   Chapter 5.8, Problem 1.3ACP

Chapter
Section
Textbook Problem

The decomposition of nitroglycerin (C3H5N3O9) produces carbon dioxide, nitrogen, water, and oxygen gases. a. Write a balanced chemical equation for the decomposition of nitroglycerin. b. If the decomposition of 1.00 g nitroglycerin releases 6.23 kJ/g of energy in the form of heat, what is the standard molar enthalpy of formation of nitroglycerin?

(a)

Interpretation Introduction

Interpretation:

The balanced equation for the decomposition of nitroglycerin has to be written.

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 decomposition of nitroglycerin produces carbon dioxide and nitrogen and water and oxygen gases

C3H5N3O9CO2+N2+H2O+O2

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

(b)

Interpretation Introduction

Interpretation:

The standard molar enthalpy of formation of the reaction has to be calculated.

Concept Introduction:

Standard enthalpy

Standard enthalpy of the reaction ΔrHo is the change in enthalpy that happens when matter is transformed by a given chemical reaction, when all reactants and products are in their standard states.

The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states.

Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

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