Answer :
The pressure of carbon dioxide in the atmosphere in mmHg is 0.239mmHg.
The pressure of carbon dioxide in the atmosphere in atm is 
.
Explanation :
The conversion used for pressure from torr to mmHg is:
1 torr = 1 mmHg
The conversion used pressure from torr to atm is:
1 atm = 760 torr
or,
As we are given the pressure of carbon dioxide in the atmosphere 0.239 torr. Now we have to determine the pressure of carbon dioxide in the atmosphere in mmHg and atm.
<u>Pressure in mmHg :</u>
As, 
So, 
Thus, the pressure of carbon dioxide in the atmosphere in mmHg is 0.239mmHg.
<u>Pressure in atm:</u>
As,
So, 
Thus, the pressure of carbon dioxide in the atmosphere in atm is .
Answer:
Enthalpy change = 74.36 kJ
Explanation:
Enthalpy change is defines as the heat absorbed or evolved during a chemical reaction at constant pressure and volume
Reaction:
H2O(l) --> H2O(g)
DHr = mCsDT
Where m is the mass of water
Cs is the specific heat capacity
DT is the temperature difference
= 31.6 * 4.18 * (25 - 3.2)
= 2879.518 J
DHvap = 44kJ/mol
Moles of water = mass/molecular weight
Molecular weight = (1*2) + 16
= 18g/mol
Moles of water = 31.6/18
= 1.756 moles
DHvap = 44 * 1.756
= 77.244kJ
DH = DHproduct - DHreactant
DHproduct = DHvap = 77.24kJ
DHreactant = DHr = 2879.518J = 2.880kJ
= 77.24 - 2.880
DH = 74.36kJ
Enthalpy change = 74.36 kJ
It just is because science is science and it's supposed to make sense
