Which of the following is an example of a chemical reaction?
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Answer:
where is the option I can't see plz give the option first the I try to give answer
Related Questions
Which of the following chemical equations is balanced?2 Al + 2 CuO ----> A1,0, + 2 CuFe, 0, + 3C --> 2Fe + 3 CO,2 SO, + 02 S0, + 0, ---> 2 SO,2 Ag,0 ----> 2 Ag + O2> 02
The molar mass of NH3 is 17.03 g/mol. The molar mass of H2 is 2.0158 g/mol. In a particular reaction, 0.575 g of NH3 forms. What is the mass, in grams, of H2 that must have reacted, to the correct number of significant figures?
How many moles are in 68.5 liters of oxygen gas at STP?
If a substance is ionic, then it likely will what?
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2H2 + O2 ⇒⇒ 2H2O
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H has 1 proton
He has 2 protons
Li has 3 protons
Be has 4 protons and so on
Each proton has a charge of +1. The other particle present in the nucleus - the neutron - has zero electrical charge and thus irrelevant when computing the charge of a nucleus. It is easy to deduce that the nucleus charge equals the number of protons (which in turn equals the atomic number). So the nucleus charges are:
for H it's+1
for He it's +2
for Li it's +3
for Be it's +4 and so on
Atom is an electroneutral particle by definition. It means it's summed charge must be 0. Since we've looked at everything within the nucleus (the protons and the neutrons) it's time we turn our gaze to the space around it, which is full of orbiting electrons. Each electron has a charge of -1. To make up for the positive charge in the nucleus you have to fill the space aroung the nucleus with negative electrons.Thanks to the elementary nature of both proton and electron charge, you simply have to take the same number of electrons as that of protons! Like this:
H has 1 proton and 1 electron
He has 2 protons and 2 electrons
Li has 3 protons and 3 electrons
Be has 4 protons and 4 electrons and so on
Fe has atomic number 26. It means that Fe has 26 protons and 26 electrons. If it's a neutral atom
You typed 3. Is it accidental? If so, then the answer is above. If not, then you could be trying to type 56Fe +3, which means an ionic iron with charge +3. Charges are formed when you have too many or too few electrons to counter-balance the prositive charge of the nucleus. Charge +3 means you're 3 electrons short to negate the nucleus positive charge.
In other words, Fe+3 has 26 protons and 23 electrons.
Final answer:
56Fe3+ is an iron ion with a charge of +3, meaning it has 23 electrons after 3 electrons are lost from the uncharged state. It loses the 4s2 electrons first, then one of the 3d electrons.
Explanation:
The student's question refers to 56Fe3+. 56Fe3+ is an iron ion with a charge of +3, which means it has lost three electrons. Understanding the Electron configuration is vital here. Normally, iron (Fe) has 26 electrons as its atomic number is 26. Each electron has a negative charge. But in 56Fe3+, 3 electrons are lost; hence, it will have 23 electrons.
Let's look further into this. The electron configuration of an uncharged Fe atom is 1s²2s²2p6 3s²3p6 4s²3d6. The iron atom loses the 4s2 electrons first (becoming Fe2+), then one of the 3d electrons (becoming Fe3+ or 56Fe3+ as indicated in the question).
Learn more about Electrons in Iron Ion here:
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***a dense substance that is hard and incompressible ***
a high-energy state of matter made up of a swirling, ionized gas
a loose association of particles moving past one another
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a dense substance that is hard and incompressible
Halite crystal is growing and can attach very quickly and eventually form a smooth, stable faces where new atoms can easily attach themselves.
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Answer:
The % yield of the reaction is 73.8 %
Explanation:
To solve this, we list out the given variables thus
Mass of aluminium in the experiment = 2.5 g
mass of oxygen gas in the experiment = 2.5 g
Molar mass of aluminium = 26.98 g/mol
molar mass of oxygen O₂ = 32 g/mol
The reaction between aluminium and gaseous oxygen can be written as follows
4Al + 3O₂ → 2Al₂O₃
Thus four moles of aluminium forms two moles of aluminium oxide
Thus (2.5 g)÷(26.98 g/mol) = 0.093 mole of aluminium and
(2.5 g)÷(32 g/mol) = 0.078125 moles of oxygen
However four moles of aluminium react with three moles of oxygen gas O₂
1 mole of aluminum will react with 3/4 moles of oxygen O₂ and 0.093 mole of aluminium will react with 0.093*3/4 moles of O₂ = 0.0695 moles of Oxygen hence aluminium is the limiting reagent and we have
1 mole of oxygen will react with 4/3 mole of aluminium
∴ 0.078125 mole of oxygen will react with 0.104 moles of aluminium
Therefore 0.093 mole of aluminium will react with O₂ to produce 2/4×0.093 or 0.0465 moles of 2Al₂O₃
The molar mass of 2Al₂O₃ = 101.96 g/mol
Hence the mass of 0.0465 moles = number of moles × (molar mass)
= 0.0465 moles × 101.96 g/mol = 4.74 g
The of aluminium oxide Al₂O₃ is 4.74 g, but the actual yield = 3.5 g
Therefore the Percentage yield = ×100 =
× 100 = 73.8 % yield