In: Chemistry
1. At a certain temperature, the Kp for the decomposition of H2S is 0.816. Initially, only H2S is present at a pressure of 0.247 atm in a closed container. What is the total pressure in the container at equilibrium?
2. If a 2.00 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? Kc= 7.01x10^-6 @ 500K.
3. At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M. If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established?
1)
H2S (g) ---------------------------------> H2 (g) + S (g)
0.247 0 0 --------------------> initial
0.247-x x x--------------------> equilibrium
Kp = PH2 x Ps / PH2S
0.816 = x^2 / 0.247 -x
x^2 + 0.816 x - 0.202 = 0
x = 0.199
pressure of H2S = 0.247 - 0.199 = 0.048 atm
pressure of H2 = S = 0.199 atm
total pressure = 0.048 + 0.199 + 0.199
= 0.446 atm
2) reaction missed
3) reaction missed