February 26th, 2018, 12:52 AM  #1 
Newbie Joined: Feb 2018 From: Afghanistan Posts: 17 Thanks: 0  Chemical equilbrium
H2(g) + I2(g)⇋2Hl(g) Kc = 49 The above reaction reaches equilibrium in a 1.12 L container at 0 °C. What will be the total pressure at equilibrium, if the system starts with 0.9 Μ H2 and 0.9 Μ I2 in the container? 
February 26th, 2018, 01:26 AM  #2 
Member Joined: Feb 2018 From: Iran Posts: 30 Thanks: 3 
H2+I2⇋2HI 0.9M 0.9M  x x +2x  (0.9x) (0.9x) (2x) Kc=49=(2x)^2/(0.9x)^2 X=0.7 SO we have 0.2 M H2 and I2 and 1.4 mole HI Now convert each of them to P using this formula p=CRT And find sum of them 
February 26th, 2018, 05:00 AM  #3  
Senior Member Joined: Jun 2015 From: England Posts: 891 Thanks: 269  Quote:
Since the total number of gas moles does not change as the reaction proceeds, the pressure does not change either (Avogadro). So all that is needed is to use the gas law to calculate the pressure of 1.8 moles of ideal gas in 1.12L , at the temperature concerned. The molar volume is 22.4 L at STP (0 degrees C and 1 Atm)  

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