   Chapter 5, Problem 33PS

Chapter
Section
Textbook Problem

Nitrogen monoxide, a gas recently found to be involved in a wide range of biological processes, reacts with oxygen to give brown NO2 gas.2 NO(g) + O2(g) → NO2(g)    ΔrH° = –114.1 kJ/mol-rxnIs this reaction endothermic or exothermic? What is the enthalpy change if 1.25 g of NO is converted completely to NO2?

Interpretation Introduction

Interpretation:

The enthalpy change of nitrogen monoxide and the nature of the reaction have to be determined.

Concept Introduction:

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.

Enthalpy of the reaction,ΔrH is the change in enthalpy that happens when matter is transformed by a given chemical reaction

The change in enthalpy, ΔH in kJ per mole of a given reactant for the reaction can be calculated as:

ΔrH=enthalpy changenumber of moles

Explanation

Given,

ΔrHo=-114.1kJ/mol

Mass=1.25g

Determine the amount of nitrogen monoxide in 1.25g

Number of moles = massofthesolutemolarmass

1.25g(1mol÷30.00g) = 0

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