Question

CH4+2O2➡️ CO2+2H2O,dleta H =-200k cal now delta E for same reaction at 300K is

Answer 1

Answer : The internal energy change is -200 kcal

Explanation :

The given balanced chemical reaction is:

$CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(g)$

Formula used :

$\Delta H=\Delta E+\Delta n_gRT$

or,

$\Delta E=\Delta H-\Delta n_gRT$

where,

$\Delta H$ = change in enthalpy = $-200kcal=-200000cal$

$\Delta U$ = change in internal energy = ?

$\Delta n_g$ = change in moles = 0  (From the reaction)

R = gas constant = 2 cal/K.mol

T = temperature = 300 K

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

$\Delta E=\Delta H-\Delta n_gRT$

$\Delta E=(-200000cal)-(0mol\times 2cal/mol.K\times 300K)$

$\Delta E=-200000cal=-200kcal$

Therefore, the internal energy change is -200 kcal

Answer 2

Answer:

-199.8

Explanation:

1. the above answer is wrong