Answer:
A, Venus.
Explanation:
Temperatures reach up to 460° C on a regular basis.
When
a solute is added to a solvent, some properties are affected and these set of
properties are called colligative properties. Freezing point depression calculation is used for this type of problem. Calculations are as
follows:
<span>ΔT(freezing point)
= (Kf)m
ΔT(freezing point)
= 1.86 °C kg / mol (50.0/92.09 mol / .200 kg)
ΔT(freezing point) = 5.04 </span>°C <span>
Tf - T = 5.04 </span>°C <span>
T = -5.04 °C</span>
<span>
</span>
Answer:
On frigid days, water vapor in the air can transform directly into solid ice, depositing a thin layer on surfaces such as a windowpane or car windshield. Though commonplace, this process is one that has kept physicists and chemists busy figuring out the details for decades.
Answer:
ΔH= 3KJ
Explanation:
The total heat absorbed is the total energy in the process, and that is in form of entalpy.
ΔH = q + ΔHvap, where q is the heat necessary for elevate the temperature of dietil ether. Suppose the initial temperature is room temperature (25ºC=298 K), then
q= 10g x2.261 J/gK x(310 K - 298K)= 271.32 J= 0.3 kJ
Then
ΔHvap = 10g C4H10O x (1 mol C4H10O/74.12 g C4H10O) x( 15.7 KJ/ 1 mol C4H10O) = 2.12 KJ
ΔH= 2.5KJ ≈ 3KJ
