H2 (g) + I2 (g) ⇌ 2HI (g)
At 400. K for the reaction above, Kp = 62.5.
(a) If 0.40 mol of HI are introduced into a 1.0 L flask and heated to 400. K, calculate the pressure of HI (g) before any reaction occurs. (4 pts)
(b) Calculate the pressure of each species when equilibrium is established in (a). (6 pts)
(c) H2 (g), I2 (g), and HI (g) are introduced to a flask at 400. K, at pressures of 0.40 atm, 0.40 atm, and 5.0 atm, respectively. Calculate the value of Q and state the direction in which the reaction will proceed to reach equilibrium
(d) In another experiment at a different temperature, H2 (g), I2 (g), and HI (g) are introduced to a flask at pressures of 0.040 atm, 0.020 atm, and 0.090 atm, respectively. If the partial pressure of HI (g) decreases by 50%, calculate the pressure of each species when equilibrium is established.
(e) For the experiment described in part (d) use the following graph as a template to carefully draw three curves – one for each of the three gases. The curves must show how the pressure of each of the three gases changes as equilibrium is established. Label each curve with the formula of the gas.
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