Question 1

The specific heat of silver is 0.235 J/g·°C. How many joules of heat are required to heat a 75 g silver spoon from 20°C to 35°C?

Accepted Answer

The answer of The specific heat of silver is 0.235...

Question 2

Aluminum oxide can be reduced to aluminum metal using carbon, the other reaction product being carbon monoxide. Determine the enthalpy change when 12.5 g of aluminum is produced by this method. [$\Delta$H°f(carbon monoxide)= -110.5 kJ/mol; $\Delta$H°f(aluminum oxide)= -1669.8 kJ/mol]

Accepted Answer

A) 725 kJ 
B) 697 kJ 
C) 310 kJ 
D) 361 kJ 
E) 1504 kJ 
A) 725 kJ 
B) 697 kJ 
C) 310 kJ 
D) 361 kJ 
E) 1504 kJ

Question 3

The enthalpy change when a strong acid is neutralized by strong base is -56.1 kJ/mol. If 12.0 mL of 6.00 M HBr at 21.30°C is mixed with 300. mL of 0.250 M NaOH, also at 21.30°C, what will be the maximum temperature reached by the resulting solution? (Assume that there is no heat loss to the container, that the specific heat of the final solution is 4.18 J/g·°C, and that the density of the final solution is that of water.)

Accepted Answer

A) 18.20°C 
B) 24.53°C 
C) 101.8°C 
D) 24.40°C 
E) 34.25°C 
A) 18.20°C 
B) 24.53°C 
C) 101.8°C 
D) 24.40°C 
E) 34.25°C

Question 4

Which of the following processes is endothermic?

Accepted Answer

A) O2(g)+ 2H2(g)$\rarr$2H2O(g) 
B) H2O(g)$\rarr$H2O(l) 
C) 3O2(g)+ 2CH3OH(g)$\rarr$2CO2(g)+ 2H2O(g) 
D) H2O(s)$\rarr$H2O(l) 
A) O2(g)+ 2H2(g)$\rarr$2H2O(g) 
B) H2O(g)$\rarr$H2O(l) 
C) 3O2(g)+ 2CH3OH(g)$\rarr$2CO2(g)+ 2H2O(g) 
D) H2O(s)$\rarr$H2O(l)

Question 5

Which of the following processes always results in an increase in the energy of a system?

Accepted Answer

A) The system loses heat and does work on the surroundings. 
B) The system gains heat and does work on the surroundings. 
C) The system loses heat and has work done on it by the surroundings. 
D) The system gains heat and has work done on it by the surroundings. 
E) None of these is always true. 
A) The system loses heat and does work on the surroundings. 
B) The system gains heat and does work on the surroundings. 
C) The system loses heat and has work done on it by the surroundings. 
D) The system gains heat and has work done on it by the surroundings. 
E) None of these is always true.

The specific heat of silver is 0.235 J/g·°C. How many joules of heat are required to heat a 75 g silver spoon from 20°C to 35°C?

Aluminum oxide can be reduced to aluminum metal using carbon, the other reaction product being carbon monoxide. Determine the enthalpy change when 12.5 g of aluminum is produced by this method. [ $\Delta$ H°_f(carbon monoxide)= -110.5 kJ/mol; $\Delta$ H°_f(aluminum oxide)= -1669.8 kJ/mol]

Which of the following processes is endothermic?

Which of the following processes always results in an increase in the energy of a system?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 6: Energy Relationships in Chemical Reactions

The specific heat of silver is 0.235 J/g·°C. How many joules of heat are required to heat a 75 g silver spoon from 20°C to 35°C?

Aluminum oxide can be reduced to aluminum metal using carbon, the other reaction product being carbon monoxide. Determine the enthalpy change when 12.5 g of aluminum is produced by this method. [ Δ\DeltaΔ H°f(carbon monoxide)= -110.5 kJ/mol; Δ\DeltaΔ H°f(aluminum oxide)= -1669.8 kJ/mol]

Which of the following processes is endothermic?

Which of the following processes always results in an increase in the energy of a system?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Aluminum oxide can be reduced to aluminum metal using carbon, the other reaction product being carbon monoxide. Determine the enthalpy change when 12.5 g of aluminum is produced by this method. [ $\Delta$ H°_f(carbon monoxide)= -110.5 kJ/mol; $\Delta$ H°_f(aluminum oxide)= -1669.8 kJ/mol]