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cestrela7 [59]
3 years ago
6

Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe2O3 are formed when 1.47 g of Fe reacts

completely with oxygen?
Chemistry
1 answer:
ozzi3 years ago
8 0

Answer:

2.10 g

Explanation:

Write the unbalanced reaction:

Fe + O₂ → Fe₂O₃

Balance it:

4Fe + 3O₂ → 2Fe₂O₃

Now use stoichiometry.  Convert mass of Fe to moles of Fe:

1.47 g Fe × (1 mol Fe / 55.8 g Fe) = 0.0263 mol Fe

Convert moles of Fe to moles of Fe₂O₃:

0.0263 mol Fe × (2 mol Fe₂O₃ / 4 mol Fe) = 0.0132 mol Fe₂O₃

Finally, convert moles of Fe₂O₃ to mass of Fe₂O₃:

0.0132 mol Fe₂O₃ × (159.7 g Fe₂O₃ / mol Fe₂O₃) = 2.10 g Fe₂O₃

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Answer: amoebae !

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Design a synthesis of acetophenone from benzene or toluene. 1275q Part 1 out of 5 Choose the best option for the nucleophile pre
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Answer:

A Fridiel craft catalyst will convert benzene to acetophenone.

Permanganate catalyst can be used to convert toluene to acetophenone.

Explanation:

Benzene can be reduced to acetophenone by the addition of anhydrous aluminium chloride, AlCl₃

The mechanism is as follows:

Benzene + Acetyl choloride → acetophenone

To convert toluene to acetophenone, the following steps are necessary:

  • Oxidation of Toluene to Benzoic acid.

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5 0
3 years ago
5.(06.04B MC)
NARA [144]

Answer:

Explanation:

1. The reaction will proceed backward, shifting the equilibrium position to the left.

2. The reaction will proceed forward, shifting the equilibrium position to the right.

3. Either add more of the products ( H2O or Cl2) or remove the reactant (HCl or O2)

7 0
2 years ago
A hydrogen fuel cell is an electrochemical reactor in which oxygen and hydrogen gas are reacted to produce energy. Rather than c
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6 0
3 years ago
Carbon dioxide, when it is at -145 degreesC has a density of 2.54 g/L. What is the pressure in torr??
Black_prince [1.1K]

Answer: The pressure in torr is 461 torr

Explanation:

To calculate the relation of density and molar mass of a compound, we use the ideal gas equation:

PV=nRT

P = pressure

V = Volume

n = number of moles

R = gas constant = 0.0821 Latm/Kmol

T = temperature =-145^0C=(273-145)K=128K

Number of moles (n) can be written as:

n=\frac{m}{M}

where, m = given mass

M = molar mass  = 44 g/mol

PV=\frac{m}{M}RT\\\\PM=\frac{m}{V}RT

where,

\frac{m}{V}=d

where d = density = 2.54 g/L

The relation becomes:

PM=dRT  

P=\frac{dRT}{M}

P=\frac{2.54\times 0.0821\times 128}{44}=0.607atm

P=461torr    (760torr=1atm)

Thus the pressure in torr is 461 torr

5 0
3 years ago
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