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Virty [35]
2 years ago
15

I need solutions, thank you very much

Chemistry
1 answer:
drek231 [11]2 years ago
7 0

The mass of carbon required to produce iron from 5 67 g iron (iii) oxide is 9.0 g.

<h3>What is the mass of carbon required to produce iron from iron (iii) oxide?</h3>

The mass of carbon required to produce iron from iron (iii) oxide is determined from the equation of the reaction.

From the given equation of reaction, 3 moles of carbon produces 4 moles of iron.

  • Moles of a substance = mass/molar mass

Molar mass of iron = 56.0 g

molar mass of carbon = 12.0 g

Moles of iron in 5.67 g of iron = 5.67/56 = 0.1 moles

Moles of carbon required = 3/4 × 0.1 = 0.75 moles

Mass of carbon = 0.75 × 12 = 9.0 g

Therefore, the mass of carbon required to produce iron from 5 67 g iron (iii) oxide is 9.0 g.

Learn more about mass and moles at: brainly.com/question/13860160

#SPJ1

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Answer :  The value of second ionization energy of Ca is 1010 kJ.

Explanation :  

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Ca(s)+\frac{1}{2}O_2(g)\overset{\Delta H_f}\rightarrow CaO(s)

\Delta H_f^o = enthalpy of formation of calcium oxide = -635 kJ

The steps involved in the born-Haber cycle for the formation of CaO:

(1) Conversion of solid calcium into gaseous calcium atoms.

Ca(s)\overset{\Delta H_s}\rightarrow Ca(g)

\Delta H_s = sublimation energy of calcium = 193 kJ

(2) Conversion of gaseous calcium atoms into gaseous calcium ions.

Ca(g)\overset{\Delta H_I_1}\rightarrow Ca^{+1}(g)

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(3) Conversion of gaseous calcium ion into gaseous calcium ions.

Ca^{+1}(g)\overset{\Delta H_I_2}\rightarrow Ca^{+2}(g)

\Delta H_I_2 = second ionization energy of calcium = ?

(4) Conversion of molecular gaseous oxygen into gaseous oxygen atoms.

O_2(g)\overset{\Delta H_D}\rightarrow OI(g)

\frac{1}{2}O_2(g)\overset{\Delta H_D}\rightarrow O(g)

\Delta H_D = dissociation energy of oxygen = \frac{498}{2}=249kJ

(5) Conversion of gaseous oxygen atoms into gaseous oxygen ions.

O(g)\overset{\Delta H_E_1}\rightarrow O^-(g)

\Delta H_E_1 = first electron affinity energy of oxygen = -141 kJ

(6) Conversion of gaseous oxygen ion into gaseous oxygen ions.

O^-(g)\overset{\Delta H_E_2}\rightarrow O^{2-}(g)

\Delta H_E_2 = second electron affinity energy of oxygen = 878 kJ

(7) Conversion of gaseous cations and gaseous anion into solid calcium oxide.

Ca^{2+}(g)+O^{2-}(g)\overset{\Delta H_L}\rightarrow CaO(s)

\Delta H_L = lattice energy of calcium oxide = -3414 kJ

To calculate the overall energy from the born-Haber cycle, the equation used will be:

\Delta H_f^o=\Delta H_s+\Delta H_I_1+\Delta H_I_2+\Delta H_D+\Delta H_E_1+\Delta H_E_2+\Delta H_L

Now put all the given values in this equation, we get:

-635kJ=193kJ+590kJ+\Delta H_I_2+249kJ+(-141kJ)+878kJ+(-3414kJ)

\Delta H_I_2=1010kJ

Therefore, the value of second ionization energy of Ca is 1010 kJ.

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<u>Answer:</u>

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For example 5 Ca_1 Cl_2 contains

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