Respuesta :
Answer : The value of w and ΔE is, 1.24 kJ and -3170.5 kJ/mol respectively.
Explanation :
Formula used :
[tex]\Delta H=\Delta E+\Delta n_gRT[/tex]
[tex]\Delta H[/tex] = change in enthalpy = -3169.3 kJ/mol = -3169300 J/mol
[tex]\Delta E[/tex] = change in internal energy
[tex]\Delta n_g[/tex] = change in moles
R = gas constant = 8.314 J/mol.K
T = temperature = 298 K
The balanced chemical reaction will be:
[tex]C_2H_6(g)+\frac{7}{2}O_2(g)\rightarrow 2CO_2(g)+3H_2O(g)[/tex]
In this case:
[tex]\Delta n_g[/tex] = change in moles
Change in moles = Number of moles of product side - Number of moles of reactant side
According to the reaction:
Change in moles = [3+2] - [1+ (7/2)]= 0.5 mole
[tex]\Delta H=\Delta E+\Delta n_gRT[/tex]
[tex]-3169300J/mol=\Delta E+(0.5mol)\times (8.314J/mol.K)\times (298K)[/tex]
[tex]\Delta E=-3170.5kJ/mol[/tex]
Now we have to calculate the work done.
[tex]w=p\Delta V=\Delta nRT[/tex]
[tex]w=(0.5mol)\times (8.314J/mol.K)\times (298K)[/tex]
[tex]w=1.24kJ[/tex]
Therefore, the value of w and ΔE is, 1.24 kJ and -3170.5 kJ/mol respectively.
