Unit 7 Review Game Board

What is the heat of fusion in kJ/g of a substance if it takes J of heat to melt a 55 g sample of the substance? 1.2 kJ/g 1

A reaction occurs spontaneously when  G is: negative 2

605 K equals how many degrees Celsius? 332  C 3

A measure of the average kinetic energy of the particles in a sample of matter? Temperature 4

What letter corresponds to the melting of a solid? b 5

6 In the equation, q = nC  T, what does q stand for? heat

What is a measure of the disorder in a system? entropy 7

What is the formula that defines the change in Gibbs energy?  G =  H – T  S  G reaction =  G products -  G reactants 8

The study of all energy changes is called Thermodynamics 9

10 In the equation, q=nC  T, what does C stand for? Molar heat capacity

11 According to ____________________, the overall enthalpy change in a reaction is equal to the sum of the enthalpy changes of individual steps. Hess’s Law

A positive  S means the process was ____________. More disorderly 12

Entropy plays a larger role in determining the Gibbs energy of reactions that take place at _____________ temperatures. Higher 13

This is the energy of a system at constant pressure. Enthalpy 14

15 In the Gibb’s energy equation, ___________ is the symbol for entropy. S

The standard enthalpy of formation of a(n) ____________ is equal to zero. element 16

17 In the expression q = nC  T, what does n represent? moles

A negative  G means the process was ____________. spontaneous 18

The term ____________________ refers to the amount of energy as heat required to raise the temperature of 1 mole of a substance by 1 K. Molar heat capacity 19

A negative  H means the process was ____________. exothermic 20

A device used to measure the heat absorbed or released in a chemical or physical change calorimeter 21

This equation is used to calculate heat. q=nC  T q=mc p  T q=mL 22

What letter represents the range where the liquid is being warmed? c 23

24 In the Gibb’s energy equation, __________ is the symbol for enthalpy. H

What is 52 Joules in calories? 12.4 calories 25

A 58.2 g sample was heated from 300 K to 350 K. It absorbed 1523 J of energy. What is the specific heat of iron? 0.53 J/gK 26

The total entropy of the products in a reaction is 732 J/K, and the total entropy of the reactants is 524 J/K. What is  S for the reaction? 208 J/K 27

452 ºF to ºC 233  C 28

How much energy as heat does an iron sample gain if its molar heat capacity is 25.1 J/K mol, its mass is g, and it is heated from 15.0°C to 42.0°C? J 29

If 1484 J of energy as heat is released from a 800 g block of aluminum. What temperature change occurred if the molar heat capacity of aluminum is 24.2 J/K. mol? 2.07 K 30

What is the boiling point of the substance (number)? 450 K 31

A g sample of gold was heated from 0°C to 20°C. It absorbed 1108 J of energy. What is the molar heat capacity of gold? 25.6 J/mol. °C 32

341 K equals how many degrees Fahrenheit? 154  C 33

What is the value of  G at 330 K for a reaction in which  H = –103 kJ/mol and  S = J/mol K? kJ/mol 34

35 For a process in which  H is –98 kJ and  S is 132 J/K, calculate the change in the free energy at 0°C kJ/mol

36 When calculating the change in enthalpy of a reaction, this is the equation that is used.  H reaction =  H products -  H reactants

Water has a specific heat of 4.18 J/gK. What is its molar heat capacity? J/molK 37

How much heat would be needed to evaporate 100 g of water if the heat of vaporization of water is 2.26 kJ/g? 226 kJ 38

How much energy as heat does a 9 mol titanium sample gain if its molar heat capacity is 27.8 J/K mol and it is heated from 15°C to 55.0°C? J 39

What is the standard thermodynamic temperature? 25  C (or 298 K) 40

The English measurement for measuring energy is the ___________ calorie 41

What is the melting point of this substance? 300 K 42 AB