Question

3.6g of butanol was burned, releasing 134kJ of energy. What would the enthalpy of change for a process in which 5.80g sample of butanol is burnt at constant pressure

Answer 1

Answer:

Explanation:

if nothing is given we assume to be the process  is at constant volume.

so apply unitary method

3.6    134

5.8     203

delh = del u +delngrt

c4h9oh+23/4o2 = 4co2+9/2h2o

delng = 4-23/4

=-7/4

delh = 203-7/4*8.314*10^-3*298