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3 years ago

How many moles of Fe3O4 are required to supply enough iron to prepare 0.472mol Fe2O3 ?

Chemistry

1 answer:

kogti [31]3 years ago

5 0

The combustion reaction for Fe₃O₄ in an oxygen molecule O₂ yields Fe₂O₃.

The number of moles of Fe₃O₄ required to prepare 0.472 moles of Fe₂O₃ is:

0.315 moles

The reaction equation is:

$\mathbf{4Fe_3O_4+O_2 \to 6Fe_2O_3}$

From the above reaction;

4 moles of Fe₃O₄ react with oxygen to produce 6 moles Fe₂O₃.

i.e.

Fe₃O₄ : Fe₂O₃ = 4 : 6

Fe₃O₄ : Fe₂O₃ = 2 : 3

$\mathbf{ = \dfrac{2}{3}\times 0.472}$

= 0.315 moles

Therefore, we can conclude that 0.472 moles of Fe₂O₃ are prepared from 0.315 moles of Fe₃O₄.

Learn more about chemical reactions here:

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For a reaction at equilibrium, which change can increase the rates of the forward and reverse reactions?a decrease in the concen

Monica [59]

Question requires a change resulting in an increase in both forward and reverse reactions. Now lets discuss options one by one and see there impact on rate of reactions.

1) A decrease in the concentration of the reactants:
When concentration of reactant is decreased it will shift the equilibrium in Backward direction, so resulting in increasing the backward reaction and decreasing the forward direction. Hence, this option is incorrect.

2) A decrease in the surface area of the products:
Greater the surface Area greater is the chances of collision and greater will be the rate of reaction. As the surface area of products is decreased it will not favor the backward reaction. Hence again this statement is incorrect according to given statement.

3) An increase in the temperature of the system:
An increase in temperature will shift the reaction in endothermic side. Hence, if the reaction is endothermic, an increase in temperature will increase the rate of forward direction or if the reaction is exothermic it will increase the rate of reverse direction. Hence, this option is correct according to given statement.

4) An increase in the activation energy of the forward reaction:
An increase in Activation energy will decrease the rate of reaction, either it is forward or reverse. So this is incorrect.

Result:
Hence, the correct answer is,"An increase in the temperature of the system".

7 0

3 years ago

Consider the following equilibrium reaction having gaseous reactants and products. 4HCl + O2 ⇌ 2H2O + Cl2 Which of the following

gulaghasi [49]

<h3>Answer;</h3>

B.The rate of forward reaction increases.

<h3>Explanation;</h3>

Le Chatelier's principle states that changing a factor such as concentration, temperature, or pressure of a reaction at equilibrium will cause the reaction to shift in the direction that counteracts the effect of that change.
Therefore, when reactants are added to a reaction at equilibrium shift when more reactants are added then the reaction shifts to the right to make more products.

3 0

3 years ago

What is the volume of 300. g of mercury vapor at 822K and 0.900 atm?

Dominik [7]

Answer:

112.2L

Explanation:

Volume (V) = 300g

Temperature (T) = 822K

Pressure (P) = 0.9atm

using the ideal gas equation;

$PV = nRT\\\\ V = \frac{nRT}{P}$

Molar gas constant (R) = $0.0821L.atm/mol.K$

Mole (n) = $\frac{Mass (m)}{Molar mass (M)}$ Molar mass of Mercury = 200.59g/mol

$n = \frac{300g}{200.59 g/mol} \\$

= 1.496mol

Now, the volume can be calculated;

V = $\frac{1.496mol* 0.0821L.atm/mol.K*822K}{0.9atm}$

∴Volume of mercury = $112.2L$

8 0

2 years ago

A 200.0mL closed flask contains 2.000mol of carbon monoxide gas and 2.000mol of oxygen gas at the temperature of 300.0K. How man

max2010maxim [7]

Answer:

There will react 0.400 moles of oxygen.

Explanation:

Step 1: Data given

Volume of the closed flask = 200.00 mL = 0.2 L

Number of moles of CO = 2.000 mol

Number of moles of O2 = 2.000 mol

Temperature = 300.0 K

Pressure decreases with 10%

Step 2: The balanced equation

2CO(g)+O2(g)⟶2CO2(g)

Step 3: Calculate the initial pressure of the flask before the reaction

P = nRT/V

⇒ with n = the number of moles (2.000 moles CO + 2.000 moles O2 = 4.000 moles)

⇒ R is gas constant (0.08206 atm*L/mol*K)

⇒T = the temperature = 300.0K

⇒ V = the volume = 200.0 mL = 0.2 L

P = (4 * 0.08206*300)/0.2

P = 492.36 atm

Step 4: When the pressure is 10 % decreased:

The final pressure = 492.36 - 49.236 = 443.124 atm

Step 5: Calculate the number of moles

n = PV/RT

⇒ with n = the number of moles

⇒ with P = the pressure = 443.124 atm

⇒ V = the volume = 200.0 mL = 0.2 L

⇒ R is gas constant (0.08206 atm*L/mol*K)

⇒T = the temperature = 300.0K

n =(443.124*0.2)/(0.08206*300)

n = 3.6 moles = total number of moles

Step 6: Calculate number of moles

For the reaction :2CO(g) + O₂(g) ⟶ 2CO₂(g)

For each mole of O2 we have 2 moles of CO, to produce 2 moles of CO2

Moles CO = (2 -2X) moles

Moles O2 = (2-X) moles

Moles CO2 = 2X

The total number of moles (4 -X)= 3.6 moles

Where X are moles that react

X = 0.400 moles

There will react 0.400 moles of oxygen.

6 0

3 years ago

What volume of a 0.424 M CO2 solution are needed to produce 63.58 mL of 0.731 M solution of K2CO3?

cricket20 [7]

Answer:

Socratic app

Explanation:

it will help you

6 0

3 years ago