Thank you for solving the previous question! This is the second Question: 2. Hydrogen iodide can be produced by the reversible reaction of hydrogen gas and iodide according to: H2(g) + I2(g) 2HI(g) a.Keqfor this reaction is 2.25 x 103 at a temperature of 753 C a. Calculate the concentration of HI in an equilibrium mixture if the concentration of H2 is 0.15M and the concentration of I2 is 0.25M. b.2.4 moles of H2(g) and 1.5 moles of I2(g) were placed in a 2.0L vessel maintained at a temperature of 753C. After 2 hours
Thank you for solving the previous question!
This is the second Question:
2. Hydrogen iodide can be produced by the reversible reaction of hydrogen gas and iodide
according to:
H2(g) + I2(g) 2HI(g)
a.Keqfor this reaction is 2.25 x 103 at a temperature of 753 C
a. Calculate the concentration of HI in an equilibrium mixture if the concentration of H2
is 0.15M and the concentration of I2 is 0.25M.
b.2.4 moles of H2(g) and 1.5 moles of I2(g) were placed in a 2.0L vessel maintained at a
temperature of 753C. After 2 hours, number of moles of each gas present were as
follows Moles of H2(g) Moles of I2(g) Moles of HI(g)
1.7 0.8 1.4
Show by calculation whether the forward or reverse reaction must increase for the system to come to a state of dynamic equilibrium
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