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Serggg [28]
3 years ago
14

The reaction between iron(II) oxide and carbon monoxide produces iron and carbon dioxide. How many moles of iron can be obtained

when 1.50 mol FeO reacts with an excess of CO ?
FeO+CO⟶Fe+CO2
Chemistry
1 answer:
aleksandrvk [35]3 years ago
5 0

Answer:

1.5 moles of Fe produced.

Explanation:

Given data:

Moles of FeO react = 1.50 mol

Moles of iron produced = ?

Solution:

Chemical equation:

FeO + CO       →       Fe + CO₂

Now we will compare the moles of ironoxide with iron.

                           FeO          :           Fe

                              1             :             1

                             1.5           :           1.5

Thus from 1.5 moles of FeO 1.5 moles of Fe are produced.                                    

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Answer:

25 mm is smaller.

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3 years ago
What is the volume of a 0.1 M HCl solution containing 1.46 moles of HCI?
Natasha_Volkova [10]
N = cv
1.46 = 0.1 x v
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5 0
3 years ago
An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO2 f
ladessa [460]

Answer: Mass of Fe_2O_3 required to form 930 kg of iron is 1328 kg

Explanation:

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

For iron:

Given mass of iron = 930 kg = 930000 g  (1kg=1000g)

Molar mass of iron = 56 g/mol

Putting values in equation 1, we get:

\text{Moles of iron}=\frac{930000g}{56g/mol}=16607mol

The chemical equation for the  production of iron  follows:

Fe_2O_3+3CO\rightarrow 2Fe+3CO_2

By Stoichiometry of the reaction:

2 moles of iron are  produced by =  1 mole of Fe_2O_3

So, 16607 moles of iron will be produced by = \frac{1}{2}\times 16607=8303moles of Fe_2O_3

Now, calculating the mass of Fe_2O_3 from equation 1, we get:

Mass of Fe_2O_3 = moles\times {\text {molar mass}}=8303\times 160=1328480g=1328kg

Thus mass of Fe_2O_3 required to form 930 kg of iron is 1328 kg

6 0
3 years ago
using the equation, c5h12 8o2 arrow 5co2 6h2o, if 108 g of water are produced, how many grams of oxygen were consumed?
vfiekz [6]
Molar mass:

H₂O = 18.0 g/mol

O₂ = 32.0 g/mol

C₅H₁₂ + 8 O₂ -> 5 CO₂ + 6 H₂<span>O
</span>
8 x (32 g )<span> ------------ 6 x (18 g )</span>
mass O₂ ------------ 108 g H₂O

mass O₂ = 108 x 8 x 32 / 6 x 18

mass O₂ = 27648 / 108

mass O₂ =<span> 256 g</span>

<span>hope this helps!</span>
8 0
3 years ago
As Mia mixed two substances in a test tube, she noticed that the test tube became warm. She also noticed gas coming from the tes
ss7ja [257]

Answer:

a new substance was forming

Explanation:

8 0
3 years ago
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