February 26th, 2018, 03:28 AM  #1 
Newbie Joined: Feb 2018 From: Afghanistan Posts: 17 Thanks: 0  Chemical equilbrium problem
H2(g) + I2(g)⇋ 2HI(g) The system is at equilibrium at a given temperature in a 2 L container. If the system has 0.2 mol of H2, 0.2 mol of I2, and 0.6 mol of HI at equilibrium; how many moles of HI should be added to increase the mol number of H2 to 0.4? I have solved the question this way H2 I2 2HI 0.1 0.1 0.3   +x 0.3 0.3 0.6 0.4 0.4 0.3+x I found Kc from first equilibrium to be 9 So (x0.3)^2/(0.4)^2=9 and x is 1.5M to find mole we multiply it by 2 which give as 3 but answer in my book is 1 is my solution correct or not if why where did I go wrong? please help 

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