| Phases of Matter | All About Chemistry | What's the Matter? | Thermochemistry | I Love Science Class!! |
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| Final Question | ||||
Anything that has a definite volume but no definite shape.
Anything that has a definite volume but no definite shape.
liquid
The temperature at which something changes from a liquid to a gas.
The temperature at which something changes from a liquid to a gas.
boiling point
The molecules in this phase of matter are attracted to each other so strongly that the molecules cannot move past one another.
The molecules in this phase of matter are attracted to each other so strongly that the molecules cannot move past one another.
Solid
A measure of the average kinetic energy of the particles in an object is the object's
A measure of the average kinetic energy of the particles in an object is the object's
Temperature
The quantity of energy released or absorbed as heat during a chemical reaction.
The quantity of energy released or absorbed as heat during a chemical reaction.
The branch of chemistry that studies the composition of substances.
The branch of chemistry that studies the composition of substances.
Analytical
The branch of chemistry that is associated with carbon containing compounds.
The branch of chemistry that is associated with carbon containing compounds.
Organic
Matter is neither created or destroyed; it is only changed in any chemical or physical process.
Matter is neither created or destroyed; it is only changed in any chemical or physical process.
Law of Conservation of Matter
This separation technique is based on the principle that substances migrate along a gradient with a solvent at a rate unique to each substance.
This separation technique is based on the principle that substances migrate along a gradient with a solvent at a rate unique to each substance.
Chromatography
Any type of reaction that involves burning can be classified as
Any type of reaction that involves burning can be classified as
Exothermic
A mixture composed of non-uniform components.
A mixture composed of non-uniform components.
Heterogeneous
A sugar water solution is an example of
A sugar water solution is an example of
Homogeneous mixture
Pure substance made of only one type of atom.
Pure substance made of only one type of atom.
Element
What is the amount of heat energy released when 50 g of water is cooled from 20*C to 10*C.
What is the amount of heat energy released when 50 g of water is cooled from 20*C to 10*C.
2090 J
A 6.75 g sample of gold is heated using 50.6 J of energy. If the original temperature of the gold is 25*C, what is its final temperature?
A 6.75 g sample of gold is heated using 50.6 J of energy. If the original temperature of the gold is 25*C, what is its final temperature?
82.7 J
The heat required to raise the temperature of 1 gram of a substance by 1 degree Celcius.
The heat required to raise the temperature of 1 gram of a substance by 1 degree Celcius.
specific heat
The amount of energy absorbed or lost by a system as heat during a process at constant pressure.
The amount of energy absorbed or lost by a system as heat during a process at constant pressure.
Enthalpy
The type of chemical reaction that absorbs energy and requires energy for the reaction to occur.
The type of chemical reaction that absorbs energy and requires energy for the reaction to occur.
Endothermic
What is the enthalpy change when 10 g of water is heated from 12 to 27 degrees celsius.
What is the enthalpy change when 10 g of water is heated from 12 to 27 degrees celsius.
627 J
How much energy is required to increase the temperature of 100 g of water from -50*C to -10*C?
How much energy is required to increase the temperature of 100 g of water from -50*C to -10*C?
8200 J
The factor in an experiment that the experimenter attempts to keep the same.
The factor in an experiment that the experimenter attempts to keep the same.
Constant
The process of converting from a gas to a solid with no liquid phase.
The process of converting from a gas to a solid with no liquid phase.
Deposition
A 4 g sample of iron was heated from 0*C to 20*C. It absorbed 35.2 J of energy as heat. What is the specific heat of this piece of iron?
A 4 g sample of iron was heated from 0*C to 20*C. It absorbed 35.2 J of energy as heat. What is the specific heat of this piece of iron?
0.44 J/g*C
How much energy does an 8 g copper sample absorb as heat as it is heated from 10*C to 40*C?
How much energy does an 8 g copper sample absorb as heat as it is heated from 10*C to 40*C?
92.2 J
What occurs when energy is removed from a liquid-vapor system at equilibrium?
What occurs when energy is removed from a liquid-vapor system at equilibrium?
The amount of liquid increases.
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