   Chapter 17, Problem 52E

Chapter
Section
Textbook Problem

# Hydrogen cyanide is produced industrially by the following exothermic reaction: 2 NH 3 ( g )   +   3 O 2 ( g )   +   2 CH 4 ( g ) → Pt-Rh 100 ∘ C 2 HCN ( g )   +   6 H 2 O ( g ) Is the high temperature needed for thermodynamic or kinetic reasons?

Interpretation Introduction

Interpretation: The reaction of production of hydrogen cyanide is given. If high temperature is required for thermodynamic or kinetic reasons is to be explained.

ΔG=ΔHTΔS

A reaction is said to be spontaneous if the value of ΔG is negative.

The sign of entropy depends on the number of moles. If number of moles decreases, then sign of the entropy will be negative whereas, if the number of moles increases, the sign of entropy will be positive.

Explanation

Explanation

The stated reaction is,

2NH3(g)+3O(g)+2CH4(g)PtRh100°C2HCN(g)+6H2O(g)

Since, the above reaction is exothermic, therefore, value of ΔH is negative.

The number of moles of gaseous molecules in reactant side is,

2+3+2=7mol .

The number of moles of gaseous molecule in product side is,

2+6=8mol

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