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krok68 [10]
3 years ago
5

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2 NO ( g

) + O 2 ( g ) − ⇀ ↽ − 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ G ° = − 69.0 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are P NO = 0.450 atm , P O 2 = 0.100 atm , and P NO 2 = 0.650 atm ?
Chemistry
1 answer:
enyata [817]3 years ago
5 0

Answer:

ΔG = -61.5 kJ/mol (<u>Spontaneous process</u>)

Explanation:

2 NO (g)  +  O₂  (g)   ⇄  2NO₂ (g)

Let's apply the thermodynamic formula to calculate the ΔG

ΔG = ΔG° + R .T . lnQ

We don't know if the gases are at equilibrium, that's why we apply Q (reaction quotient)

ΔG = - 69 kJ/mol + 8.31x10⁻³ kJ/K.mol . 298K . ln Q

How can we know Q? By the partial pressures (Qp)

P NO = 0.450atm

PO₂ = 0.1 atm

PNO₂ = 0.650 atm

Qp = [NO₂]² / [NO]² . [O₂]

Qp = 0.650² / 0.450² . 0.1 = 20.86

ΔG = - 69 kJ/mol + 8.31x10⁻³ kJ/K.mol . 298K . ln 20.86

ΔG = -61.5 kJ/mol (<u>Spontaneous process</u>)

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Calculate the mass in grams of carbon dioxide produced from 11.2 g of octane (C8H18) in the reaction above.
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Unknown:

Mass of carbon dioxide produced  = ?

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From the balanced reaction equation;

         2 mole of octane produced 16 moles of carbon dioxide

From the given specie, let us find the number of moles;

    Number of moles  = \frac{mass}{molar mass}  

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Number of moles of octane  = \frac{11.2}{114}   = 0.098mole

   

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8 0
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NH4Cl + AgNO3 → AgCl + NH4NO3
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pychu [463]
The solution for this problem is:
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matrenka [14]

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