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.

Question

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
please help!c

Answer 1

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.

Answer 2

To calculate the heat absorbed due to vaporization of the aerosol, you first need to determine the number of moles of each component in the aerosol spray.

Step 1: Calculate the number of moles of ethanol (C2H5OH) in 1.0 g of the aerosol spray.
First, find the molar mass of C2H5OH:
C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol

Molar mass of C2H5OH = (2 * 12.01 g/mol) + (6 * 1.008 g/mol) + 16.00 g/mol = 46.07 g/mol

Next, calculate the number of moles of ethanol:
Number of moles of ethanol = mass of ethanol (in g) / molar mass of ethanol

Number of moles of ethanol = 0.10 g / 46.07 g/mol

Step 2: Calculate the number of moles of water (H2O) in 1.0 g of the aerosol spray.
In this case, the mixture is 90% water. So, we can assume that 1 g of the aerosol contains 0.90 g of water.

Next, calculate the number of moles of water:
Number of moles of water = mass of water (in g) / molar mass of water

Number of moles of water = 0.90 g / 18.02 g/mol

Step 3: Calculate the heat absorbed due to vaporization of ethanol and water.
For ethanol:
Heat absorbed due to vaporization of ethanol = moles of ethanol * ΔHvap of ethanol

For water:
Heat absorbed due to vaporization of water = moles of water * ΔHvap of water

Finally, sum up the heat absorbed due to vaporization of ethanol and water to get the total heat absorbed.

Remember to convert moles of ethanol and water into kJ/mol using the molar heat of vaporization provided.

I hope this helps you solve the problem!