   Chapter 5, Problem 55PS

Chapter
Section
Textbook Problem

(a) Write a balanced chemical equation for the formation of 1 mol of Cr2O3(s) from Cr and O2 in their standard states. (Find the value for ΔfH° for Cr2O3(s) in Appendix L.)(b) What is the standard enthalpy change if 2.4 g of chromium is oxidized to Cr2O3(s)?

(a)

Interpretation Introduction

Interpretation:

The balanced chemical equation for the formation of Cr2O3 has to be determined.

Concept Introduction:

Balanced reaction is a chemical reaction in which number of atoms for each element in the reaction and the total charge are same on both reactant side and the product side.

Steps in balancing the information

• Step 1: Write the unbalanced equation
• Step 2: Find the coefficient to balance the equation.

The coefficient should be reduced to the smallest whole number

Explanation

The unbalanced equation for the reaction is Cr+O2Cr2O3. The equation can be balanced by multiplying the atoms with appropriate number, in the above equation, on the left one chromium atom and two oxygens and on the right hand side two chromium atoms and three oxygen atoms

(b)

Interpretation Introduction

Interpretation:

The enthalpy change for the formation of one mole of Cr2O3 has to be determined.

Concept Introduction:

If a reaction proceeds in two or more other reaction,ΔrH0 for the overall process is the sum of ΔrH0 values of those reactions-Hess’s law.

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