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The equilibrium constant, Kp, for the following reaction is 80×10-2at 698 K.2HI(g) H2(g) +  I2(g) If ΔH° for this reaction is 10.4 kJ, what is the value of Kp at 617 K?Kp =

Question
  1. The equilibrium constant, Kp, for the following reaction is 80×10-2at 698 K.

    2HI(g) H2(g) +  I2(g) 


    If ΔH° for this reaction is 10.4 kJ, what is the value of Kp at 617 K?

    Kp =  
check_circleAnswer
Step 1

Kp at 617 K for the given reaction can be determined using van't Hoff equation.

AH1
K2
van 't Hoff equation :ln
K1
1
pl
K22 80x10
T617K
T 698K
AH°10.4kJ= 10.4x103 J
help_outline

Image Transcriptionclose

AH1 K2 van 't Hoff equation :ln K1 1 pl K22 80x10 T617K T 698K AH°10.4kJ= 10.4x103 J

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Step 2

Calculate Kp at 61...

AH1
K
p2
n
1
RT
K
pl
T2
(80x102)
10.4x103
1
1
n
8.314 J/K.mol ( 617K
K
pl
698K
(80x100.23527
In
K
"pl
(80x101.26538
K
K=0.6322
"pl
help_outline

Image Transcriptionclose

AH1 K p2 n 1 RT K pl T2 (80x102) 10.4x103 1 1 n 8.314 J/K.mol ( 617K K pl 698K (80x100.23527 In K "pl (80x101.26538 K K=0.6322 "pl

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