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Exactly 56 grams of iron is mixed with 156 grams of oxygen. The elements are heated and they react. What best describes which re

Mars2501 [29]

Answer:

Explanation:

The chemical expression for the reaction between iron and oxygen is:

4Fe(s) + 3O₂ (g) $\to$ 2Fe₂O₃ (s)

The number of moles of Fe = mass of Fe/ molecular mass of Fe

The number of moles of Fe = 56 g/ 55.845 g/mol

The number of moles of Fe = 1.002 moles of Fe

The number of moles of oxygen = mass of oxygen/ molecular mass of oxygen

The number of moles of oxygen = 156 g /32 g/mol

The number of moles of oxygen = 4.875 moles of oxygen

Assume that Fe is the limiting reactant, the number of Fe₂O₃ can be calculated as:

moles of Fe₂O₃ = 1.002 mole of Fe × 2 moles of Fe₂O₃/ 4 moles of Fe

moles of Fe₂O₃ = 0.501 mole of Fe₂O₃

Assume that O₂ is the limiting factor, the number of Fe₂O₃ is:

moles of Fe₂O₃ = 4.875 moles of O₂ × 2 moles of Fe₂O₃/ 3 moles of O₂

moles of Fe₂O₃ = 3.25 mole of Fe₂O₃

Thus, after the reaction is complete, Fe and O₂ contain different moles of Fe₂O₃. Only Fe gets consumed in the reaction and it is the limiting factor.

8 0

1 year ago

Which statement explains why NaBr is classified as a compound?

charle [14.2K]

Answer:1

Explanation:i know cuz I got it right

5 0

2 years ago

Diatomic hydrogen gas and diatomic nitrogen gas react spontaneously to form a gaseous product. Give the balanced chemical equati

alex41 [277]

Answer : $NH_{3}$

Explanation : When diatomic hydrogen gas and diatomic nitrogen gas reacts spontaneously it forms ammonia gas as the product.

we will have the following reactions; As all the reactants and products are in the gaseous state the subscript (g) is given to the molecules.

$H_{2}_{(g)} + N_{2}_{(g)} ----> NH_{3}_{(g)}$

But this is not a balanced equation, as on the right side of reactants we have 2 hydrogen atoms and 2 nitrogen atoms which gives the product which has one nitrogen and three hydrogen in the compound state.

So, balancing the equation, we get,

$3H_{2}_{(g)} + N_{2}_{(g)} ----> 2NH_{3}_{(g)}$

We multiplied 2 with the diatomic hydrogen molecule which resulted in production of 2 moles of ammonia as the product.

So, the complete balanced equation is;

$3H_{2}_{(g)} + N_{2}_{(g)} ----> 2NH_{3}_{(g)}$

5 0

2 years ago

Read 2 more answers

If 4.59 g of potassium reacts with 3.6 g of sulfur according to the following reaction, how many grams of potassium sulfide can

EleoNora [17]

First convert the amount of grams you have of each substance to moles. Find your limiting reactant by calculating how many grams are needed to complete this reaction. If done correctly, you would see that we need .226 moles of Potassium to complete this reaction. However, we only have .118 moles of Potassium, so K must be our limiting reactant. Then use the moles of K to find out how many moles of K^2S are made. Then convert the amount of moles of K^2S to grams and you should get 10.3 g K^2S

8 0

2 years ago

Anne prepares a solution of copper nitrate with a concentration of 30 g/dm³. What mass of copper nitrate did she add to 100cm³ o

strojnjashka [21]

Answer:

3 g

Explanation:

Concentration of copper nitrate needed = 30 g/dm³

Volume of water = 100 cm³ = 0·1 dm³

( ∵ 1 dm³ = 1000 cm³)

Let the mass of copper nitrate that should be added to 100 cm³ water be m g

m ÷ 0·1 = 30

∴ m = 3 g

∴ Mass of copper nitrate that should be added to 100 cm³ of water = 3 g

7 0

2 years ago