Question

At constant temperature for the reaction C3H8(g) + 5O2(g) ➡ 3CO2(g) + 4H2O(L) , ΔH - ΔE is :-

1)+RT
2)-3RT
3)+3RT
4)-RT ​

Answer 1

At constant temperature for the reaction , $C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(l)$, $\Delta H-\Delta E=-3\times RT$

Explanation:

The reaction given is:

$C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(l)$

$\Delta H=\Delta E+\Delta n_g\times RT$

where,

$\Delta H$ =  enthalpy of the reaction

$\Delta E$= internal energy of the reaction

$\Delta n_g$ = change in the moles of the reaction = Moles of product - Moles of reactant = 3 - 6 = -3

R = gas constant

T = temperature

Putting in the values we get:

$\Delta H=\Delta E+(-3)\times RT$

$\Delta H-\Delta E=(-3)\times RT$

Learn More about internal energy change and enthalpy change

https://brainly.in/question/12558547

https://brainly.in/question/12433624