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3 years ago

Identify the reactants and the products in this chemical equation. 2Fe2O3 + 3C → 4Fe + 3CO2

Chemistry

1 answer:

aivan3 [116]3 years ago

7 0

Answer:

Fe₂O₃ and C are reactants

Fe and CO₂ are products

Explanation:

Reactants:

Chemical species that are present on left side of chemical reaction equation are called reactants.

Product:

Chemical species that are present on right side of chemical reaction equation are called product.

Chemical equation:

2Fe₂O₃ + 3C → 4Fe + 3CO₂

In this reaction 2 mole of iron oxide is react with three moles of carbon and produced four moles of iron and three moles of carbon dioxide. There are equal numbers of atoms of all elements present on both side of chemical reaction so this reaction follow the law of conservation of mass.

Law of conservation of mass:

According to the law of conservation mass, mass can neither be created nor destroyed in a chemical equation.

Explanation:

This law was given by french chemist Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.

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A sample of propane (C3H8) is placed in a closed vessel together with an amount of O2 that is 3 times the amount needed to compl

Aneli [31]

Answer:

final mole fraction of O₂ = 58.84% , CO₂ = 17.64% , H₂O = 23.52% .

final partial pressure of O₂ = 2.942 atm , CO₂ = 0.882 atm , H₂O = 1.176 atm .

Explanation:

Assuming that propane is present as a gas , and also that the combustion is complete:

C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O

then taking as a reference propane sample= 1 mol , then

initial moles of O₂ = 3* 5 moles = 15 moles

final moles of O₂= 3* 5 moles - 5 moles = 10 moles

final moles of CO₂ = 3 moles

final moles of H₂O = 4 moles

total number of moles = 10 + 3 + 4 = 17 moles

final mole fraction of O₂ = 10/17 = 0.5884 = 58.84%

final mole fraction of CO₂ = 3/17 = 0.1764 = 17.64%

final mole fraction of H₂O = 4/17 = 0.2352 = 23.52%

From Dalton's law for ideal gases , the partial pressure p=P*x then

final partial pressure of O₂ = 5 atm * 10/17 = 2.942 atm

final partial pressure of CO₂ = 5 atm * 3/17 = 0.882 atm

final partial pressure of H₂O = 5 atm * 1/17 = 1.176 atm

4 0

3 years ago

Read 2 more answers

How many moles are present in 356.4 g of NiBr3

lozanna [386]

1.194 mol

(remember to use sig figs!)

8 0

3 years ago

1: A man standing on the South Pole of the Earth drops a ball. Mike thinks that the ball will move away from the Earth and Maria

m_a_m_a [10]

Answer:

Maria

Explanation:

The gravity of the earth is so strong it causes the magnetic pull of anything and everything, this causing the ball to be dropped and pulled towards earth

5 0

2 years ago

How many significant figures does 0.005505 have

Viktor [21]

Answer:

it has six significant figures

8 0

3 years ago

A student reacts 20.0 grams of sodium hydroxide with excess hydrochloric acid, and obtains a

Tcecarenko [31]

Answer:

Percent yield of NaCl = 87.75 %

Explanation:

Data given

mass of sodium = 20.0 g

actual yield of Sodium chloride = 25 g

percent yield of sodium chloride = ?

Reaction Given:

NaOH + HCI --> NaCl + H₂O

Solution:

First we have to find theoretical yield.

So, Look at the reaction

NaOH + HCI ---------> NaCl + H₂O

1 mol 1 mol

As 1 mole of NaOH give 1 mole of NaCl

Convert moles to mass

molar mass of NaOH = 23 + 16 + 1 = 40 g/mol

molar mass of NaCl = 23 +35.5 = 58.5 g/mol

Now

NaOH + HCI ---------> NaCl + H₂O

1 mol (40 g/mol) 1 mol (58.5 g/mol)

40 g 58.5 g

So 40 g of NaOH gives 58.5 g of NaCl so how many grams of Sodium chloride will be produced by 20 g of NaOH.

Apply Unity Formula

40 g of NaOH ≅ 58.5 g of NaCl

20 g of NaOH ≅ X g of NaCl

Do cross multiply

g of NaCl = 58.5 g x 20 g / 40 g

g of NaCl = 29.25 g

So the Theoretical yield of NaCl = 29.25 g

Now Find the percent yield of NaCl

Formula Used

percent yield = actual yield /theoretical yield x 100 %

Put value in the above formula

percent yield = 25 / 29.2 x 100 %

percent yield = 87.75 %

percent yield of NaCl = 87.75 %

7 0

4 years ago