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100
Energy that is due to the position or composition of a substance. 

potential energy 

100
These are the two ways to transfer energy 
work and heat 
100
This measures the average kinetic energy of the particles in a substance 
temperature 
200

Kinetic energy depends on these two things of an object 

mass and velocity, KE= 1/2 mv2

200
When particles have the same average kinetic energy, they will have the same 
temperature 
200
This equation gives the enthalpy change of a chemical reaction 

ΔH = Hproducts - Hreactants 

300
This involves the transfer of energy between two objects due to a difference in temperature. 
Heat 
300

If a metal block at 80 °C is placed into a beaker of water at 25 °C, explain the transfer of energy that occurs. 

collisions transfer energy from the metal to the water. 

300
If a solution feels cold, the energy moved from ________________ to __________________. 
the surroundings into the system 
400

A system absorbs 125 kJ of heat while doing 40 kJ of work on the surroundings. Calculate the internal energy, ΔE for the system and include the units in your final answer.  

ΔE = q + w 

ΔE = (+125) + (−40) = +85 kJ

400

This is the energy required to raise the temperature of 1g a substance by 1 °C. 

specific heat capacity

400

The following is an ____________________ reaction.

CH4(g)+2O2(g) → CO2(g) + 2H2O(g) + energy

exothermic 

500

Explain why the following reaction is exothermic in terms of the energy required: 

Xe(g)+2F2(g)→XeF4(s) 

the forming of bonds releases more energy than is required to break bonds. 
500

The magnitude of ΔH is _______________ proportional to the quantities of reactants and products in a reaction. 

directly 
500
The enthalpy change is the same when going from a set of reactants to a set of products regardless of the amount of steps. 
Hess's Law