Practice Test: Chapter 6

Matching skip

Short Answer skip

1. work
   
2. law of conservation of energy
   
3. 2 characteristics of ∆H for a reaction
   
4. Standard Enthalpy of Formation ∆Hf˚
   
5. frictional heating
   

Multiple Choice skip

1. hess's law
   1. Energy flows out of a system. Some of the potential energy stored in the chemical bonds is being converted to thermal energy via heat. ∆(PE) transferred to surroundings through heat
   2. Transfer of energy between two objects due to a temperature difference. Not a substance contained by an object
   3. H products - H reactants. Endothermic: ∆H = +. Exothermic: ∆H = -
   4. energy due to position or composition
   5. Change in enthalpy in going from some initial state to some final state is independent of the pathway. In going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps. ∆H = enthalpy change
2. ∆H =
   1. =c x m x ∆T
   2. Change in enthalpy that accompanies the formation of one mole of a compound from its elements with all substances in their standard states
   3. Kinetic energy transferred to a surface as heat
   4. Energy can be converted from one form to another but can be neither created nor destroyed
   5. H products - H reactants. Endothermic: ∆H = +. Exothermic: ∆H = -
3. exothermic
   1. Transfer of energy between two objects due to a temperature difference. Not a substance contained by an object
   2. No work is done. Energy change determined by measuring increase in the temperature of water and other calorimeter parts. ∆E = q +w = qv
   3. Energy flows out of a system. Some of the potential energy stored in the chemical bonds is being converted to thermal energy via heat. ∆(PE) transferred to surroundings through heat
   4. A change in function in going from one state to another state is independent of particular pathway taken between two states. Eg. Total energy. Work and heat are not state functions
   5. Heat capacity per mole
4. specific heat capacity
   1. Heat capacity per mole
   2. Energy can be converted from one form to another but can be neither created nor destroyed
   3. heat capacity per gram
   4. The energy of the universe is constant. Same as law of conservation of energy
   5. If a reaction is reversed, the sign of ∆H is also reversed. The magnitude of ∆H is directly proportional to the quantities of reactants and products in a reaction. If the coefficients in a balanced reaction are multiplied by an integer, the value of ∆H is multiplied by the same integer
5. heat
   1. Transfer of energy between two objects due to a temperature difference. Not a substance contained by an object
   2. H = E + PV. State function. At constant pressure, (where only PV work is allowed), the change in enthalpy ∆H of the system is equal to the energy flow as heat. Heat of reaction = change in enthalpy
   3. Subtracting the enthalpies of formation of the reactants from the enthalpies of formation of the products. Multiply the enthalpies of formation by integers as required by the balanced equation. When reaction reversed, sign changes ∆H. Elements in their standard states are not included
   4. Heat capacity per mole

True or False skip

1. constant pressure calorimetry
   Corresponding process has been carried out under standard conditions

   True   False

2. temperature
   A change in function in going from one state to another state is independent of particular pathway taken between two states. Eg. Total energy. Work and heat are not state functions

   True   False

3. w = -P∆V
   Science of measuring heat based on observing temperature change

   True   False

4. potential energy
   energy due to position or composition

   True   False

5. Degree symbol on a thermodynamic function
   Kinetic energy transferred to a surface as heat

   True   False