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3 years ago

Consider the following data:

Chemistry

2 answers:

VikaD [51]3 years ago

8 0

∆H ° rxn =-2855.56 kJ

<h3>Further explanation</h3>

Given

ΔHf CO₂ = -393.5 kJ/mol

ΔHf H₂O = -241.82 kJ/mol

ΔHf C₂H₆ = - 84.68 kJ/mol

Reaction

2C2H6(g) + 7O2(g) -> 4CO2(g) + 6H2O(g)

Required

ΔHrxn=

Solution

<em>∆H ° rxn = ∑n ∆Hf ° (product) - ∑n ∆Hf ° (reactants) </em>

∆H ° rxn = (4.-393.5+6.-241.82)-(2.-84.68)

∆H ° rxn = (-1574-1450.92)-(-169.36)

∆H ° rxn =-3024.92+169.36

∆H ° rxn =-2855.56 kJ

Dafna1 [17]3 years ago

5 0

Answer:

-2856 kJ

Explanation:

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Answer: 1.57 M

Explanation:

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If a muriatic acid solution has a pH of 2.50, what is the hydronium ion concentration (hydronium ion concentration is also the m

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Answer:

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Explanation:

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When you know the pH value you can find hydronium concentration using the antilogaritm function:

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The vaporization of 1 mole of liquid water (system) at 100.9 C, 1.00 atm, is endothermic.

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Answer:

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b) The water's change in internal energy is -122.1973 kJ

Explanation:

Given data:

1 mol of liquid water

T₁ = temperature = 100.9°C

P = pressure = 1 atm

Endothermic reaction

T₂ = temperature = 100°C

1 mol of water vapor

VL = volume of liquid water = 18.8 mL = 0.0188 L

VG = volume of water vapor = 30.62 L

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b) Calculate the water's change in internal energy, ΔU = ?

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$Q_{1} =3.25*(-40.7)=-132.275kJ$

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The change in internal energy:

$delt(U)=W+Q_{1} =10.0777-132.275=-122.1973kJ$

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