Answer:
I believe it is a hope this helps
Answer:
Before heating, the can is filled with water and air. By boiling the water, the water changes states from a liquid to a gas. This gas is called water vapor. The water vapor pushes the air that was originally inside the can out into the atmosphere. When the can is turned upside down and placed in the water, the mouth of the can forms an airtight seal against the surface of the water in the bowl. And then just after that, all of the water vapor that pushed the air out of the can and filled up the inside of the can turns into only a drop or two of liquid, which takes up much less space. This small amount of condensed water cannot exert much pressure on the inside walls of the can, and none of the outside air can get back into the can. The result is the pressure of the air pushing from the outside of the can is great enough to crush it.
To make the internal pressure of the can balance with the external pressure on the can, the can implodes.
The outside air pressure pushing downward on the surface of the water is greater than the force inside the can and the water gets pushed up into the can.
Answer:
Increasing the temperature of a system will increase the rate of a reaction. More particles are moving faster, and have more energy, increasing the overall rate of reaction.
Explanation:
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Answer:
Bonding Order = number of bonding electrons – number of antibonding electrons/2.
So for CO2, there is a total of 16 electrons, 8 of which are antibonding electrons.
So 16 – 8 = 8; divided by 2 = 4. So, 4 is the bonding order of CO2. The molecular structure of CO2 looks like this:
..~-~~..
O=C=O
..~-~~..
Answer:
i = 2.79
Explanation:
The excersise talks about the colligative property, freezing point depression.
Formula to calculate the freezing point of a solution is:
Freezing point of pure solvent - Freezing point of solution = m . Kf . i
Let's replace data given. (i = Van't Hoff factor, numbers of ions dissolved in solution)
48.1°C - 44°C = 0.15 m . 9.78°C/m . i
4.1°C / (0.15 m . 9.78°C/m) = i
i = 2.79
In this case, numbers of ions dissolved can decrease the freezing point of a solution, which is always lower than pure solvent.