Question
At 585 K and a total pressure of 1.00 atm, NOCl(g) is 56.4/0 dissociated. Assume that 1.00
mol of ONCl(g) was present before dissociation, (a) How many moles of ONCl(g), NO(g),
and Cl2(g) are present at equilibrium? (b) What is the total number of moles of gas present
at equilibrium? (c) What are the equilibrium partial pressures of the three gases? (d) What
is the numerical value of Kp at 585 K?
mol of ONCl(g) was present before dissociation, (a) How many moles of ONCl(g), NO(g),
and Cl2(g) are present at equilibrium? (b) What is the total number of moles of gas present
at equilibrium? (c) What are the equilibrium partial pressures of the three gases? (d) What
is the numerical value of Kp at 585 K?