   Chapter 13, Problem 70E

Chapter
Section
Textbook Problem

# Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction N 2 ( g ) + 3 H 2 ( g ) ⇌ 2 NH 3 ( g ) equilibrium constants (Kp values) as a function of temperature are300°C, 4.34 × 10−3500°C, 1.45 × 10−5600°C, 2.25 × 10−6Is the reaction exothermic or endothermic?

Interpretation Introduction

Interpretation: The reaction of production of ammonia and values of equilibrium constant with increase in temperature are given. The type of reaction (endothermic or exothermic) is to be predicted.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented as K .

To determine: If the reaction of production of ammonia is endothermic or exothermic with increase in temperature

Explanation

Explanation

The stated reaction is,

N2(g)+3H2(g)2NH3(g)

At equilibrium, the equilibrium ratio is expressed by the formula,

K=ConcentrationofproductsConcentrationofreactants

Where,

• K is the equilibrium constant

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