Consider the following equilibrium reactions: 4NH3(g) + 502(g) 4NO(g) + 6H20(g)
ID: 721095 • Letter: C
Question
Consider the following equilibrium reactions: 4NH3(g) + 502(g) 4NO(g) + 6H20(g) Kp = 1200 at 325 C Into a 6.50 L vessel are added 0.120 moles ammonia, 1.20 moles oxygen, 0.600 moles of nitric oxide, and 0.960 moles of water at 325 C. Will the partial pressure of nitric oxide increase, decrease or stay the same as the reaction approaches equilibrium? Briefly explain your answer! PCI3(g) + 3NH3(g) P(NH2)3(S) + 3HCL(g) KP = 2.81 at 450 K Into a 4.00 L vessel are added 0.600 moles of phosphorus trichloride, 0.160 moles of ammonia, 0.800 moles of triaminophosphine, and 0.120 moles of hydrogen chloride at 450 K. Will the partial pressure of hydrogen chloride increase, decrease, or stay the same as the reaction approaches equilibrium? Briefly explain your answer! Na2CO2(s) + SO2(g) + 1/2O2(g) Na2SO4(s) + CO(g) Kp =0 486 at 145 C Into a 2.50 L vessel are added 0.476 moles of sulfur dioxide, 0.420 moles of oxygen, and 0.354 moles of carbon dioxide at 145 C. Will the partial pressure of sulfur dioxide increase, decrease, or stay the same as the reaction approaches equilibrium? Briefly explain your answer!Explanation / Answer
Can you make it so that all of the info on the page is being shown. the Kp value is being covered.
You can do Kp= Kc(RT)^n
And I would review La Chatlier's Principle, because all of these questions revolve around that.
If you make it so I can see the whole question then I can do some real work on this for ya