Question

The heat of combustion of CH4 (g) at constant volume is measured in a bomb calorimeter at 298-2 K and
found to be - 885389 J/mol. Find the value of enthalpy change.​

Answer 1

Answer:

hope this helps you mate

Answer 2

The value of enthalpy change is -890347.5 J/mol

Explanation:

The reaction for combustion of reaction is

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

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

where,

$\Delta H$ =  enthalpy of the reaction =?

$\Delta E$ = internal energy of the reaction = heat of combustion at constant volume

$\Delta n_g$ = change in the moles of the reaction = Moles of product - Moles of reactant = 1 - 3 = -2

R = gas constant = 8.314J/Kmol

T = temperature = 298.2 K

Putting in the values we get:

$\Delta H=-885389J/mol+(-2)\times 8.314J/Kmol\times 298.2K$

$\Delta H=-885389J/mol+(-4958.5)J/mol$

$\Delta H=-890347.5J/mol$

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