A 6.00L reaction vessel at 491°C contained 0.488 mol H2, 0.206 mol I2 and 2.250
mol HI. Assuming the substances are at equilibrium, find the value of Kc at
491°C for the reaction of hydrogen and iodine to give hydrogen iodide. The
equation is
H2(g) + I2(g) -> HI(g)
If the above reaction was reversed, but the same amounts of compounds were
present at equilibrium, what is the Kc of this reverse reaction? What is the
relationship between the Kc for the forward reaction and the Kc for the reverse
reaction?
mol HI. Assuming the substances are at equilibrium, find the value of Kc at
491°C for the reaction of hydrogen and iodine to give hydrogen iodide. The
equation is
H2(g) + I2(g) -> HI(g)
If the above reaction was reversed, but the same amounts of compounds were
present at equilibrium, what is the Kc of this reverse reaction? What is the
relationship between the Kc for the forward reaction and the Kc for the reverse
reaction?