Here we have some questions about ideal gases, we will see that the solutions are:
1) The equation for an ideal gas is:
P*V = n*R*T
Taking the quotient in the problem we get that:
(P/T) = n*R/V
The left side is only constant if the right side is also constant, then we must have that:
These are the things that must be held constant.
2) Using the given equation:
[tex]\frac{P_1}{T_1} = \frac{P_2}{T_2}[/tex]
We can just replace the correspondent values:
[tex]\frac{693 \ mmhg}{25 \°C} = \frac{P_2}{37 \° C}\\\\P_2 = (37 \° C)*\frac{693 \ mmhg}{25 \°C} = 1,025.64 \ mmhg[/tex]
3) The heat of vaporization is 40.7 kJ/mol.
We know that 1 mol of water weighs 18.02g
Then in 5 grams, we have:
(5/18.02) = 0.277 moles of water.
If the water is already at 100°C, then we don't need to increase its temperature, so we only need to give enough energy to vaporize it. It is given by the product between the number of moles and the heat of vaporization:
(0.277 moles)*40.7 kJ/mol = 11.29 kJ
4) You can see that a perfume usually vaporizes when it finds a change in the pressure (such that the pressure decreases). From this, we can assume that the vapor pressure is high, or at least larger than the atmospheric pressure
If you want to learn more about ideal gases, you can read:
https://brainly.com/question/25290815
