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Aliun [14]
3 years ago
9

Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g)ΔH = −184.6 kJ / mol If 2.00 moles of H2 re

act with 2.00 moles of Cl2 to form HCl, what is ΔU (in kJ) for this reaction at 1.0 atm and 25°C? Assume the reaction goes to completion.
Chemistry
1 answer:
serious [3.7K]3 years ago
6 0

Answer : The value of \Delta E of the reaction is, -369.2 KJ

Explanation :

Formula used :

\Delta E=\Delta H-\Delta n_g\times RT

where,

\Delta E = internal energy of the reaction = ?

\Delta H = enthalpy of the reaction = -184.6 KJ/mole = -184600 J/mole

The balanced chemical reaction is,

H_2(g)+Cl_2(g)\rightarrow 2HCl(g)

when the moles of H_2\text{ and }Cl_2 are 2 moles then the reaction will be,

2H_2(g)+2Cl_2(g)\rightarrow 4HCl(g)

From the given balanced chemical reaction we conclude that,

\Delta n_g = change in the moles of the reaction = Moles of product - Moles of reactant = 4 - 4 = 0 mole

R = gas constant = 8.314 J/mole.K

T = temperature = 25^oC=273+25=298K

Now put all the given values in the above formula, we get:

\Delta E=(-184600J/mole\times 2mole)-(0mole\times 8.314J/mole.K\times 298K)

\Delta E=-369200J

\Delta E=-369.2KJ

Therefore, the value of \Delta E of the reaction is, -369.2 KJ

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