Answer:
32.4°C
Explanation:
Consider the following expression:
P•V/T =P'•V'/T'
Where P and P' are respectively the initial and the final pressure, V and V's are respectively initial and final volume, and T and T' are respectively initial and final temperature.
We know that the pressure cannot change, so it means that P = P'
We also know that the volume must be increased in 20%, and if we multiply the volume by 1.2 is like increase it in 20%, so we can write that V' = 1.2•V, and changing a little more we can write that V'/V = 1.2
So let's do some maths:
P•V/T = P'•V'/T'
T'•P•V/T = P'•V'
T'•P•V = P'•V'•T
T'=P'•V'•T/P•V
We know that P'=P so the division is equal to 1:
T'= 1•V'•T/V
We also know that V'/V = 1.2, so:
T' = 1.2•T
And we know the value of T, it's 27, so now we just have to solve it:
T' = 1.2•27
T' = 32.4°C
Probably the answer will be 28.60 because it's a lower number
<h2>
B) Low-pressure systems lead to rain. </h2>
Why? Because high-pressure systems don't allow vapor to get high enough to "become clouds," therefore it will not rain. :)
~pinetree
Answer:
Temperature of boiling point for solution is 101.60°C
Explanation:
This colligative property is boiling point elevation.
ΔT = Kb . m . i
ΔT = T° boiling point for solution - T° boiling point for pure solvent
Kb = The molal boiling point constant
m = molality
i = Van't Hoff factor ( for NaCl i = 2)
NaCl → Na⁺ + Cl⁻
Let's calculate molality (mol of solute in 1kg of solvent)
Mol of salt = Salt mass / Salt Molar mass
Mol of salt = 45 g / 58.45 g/m → 0.769 moles
0.769 moles/0.5 kg = 1.54 m
T° boiling point for solution - 100°C = 0.52°C/m . 1.54m . 2
T° boiling point for solution = (0.52°C/m . 1.54m . 2) + 100°C
T° boiling point for solution = 101.60°C