Consider the reaction: 2H 2 S (g) + 3O 2 (g) 2SO 2 (g) + 2H 2 O (g) to answer th
ID: 103748 • Letter: C
Question
Consider the reaction: 2H2S (g) + 3O2 (g) 2SO2 (g) + 2H2O (g) to answer the following questions.
Refer to the reaction shown above. Increasing the pressure __________.
will shift the reaction to the right
will have no effect
will shift the reaction to the left
will have an unknown effect, since the temperature is unknown
Kp = [NH3]2/[N2][H2]3
Kp = [2NH3]2/[N2][3H2]3
Kp = [N2][H2]3/[NH3]2
Kp = [N2][3H2]3/[2NH3]2
Consider the reaction: 2H2S (g) + 3O2 (g) 2SO2 (g) + 2H2O (g) to answer the following questions.
Refer to the reaction shown above. Which of the following will shift the equilibrium to the left?
adding sulfur dioxide
adding hydrogen sulfide
decreasing the pressure
both A and C
Kp = PH2S2PO23/PSO2PH2O2
Kp = PSO2PH2O2/PH2S2PO23
Kp = PSO2PH2O/PH2SPO2
Kp = PH2SPO2/PSO2PH2O
A.will shift the reaction to the right
B.will have no effect
C.will shift the reaction to the left
D.will have an unknown effect, since the temperature is unknown
Explanation / Answer
Q1.
increase in pressure favour the least mol formation
therefore, these are the products, so increases to the right
Q2
N/A
Q3
2H2S (g) + 3O2 (g) 2SO2 (g) + 2H2O (g)
addition of SO2 increases the shift to the right,
addition of H2S wil not go to the left
decrease in P --> Favours the most moles, therefore, lef tshift
chose D
Q4 N/A