Question 1

Given the following data:   calculate F1F1F1S1F1F1F10H° for the reaction
NO(g) + O(g) F1F1F1S1F1F1F10 NO2(g)

Accepted Answer

F1F1F1S1F

Question 2

A system delivers 1275 J of heat while the surroundings perform 855 J of work on it. Calculate F1F1F1S1F1F1F10E in J.

Accepted Answer

A)  -2130 J 
B)  -420 J 
C)  420 J 
D)  2130 J 
E)  -1275 J 
A)  -2130 J 
B)  -420 J 
C)  420 J 
D)  2130 J 
E)  -1275 J

Question 3

Calculate the enthalpy change for the reaction NO(g) + O(g) F1F1F1S1F1F1F10 NO2(g)
From the following data:
NO(g) + O3(g) F1F1F1S1F1F1F10 NO2(g) + O2(g) F1F1F1S1F1F1F10H = -198.9 kJ
O3(g) F1F1F1S1F1F1F10 1.5O2(g) F1F1F1S1F1F1F10H = -142.3 kJ
O2(g) F1F1F1S1F1F1F10 2O(g) F1F1F1S1F1F1F10H = 495.0 kJ

Accepted Answer

A)  -551.6 kJ 
B)  -304.1 kJ 
C)  190.9 kJ 
D)  153.8 kJ 
E)  438.4 kJ 
A)  -551.6 kJ 
B)  -304.1 kJ 
C)  190.9 kJ 
D)  153.8 kJ 
E)  438.4 kJ

Question 4

Although internal energy (E) is more fundamental and conceptually easier than enthalpy (H), in most chemical applications F1F1F1S1F1F1F10H is more relevant and useful than F1F1F1S1F1F1F10E. Why?

Accepted Answer

Most chemical processes of interest occu

Question 5

If, as a pioneer, you wished to warm your room by taking an object heated on top of a pot-bellied stove to it, which of the following 15-pound objects, each heated to 100°C, would be the best choice? The specific heat capacity (in J/(g·K)) for each substance is given in parentheses. Iron (0.450), copper (0.387), granite (0.79), gold (0.129), water (4.18).

Accepted Answer

A)  iron 
B)  copper 
C)  granite 
D)  gold 
E)  water 
A)  iron 
B)  copper 
C)  granite 
D)  gold 
E)  water

Given the following data: calculate H° for the reaction NO(g) + O(g)  NO₂(g)

A system delivers 1275 J of heat while the surroundings perform 855 J of work on it. Calculate E in J.

Calculate the enthalpy change for the reaction NO(g) + O(g)  NO₂(g) From the following data: NO(g) + O₃(g)  NO₂(g) + O₂(g) H = -198.9 kJ O₃(g)  1.5O₂(g) H = -142.3 kJ O₂(g)  2O(g) H = 495.0 kJ

Although internal energy (E) is more fundamental and conceptually easier than enthalpy (H), in most chemical applications H is more relevant and useful than E. Why?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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Exam 6: Thermochemistry: Energy Flow and Chemical Change

Given the following data: calculate H° for the reaction NO(g) + O(g)  NO2(g)