Question

23g of ethanol is subjected to combustion in a bomb calorimeter and the heat produced is 682kJ .Find the value of Delta H​

Answer 1

Given info : 23g of ethanol is subjected to combustion in a bomb calorimeter and the heat produced is 682 kJ.

We have to find the value of ∆H° of C₂H₅OH in kJ/mol.

Solution : here given weight of ethanol = 23 g

We know molecular weight of ethanol = 46.07 g/mol

so no of moles = 23g/46.07g/mol = 0.4992 mol

now ∆H° = heat produced/no of moles

= 682/0.4992

≈ 1366.1 kJ/mol (nearly 1366.47 kJ/mole)

So, ∆H° = 1366.47 kJ/mole

As we know combustion of ethanol is exothermic reaction so, ∆H° = -1366.47 kJ/mole

Therefore the value of ∆H° = -1366.47 kJ/mole