Explanation The required reaction is given below. N 2 ( g ) + 3 H 2 ( s ) ⇌ 2 N H 3 ( g ) The expression for equilibrium constant for the above reaction can be written as shown below, K c = [ N H 3 ] 2 [ N 2 ] [ H 2 ] 3 Given that, the 0.20 m o l N 2 a n d 0.20 m o l H 2 was introduced into a flask of volume 25.0 L . The concentrations of N 2 ( g ) a n d H 2 ( g ) can be calculated as given below. [ N 2 ] = M o l e s V o l u m e = 0.20 m o l 25.00 L = 8 × 1 0 - 3 M [ H 2 ] = M o l e s V o l u m e = 0.20 m o l 25.00 L = 8 × 1 0 - 3 M An equilibrium table can be set up as given below. C o m p o s i t i o n ( M ) N 2 H 2 N H 3 I n i t i a l c o n c e n t r a t i o n 8 × 10 − 3 8 × 10 − 3 0 C h a n g e i n c o n c e n t r a t i o n − x − 3 x + 2 x E q u i l i b r i u m c o n c e n t r a t i o n 8 × 10 − 3 − x 8 × 10 − 3 − 3 x 2 x Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below. K c = ( 2 x ) 2 ( 8 × 10 − 3 − x ) ( 8 × 10 − 3 − x ) 3 It is given that, at equilibrium 5 % of the nitrogen gas had reacted, that means the change in concentration of nitrogen gas is 5 % of its initial concentration

Chemical Principles: The Quest for Insight

7th Edition

ISBN: 9781464183959

Author: Peter Atkins, Loretta Jones, Leroy Laverman

Publisher: W. H. Freeman

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Chapter 5, Problem 5I.20E

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Interpretation:

The equilibrium constant for the reaction N2(g)+3H2(s)⇌2NH3(g) has to be calculated.

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Chapter 5, Problem 5I.19E

Chapter 5, Problem 5I.21E

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A reaction mixture that consisted of 0.20 mol N2(g) and 0.20 mol H2(g) was introduced into a reactor of volume 25.0 L and heated. At equilibrium, 5.0% of the nitrogen gas had reacted. What is the value of the equilibrium constant KC for the reaction N2(g) + 3H2(g) ⇋ 2 NH3(g) at this temperature?

When equal amounts of hydrogen, H2, and iodine, I2, are mixed together at a total pressure of 1 bar, the partial pressure of hydrogen iodide, HI, vapour produced from by the reaction H2(g) + I2(g) ⇌ 2 HI(g) is 22.8 kPa. Calculate the equilibrium constant for the reaction.

The equilibrium constant Kc for the reaction N2(g) + O2(g)⇋ 2NO(g) at 1200 degrees Celsius is 1.00 x 10-5. Calculate the equilibrium molar concentrations of NO, N2, O2 in a reaction vessel of volume 10.00 L that initially held 0.312 mol N2 and 0.407 mol O2.

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Chemical Principles: The Quest for Insight

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The equilibrium constant for the reaction N 2 ( g ) + 3 H 2 ( s ) ⇌ 2 N H 3 ( g ) has to be calculated.

Solution Summary: The author explains how the equilibrium constant for the reaction N_2(g)+3H

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Interpretation:

The equilibrium constant for the reaction N2(g)+3H2(s)⇌2NH3(g) has to be calculated.

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Chapter 5 Solutions

The equilibrium constant for the reaction N 2 ( g ) + 3 H 2 ( s ) ⇌ 2 N H 3 ( g ) has to be calculated.

Solution Summary: The author explains how the equilibrium constant for the reaction N_2(g)+3H

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Interpretation: The equilibrium constant for the reaction N2(g)+3H2(s)⇌2NH3(g) has to be calculated.

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Chapter 5 Solutions

Interpretation:

The equilibrium constant for the reaction N2(g)+3H2(s)⇌2NH3(g) has to be calculated.