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never [62]
3 years ago
13

An elimination reaction can best be described as a reaction in which an elimination reaction can best be described as a reaction

in which a hydrocarbon reacts with oxygen to produce co2, h2o, and energy. two reactants combine to form one new product with no extra atoms. a single reactant splits into two products. two reactants exchange atoms to give two new products. a single reactant undergoes reorganization of its chemical bonds, producing an isomer of the reactant.
Chemistry
1 answer:
tresset_1 [31]3 years ago
4 0
So I’m not 100% sure what you’re asking but I’m going to give it a go. The elimination reaction is a term used in organic chemistry that describes a type of reactions. The name kinda tells you what’s going to happen. Something is going to be removed/eliminated from initial reactant/substrate and as a result, an alkene (double bond containing compound) will form.

In elimination reactions a hydrogen atom is first removed (as a H+) from the beta carbon. As a result, the left behind electrons create a pi bond between the beta carbon and the neighboring alpha carbon. This promotes the electronegative atom, on the alpha carbon, to leaves the substrate taking both electrons from the shared sigma bond with the alpha carbon.
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How many liters of space are in 4.00x10^22 of O2 occupy at STP
irinina [24]

Answer:

V O2 = 1.623 L

Explanation:

  • 1 mol ≡ 6.022 E23 molecules

∴ molecules O2 = 4.00 E22 molecules

⇒ moles O2 = (4.00 E22 molecules O2)×(mol O2/6.022 E23 molecules)

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assuming ideal gas:

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5 0
3 years ago
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How many grams of Ni are formed from 55.3 g of Ni2O3?<br><br> 2Ni2O3(s)⟶4Ni(s)+3O2(g)
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Answer:

39.2 g

Explanation:

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First we <u>convert 55.3 grams of Ni₂O₃ into moles of Ni₂O₃</u>, using its<em> molar mass</em>:

  • 55.3 g ÷ 165.39 g/mol = 0.334 mol Ni₂O₃

Then we <u>convert 0.334 moles of Ni₂O₃ into moles of Ni</u>, using the <em>stoichiometric coefficients of the balanced reaction</em>:

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Finally we <u>calculate how much do 0.668 Ni moles weigh</u>, using the<em> molar mass of Ni </em>:

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7 0
3 years ago
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