A student heats water to make spaghetti. The student observes that the water in the pot is converted to steam. At the same time, the student observes water droplets sliding down the kitchen window. Which change of state is happening over the pot and which change of state is happening on the kitchen window? The water in the pot is boiling and the water on the kitchen window is condensing. The water in the pot is boiling and the water on the kitchen window is melting. The water in the pot is evaporating and the water on the kitchen window is boiling. The water in the pot is condensing and the water on the kitchen window is boiling.

A student leaving campus for spring break wants to make sure the air in her dorm room has a high water vapor pressure so that her plants are comfortable. The dorm room measures 3.25 m × 4.03 m × 3.04 m and the student places a pan containing 0.580 L of water in the room. Assume that the room is airtight, that there is no water vapor in the air when she closes the door, and that the temperature remains a constant 22 °C. The vapor pressure of water at 22 °C is 19.8 mm Hg. Calculate the pressure that the water vapor would exert if all of the liquid water evaporated. mm Hg Will all of the water in the pan evaporate?

Which diagram corresponds to pure methanol (CH3OH)? (The normal boiling point of methanol is 64.70°C.) O CH, но O CH, HO. O CH, он он

Physical states and phase changes (1) The forces that cause butter to melt on a slice of hot bread are (2) The forces that prevent O2 molecules in the upper atmosphere from forming O atoms are (3) A dog regulates its body temperature by panting, exhaling moisture through its tongue. This phase change is called + . In this process, energy is (4) Frost forms on your car's windshield overnight in the winter. This phase change is called In this process, energy is

33.0 mL of water at 38.9 °C is heated to steam at 128.7 °C. Calculate the the total heat (in kJ) required to accomplish this.Cwater=4.18 J/g°C, Csteam = 2.00 J/g°C, Hvap= 40.7 kJ/mol, dH2O = 1.00 g/mIHint: Draw a heating curve and calculate heat for each segment.

You perform a distillation of a certain liquid at two different pressures The first distillation was done on a day when the pressure was 760 mmHg .   The boiling point (the range where we saw drips come over) is 382.  This is in Kelvin. (This is the normal boiling point of that liquid) Then you connected the adapter to a vacuum.    The liquid now boils at 345 Kelvin.  The enthalpy of vaporization in kJ/mol is 18.5   What is the pressure of the vacuum in mm Hg ?   Hint: Clausius Clapeyron equation ln(P2/P1) =DHvap/R  * (T2-T1)/(T2T1)   or  ln(P2/P1) =DHvap/R  * (1/T1 - 1/T2)   R = 8.3145 J/mol K

Chlorine trifluoride (ClF3) melts at -76.3 °C and boils at 11.8 °C at a constant pressure of 1 atm. What state of matter must a sample of chlorine trifluoride be in at 20°C and 1 atm?

Calculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to 99°C. The specific heat of liquid water is 1.00 cal/g °C

Table 1. Listed below are the common metals with different masses. These metals also have different heat energy and different final temperature at a constant time depending on its thermal conductivity. Metals 25 grams of copper 100 grams of aluminum 20 grams of brass 1 kg steel 50 grams of bronze T₁ 21.4 °C 21.4 °C 21.4 °C 21.4 °C 21.4 °C LE (Ctrl) - T₂ 75 °C 60 °C 55 °C 40 °C 35 °C Heat energy

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on.