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maksim [4K]
3 years ago
6

3. The alcohol in "gasohol" burns according to the following equation. C2H6O + 3 O2 --------> 2 CO2 + 3 H2O (a) If 25 moles o

f ethyl alcohol burns this way, how many moles of oxygen are needed? (b) If 30 moles of oxygen is consumed by this reaction, how many moles of alcohol are used up? How many moles of carbon dioxide are formed? (c) In one test, 23 moles of carbon dioxide was produced by this reaction. How many moles of oxygen were consumed? (d) In another test, 41 moles of water is collected from this reaction. How many moles of alcohol had been consumed?
Chemistry
1 answer:
Vanyuwa [196]3 years ago
7 0
For all question, all you need to use is the mole-mole ratio. 

a) 25 moles C2H6O (3 moles O2/ 1 mol C2H6O)= 75 moles O2 

b) 30 moles O2 (1 moles C2H6O/ 3 moles O2)= 10 moles C2H6O

c) 23 moles CO2 (3 moles O2/ 2 moles CO2) = 34.5 moles O2

d)  41 moles H2O ( 1 moles C2H6O/ 3 moles H2O= 13.7 moles C2H6O
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Hydrogen gas can be produced from the reaction between methane and water. Write the balanced chemical equation that represents t
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Answer:

Atoms are neither created, nor distroyed, during any chemical reaction ... Chemical reactions are represented on paper by chemical equations. For example, hydrogen gas (H2) can react (burn) with oxygen gas (O2) to form water (H20). ... Write 'balanced' equation by determining coefficients that provide equal numbers of ...

Explanation:

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3 years ago
what volume, in liters, will 6.32 × 10^2 of air occupy if the density of air is 1.29 g/L? Express your answer in scientific nota
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4.90× 10^2 L

I am guessing that the mass of the air is 6.32 × 10^2 <em>g</em>. Then,

Volume = 6.32 × 10^2 g × (1 L/1.29 g) = 4.90× 10^2 L

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3 years ago
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A 1.25 g sample of aluminum is reacted with 3.28 g of copper (II) sulfate. What is the limiting reactant? 2Al(s) + 3CuSO4(aq) →
vova2212 [387]

Answer:

Copper (II) sulfate

Explanation:

Given reaction is

2Al(s) + 3CuSO4(aq) → Al2(SO4)3(aq) + 3Cu(s)

Amount of aluminum = 1·25 g

Amount of copper (II) sulfate = 3·28 g

Atomic weight of Al = 26 g

Molecular weight of CuSO4 ≈ 159·5

Number of moles of Al = 1·25 ÷ 26 = 0·048

Number of moles of CuSO4 = 3·28 ÷ 159·5 = 0·021

From the above balanced chemical equation for every 2 moles of aluminum, 3 moles of copper (ll) sulfate will be required

So for 1 mole of Al, 1·5 moles of copper (ll) sulfate will be required

For 0·048 moles of Al, 1.5 × 0·048 moles of copper (ll) sulfate will be required

∴ Number of moles of copper (ll) sulfate required = 0·072

But we have only 0·021 moles of copper (ll) sulfate

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7 0
3 years ago
A solution contains [Ba2+] = 5.0 × 10−5 M, [Zn2+] = 2.0 × 10−7 M, and [Ag+] = 3.0 × 10−5 M. Sodium oxalate (Na2C2O4) is slowly a
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Answer:

BaC₂O₄, then ZnC₂O₄, then Ag₂C₂O₄  

Explanation:

1. Calculate the equilibrium concentrations of oxalate ion

Let [C₂O₄²⁻] = c

(a) Barium oxalate

                 BaC₂O₄ ⇌   Ba²⁺   + C₂O₄²⁻

E/mol·L⁻¹:                   5.0 × 10⁻⁵     c

Ksp = [Ba²⁺][C₂O₄²⁻] = 5.0 × 10⁻⁵c = 1.5 × 10⁻⁸

c = (1.5 × 10⁻⁸)/(5.0 × 10⁻⁵) = 3.0 × 10⁻⁴ mol·L⁻¹

(b) Zinc oxalate

                ZnC₂O₄ ⇌   Zn²⁺   + C₂O₄²⁻

E/mol·L⁻¹:                 2.0 × 10⁻⁷      c

Ksp = [Zn²⁺][C₂O₄²⁻] = 2.0 × 10⁻⁷c = 1.35 × 10⁻⁹

c = (1.35 × 10⁻⁹)/(2.0 × 10⁻⁷) = 6.8 × 10⁻³ mol·L⁻¹

(c) Silver oxalate

                 Ag₂C₂O₄ ⇌   2Ag⁺   +   C₂O₄²⁻  

E/mol·L⁻¹:                      3.0 × 10⁻⁵       c

Ksp = [Ag⁺]²[C₂O₄²⁻] = (3.0× 10⁻⁵)²c = 9.0 × 10⁻¹⁰c = 1.1 × 10⁻¹¹

c = (1.1 × 10⁻¹¹)/(9.0 × 10⁻¹⁰) = 0.012 mol·L⁻¹

2. Decide the order of precipitation

BaC₂O₄ will precipitate when   c > 3.0 × 10⁻⁴ mol·L⁻¹

ZnC₂O₄ will precipitate when   c > 6.8 × 10⁻³ mol·L⁻¹

Ag₂C₂O₄ will precipitate when c > 0.028       mol·L⁻¹

This happens to be the order of increasing concentration of oxalate ion.

The order of precipitation is

BaC₂O₄, then ZnC₂O₄, then Ag₂C₂O₄

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