1. A flask is charged with 2.50 atm of N2O4 (g) and 1.50 atm of NO2 (g) at 25.0 degree celcius, then the following equilibrium is acheived. After equilibrium is reached, the partial pressure of NO2 is 2.816.
N2O4 (g) goes to 2NO2 (g)
a.) Calculate the equilibrium partial pressure of N2O4.
b.) Calculate the value of Kp for the reaction at 25.0 degrees celcius.
2. Consider the following reaction for which Kp=0.0752 at 480.0 degree celcius:
2Cl2 (g) + 2H2O (g) goes to 4HCl (g) + O2 (g)
a.) Calculate Kp for: 2HCl (g) + 1/2O2 (g) goes to Cl2 + H2O (g)
b.) Calculate Kp for: 8Cl2 (g) + 8H2O (g) goes to 16HCl (g) + O2 (g)
3. Consider the following reaction for which Kp=0.0752 at 480.0 degree celcius:
2Cl2 (g) + 2H2O (g) goes to 4HCl (g) + O2 (g)
Calculate Kc.
4. For the reaction 2IBr (g) goes to I2 (g) + Br2 (g), Kc=280 at 150.0 degree celcius. Suppose that 0.900 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150.0 degree celcius, what are the equilibrium concetrations of I2, Br2, and IBr?