Question

Find ΔH for the combustion of methanol (CH4O) to carbon dioxide and liquid water from the following data. The heat capacity of the bomb calorimeter is 34.65 kJ/K and the combustion of 1.777 g of methanol raises the temperature of the calorimeter from 294.50 K to 295.66 K .

Answer 1

CH₂OH +30 • CO₂ + 2H₂o. Tho? Methanal 2 CH OH + 3% (g) - 2co (g) +4 hores Hleet capacity of Band Calorimeter i 34.65 KJ/K Ti (Pmitial Temperature) - 294.5% Top (final semperature) = 295.60K, Bo, AT (rise in Temperature) = Is -Ti = 1.16k Here the energy /enthalpy released from the combustion of methand is being by the Calorimeter set-up assuming no. heat losses , Awam q = CAT 34,65 ks 31.65 vlek Heat capacity a yo. 194 KJ Now 1.7779 of methand releases 40,194 kg of (rolar mass of methanol (CH OH) = 12 +4 +16 = 32 о чк1 1 амалуу- u = 12 +4 +16= 32g/mole ) 329 of methaud releases 40 - 194 x 32 KJ of energy I imole of methand - 1.772 releases & 723,8 kg 723.8 KJ of energy so, (AH)centration (for equation ) 39723.PKT moto (energy released)