Ok so I am given H2 + I2 = 2HI
.500 mol H2
1.00 mole I2
placed in a 10 L vessel what is the mole fraction of HI in mixturewhen equilibrium is reached at 205C
I have an appendix that provides deltaG,H ect
from this I conclude that I have a reaction that has 16.208KJ/mol
an equilibrium constain of K= 1.44x10^-3
I have a K2 = 6.14x10^-3

and delta G of 16.208. What is the mole fraction of this reaction?

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debnathtonmoy93Lv3

12 Feb 2023

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Related questions

Consider the following reaction:

H₂(g) + I₂(g) <=> 2HI(g)

i) If 12.7 g of I₂solid is placed in a 10 dm³ vessel at 40.0 Â°C and allowed to react, how much H₂ gas must be added to remove the solid? The vapor pressure of I₂ is 0.10 bar at this temperature and the equilibrium constant, Kp = 20.00 at this temperature.

ii) The following data were obtained for this reaction; DHÂ° = -9.6 kJmol^-1, DSÂ° = 22.18 JK^-1mol^-1, and DC_P = -7.11 JK^-1mol^-1. Calculate the equilibrium constants K_P, K_C and K_X at 500 K.

c)What would the mole fraction of HI present at equilibrium be if at the start 10 bar HI were added to a 10 dm³ vessel. How would this value change with pressure?

H₂(g) + I₂(g) <--> 2HI(g)

i) If 12.7 g of I₂ solid is placed in a 10 dm³ vessel at 40.0 Â°C and allowed to react, how much H₂ gas must be added to remove the solid? The vapor pressure of I₂ is 0.10 bar at this temperature and the equilibrium constant, Kp = 20.00 at this temperature.

ii) The following data were obtained for this reaction; dHÂ°= -9.6 kJmol^-1,dSÂ°= 22.18 JK^-1mol^-1, and dC_P= -7.11 JK^-1mol^-1. Calculate the equilibrium constants K_P, K_C and K_X at 500K.

c)What would the mole fraction of HI present at equilibrium be if at the start 10 bar HI were added to a 10 dm³ vessel. How would this value change with pressure?

Physical chemistry. Please show your steps and assumptions made. Thank you for your time