A(g) + 2B(g) C(g) + D(g) If you initially start with 1.00 atm of both A and B an
ID: 878878 • Letter: A
Question
A(g) + 2B(g) C(g) + D(g)
If you initially start with 1.00 atm of both A and B and find that at equilibrium 0.295 atm of C is present, what is the value of Kp for the reaction at the temperature the reaction was run?
A(g) + 2B(g) 2C(g)
If Kp for the above reaction is 4.50 x 10-2, what is the value of Q if the pressures of A, B, and C are 0.250 atm, 0.127 atm, and 0.450atm respectively?
A(aq) + B(aq) 2C(aq)
If the value of Kc for the reaction is 449, what is the concentration of C at equilibrium if initial concentrations of A and B are both 0.500 M. (Hint: Everthing is squared after you set-up the equilibrium expression with the values given.
A(s) + 2B(g) 2C(g) + D(g)
If the value of Kc for the reaction is 10.5, what is the value of Kp at 295 K?
A(g) + 2B(g) C(g) + D(g)
At equilibrium the above reaction is found to contain C and D at a pressure of 2.41 atm and A at a pressure of 1.23 atm and B at a pressure of 0.480 atm. What is the value of Kp for the reaction?
Explanation / Answer
Kp = PCPD / PAPB = (0.295)2 = 0.087
Q = [0.450]2 / [0.25][0.127]2 = 50.22
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