/1 6=4.348 moles
find the mole ratio by dividing each moles with smallest number of mole( 2.174)
nitrogen = 2.174/2.174= 1
oxygen = 4.348/2.174=2
The balanced equation for its formation from the element nitrogen and oxygen is as below
N2 +2 O2 → N2O4
therefore the empirical formula= NO2
molecular formula calculation
[NO2] n= 92.02 amu
[(14) + (16x2)]n = 92.02 amu
46n= 92.02
divide both side by 46
n=2
therefore the molecular formula is gotten by multiplying the empirical formula by 2= [NO2]2= N2O4
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This hypothetical process would produce actinium-230.
Explanation
An alpha decay reduces the atomic number of a nucleus by two and its mass number by four.
There are two types of beta decay: beta minus β⁻ and beta plus β⁺.
The mass number of a nucleus stays the same in either process. In β⁻ decay, the atomic number increases by one. An electron e⁻ is produced. In β⁺ decay, the atomic number decreases by one. A positron e⁺ is produced. Positrons are antiparticles of electrons.
β⁻ are more common than β⁺ in decays involving uranium. Assuming that the "beta decay" here refers to β⁻ decay.
Gamma decays do not influence the atomic or mass number of a nucleus.
Uranium has an atomic number of 92. 238 is the mass number of this particular isotope. The hypothetical product would have an atomic number of 92 - 2 ⨯ 2 + 1 = 89. Actinium has atomic number 89. As a result, the product is an isotope of actinium. The mass number of this hypothetical isotope would be 238 - 2 ⨯ 4 = 230. Therefore, actinium-230 is produced.
The overall nuclear reaction would involve five different particles. On the reactant side, there is
- one uranium-238 atom.
On the product side, there are
- one actinium-230 atom,
- two alpha particles (a.k.a. helium-4 nuclei),
- one electron, and
- one gamma particle (a.k.a. photon).
Consider: what would be the products if the nucleus undergoes a β⁺ decay instead?
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? mol H₂O --------- 2.0x10²² molecules
Number of moles = Number of molecules / Avogadro's number
moles = 2.0x10²² * 1 / 6.02x10²³
= 2.0x10²² / 6.02x10²³
= 0.3322 moles
hope this helps!