   Chapter 10, Problem 91GQ

Chapter
Section
Textbook Problem

Nitrogen trifluoride is prepared by the reaction of ammonia and fluorine.4 NH3(g) + 3 F2(g) → 3 NH4F(s) + NF3(g)If you mix NH3 with F2 in the correct stoichiometric ratio, and if the total pressure of the mixture is 120 mm Hg, what are the partial pressures of NH3 and F2? When the reactants have been completely consumed, what is the total pressure in the flask? (Assume T is constant.)

Interpretation Introduction

Interpretation:

The nitrogen trifluride prepared from ammonia and fluorine gas, the stoichiometric ratio was given in the reaction.  Further given the reaction partial pressure and total pressure should be calculate and identified.

Concept introduction:

Molar mass: The molar mass of a substance is determined by dividing the given mass of substance by the amount of the substance.

Partial pressure: The mixture of gases each gas has a partial pressure which is the hypothetical pressure of that gas if it alone occupied the entire volume of the original mixture at the same temperature.

Total pressure: The total pressure of a mixture of gases is equal to the sum of the partial pressures of the given component of reaction.  In other words this equation can be used to determine the partial pressure of an individual gas in the mixture.

Explanation

Let us consider the given the equation

4NH3(g)+3F2(g)3NH4F(s)+NF3(g)Thetotlalpressureofreactionmixture=120mmHgHerepartialpressure=partialtemprature×molefractionpartialpressure=120mmHg×14partialpressure=69mmHg

Next we calculate partial pressure of fluorine molecule

4NH3(g)+3F2

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