When a vehicle is parked in the sunlight on a hot summer day, the temperature inside can approach 55°C. One company has patented a non-CFC propelled aerosol that can be sprayed inside a vehicle to reduce the temperature to 25°C within seconds. The spray contains a mixture of two liquids: 10% ethanol, C2H5OH, and 90% water by mass.
equation: C2H5OH + H2O = 2CO2 + 6H2
1.0 g of the aerosol is sprayed into a hot vehicle. How much heat (in kJ) can be absorbed due to vaporization of the aerosol? Note: ΔHvap of water = 44.0 kJ/mol and ΔHvap of ethanol = 38.56 kJ/mol
i used the deltaH = n(deltaHx)
and then found the molar mass, and thereafter i am stuck
chemistry - heat absorption (help) - DrBob222, Friday, April 1, 2011 at 10:47pm
moles ethanol = 0.1/46 = ??
heat absorbed = ?? x 38.58 = z kJ
moles H2O = 0.9/18 = xx
heat absorbed = xx x 44 = y kJ
Total heat absorbed = 2.284 kJ according to my calculation but you need to confirm that.