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larisa [96]
3 years ago
8

How many moles of C2H2 are needed to react completely with 84.0 mol O2?

Chemistry
2 answers:
docker41 [41]3 years ago
5 0

Answer: 33.6 moles

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

Combustion of ethylene is represented by following balanced equation:

2C_2H_2+5O_2\rightarrow 4CO_2+2H_2O

According to stoichiometry:

5 moles of O_2 react completely with = 2 moles of C_2H_2  

Thus 84.0 moles of O_2 react completely with =\frac{2}{5}\times 84.0=33.6 moles of C_2H_2  

Thus 33.6 moles of C_2H_2 are needed to react completely with 84.0 mol O_2

Airida [17]3 years ago
3 0
33.6 moles are needed to completely react with 84.0 moles of O2
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Answer:

0.91 atm is the partial pressure of just hydrogen gas.

Explanation:

Vapor pressure of water , p= 0.0313 atm

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According Dalton's law of partial pressure:

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p_{H_2}=0.94 atm - 0.0313 atm =0.9087 atm \approx 0.91 atm

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3 years ago
When a piece of metal A is placed in a solution containing ions of metal B, metal B plates out on the piece of A.(a) Which metal
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Metal A is being displaced because, through oxidation, it transforms from a solid metal to ions in a solution.

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5 0
2 years ago
Calculate ∆G ◦ r for the decomposition of mercury(II) oxide 2 HgO(s) → 2 Hg(ℓ) + O2(g) ∆H◦ f −90.83 − − (kJ · mol−1 ) ∆S ◦ m 70.
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Answer:

4. +117,1 kJ/mol

Explanation:

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As ΔHf of Hg(l) and ΔHf O₂(g) are 0:

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<u><em /></u>

In the same way ΔSr is:

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ΔGr = 181,66 kJ/mol - 298K*0,216kJ/Kmol

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<em></em>

I hope it helps!

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