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3 years ago

If 0.905 mol Al2O3 is produced in the reaction, what mass of Fe in product's

Chemistry

1 answer:

Marrrta [24]3 years ago

3 0

Answer: Amount of iron produced is 101.36 grams.

Explanation:

For the reaction of aluminium and iron oxide, the equation follows:

$2Al+Fe_2O_3\rightarrow Al_2O_3+2Fe$

By Stoichiometry of the reaction,

When 1 mole of aluminium oxide is produced, then 2 moles of iron is also produced.

So, when 0.905 moles of aluminium oxide is produced, then $\frac{ 2}{1}\times 0.905mol=1.81moles$ of iron is also produced.

Now, to calculate the amount of iron produced, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Molar mass of iron = 56 g/mol

Moles of iron = 1.81 moles

Putting values in above equation, we get:

$1.81mol=\frac{\text{Mass of iron}}{56g/mol}\\\\\text{Mass of iron produced}=101.36g$

Hence, amount of iron produced is 101.36 grams.

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It is possible to obtain the ΔH of a reaction from ΔH's of formation for each compound, thus:

ΔHr = (ΔH products - ΔH reactants)

For the reaction:

CH₄(g) + Cl₂(g) → CCl₄(g) + HCl(g)

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3 years ago

Consider the reaction of NO and CO to form N2 and CO2, according to the balanced equation: 2 NO (g) + 2 CO (g) → N2 (g) + 2 CO2

Gekata [30.6K]

The image is not given in the question, it is attached below:

Answer: The excess reactant is NO, the limiting reactant is CO and the products are shown in the image attached below.

Explanation:

In the given image:

Red spheres represent oxygen atoms, blue spheres represent nitrogen atoms and black spheres represent carbon atoms

The combination of 1 black and 2 red spheres will represent carbon dioxide $(CO_2)$ compound

The combination of 2 blue spheres will represent nitrogen molecule $(N_2)$

The combination of 1 blue and 1 red sphere will represent nitrogen monoxide $(NO)$ compound

The combination of 1 black and 1 red sphere will represent nitrogen monoxide $(NO)$ compound

Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.

Excess reagent is defined as the reagent which is left behind after the completion of the reaction.

We are given:

Given moles of NO = 6 moles

Given moles of CO = 4 moles

For the given chemical equation:

$2NO(g)+2CO(g)\rightarrow N_2(g)+2CO_2(g)$

By stoichiometry of the reaction:

If 2 moles of CO reacts with 2 moles of NO

So, 4 moles of CO will react with = $\frac{2}{2}\times 4=4mol$ of NO

As the given amount of NO is more than the required amount. Thus, it is present in excess and is considered as an excess reagent.

Thus, CO is considered a limiting reagent because it limits the formation of the product.

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3 years ago