Chemistry 121 Chapter 5 Part 1
16 Questions
| Total Attempts: 118
Study for chemistry test
Questions and Answers
- 1.The study of the heat associated with chemical reactions and physical processes
- A.
State Function
- B.
Thermochemistry
- C.
Chemical Energy
- 2.One that can exchange energy to the surroundings freely
- A.
Open Systems
- B.
Closed System
- C.
Isolated
- 3.Allows energy to escape but not the mass
- A.
Open Systems
- B.
Isolated
- C.
Closed System
- 4.Allows nothing to transfer between the system and the surroundings
- A.
Open Systems
- B.
Isolated
- C.
Closed System
- 5.The ability to do work
- A.
Joules
- B.
State Function
- C.
Energy
- 6.The energy that is stored in the structural units of the chemical substances
- A.
Calorimetry
- B.
Chemical Energy
- C.
Enthalpy (H)
- 7.Gives out heat and transfers heat energy to the surroundings. Theses heat values are always negative
- A.
Endothermic
- B.
Bond Energy
- C.
Exothermic
- 8.Chemical reaction that takes in heat from the surroundings. These heat values are always positive
- A.
Endothermic
- B.
Exothermic
- C.
Chemical Energy
- 9.The unit of measure used for measuring energy changes
- A.
Joules
- B.
Enthalpy Change
- C.
Thermochemistry
- 10.Properties that are determined by the state of the system, regardless of how that condition was achieved
- A.
Hess’s Law
- B.
Closed System
- C.
State Function
- 11.Used to quantify the heat flow into or out of a system in a process that occurs at constant P, V.
- A.
Enthalpy Change
- B.
Enthalpy (H)
- C.
Endothermic
- 12.The measurement of heat changes.
- A.
Calorimetry
- B.
Joules
- C.
State Function
- 13.The value of energy needed to break a bond
- A.
Enthalpy Change
- B.
Energy
- C.
Bond Energy
- 14.The difference in energy between product and reactant
- A.
Thermochemistry
- B.
Enthalpy Change
- C.
State Function
- 15.It takes energy to break bonds, and energy is given back when bonds are made
- A.
Energy, taken
- B.
Energy, given back
- C.
Calorimetry, given back
- 16.When reactants are converted to products, the enthalpy of the reaction is the same, no matter if it occurs in one step or a series of steps
- A.
Hess’s Law
- B.
Calorimetry
- C.
Enthalpy (H)
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