A sample of N_2O_4 (0.400 mol) was placed in an empty 1.00 L container at 500 K.
ID: 919896 • Letter: A
Question
A sample of N_2O_4 (0.400 mol) was placed in an empty 1.00 L container at 500 K. After equilibrium was reached, the concentration of NO_2 was found to be 6.29 times 10_4 M. Calculate the value of K_c at 500 K for the reaction: N_2O_4(g) 2 NO_2(g) The a pale yellow solid, NH_4HS, decomposes readily to give H_2S and NH_3 as shown below: NH_4HS (s) H_2S(g) + NH_3 (g) What is the partial pressure equilibrium constant, K_p, for the reaction given that the partial pressure of H_2 S(g) gas in an equilibrium mixture at 50 degree C is 0.65 atm. If the value of the partial equilibrium constant, k_p, for the reaction: 2SO_3(g) 2SO_2(g) + O_2(g)Explanation / Answer
7)
NH4HS (s) <----> H2S (g) + NH3 (g)
p p
given that partial pressure of H2S = 0.65 atm
So,
p = 0.65 atm
Kp = p(H2S) * p(NH3)
= p*p
= 0.65 * 0.65
=0.4225
Answer: 0.4225