For this reaction: PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K Initially, you have...
For this reaction:
PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K
Initially, you have 0.10 mol PCl3, 0.10 mol Cl2, and 0.010mol PCl5
all in a 6.40L flask.
Assuming ideal gas conditions, calculate:
Kp, Qp, and state which direction the reaction will shift.
Homework Answers
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For this reaction:
PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K
Initially, you have...
Here is the problem: PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K all in...
Here is the problem: PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K all in a 6.40 L flask PCl3: .1 mol Cl2: .1 mol PCl5: .01 mol Assuming ideal gas conditions, What is the Kp, Qp, and the shift of direction? (if someone can help me set up this problem that would be great!)
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For the reaction, PCl5 (g) <--> PCl3 (g) + Cl2 (g), Kc=33.3 at 760.0 C. In a container at equilibrium, there are 1.29 x 10-3 mol/L of PCl5 and 1.87 x 10-1 mol/L of Cl2. Calculate the [PCl3] in the container.
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The equilibrium constant Kc for the reaction: PCl3(g) + Cl2(g) PCl5(g) is 490 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established? (show work)
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) <=> PCl3 (g) + Cl2 (g) Kc...
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) <=> PCl3 (g) + Cl2 (g) Kc = 1.80 at 250 C A 0.3391 mol sample of PCl5 (g) is injected into an empty 3.60 L reaction vessel held at 250 ∘ C. Calculate the concentrations of PCl5 ( g ) and PCl3 ( g ) at equilibrium. [PCl5] = __________M. [PCl3]=___________M.
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) <---> PCl3(g) + Cl2(g) Kc= 1.80 at...
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) <---> PCl3(g) + Cl2(g) Kc= 1.80 at 250°C A 0.314 mol sample of PCl5(g) is injected into an empty 3.45 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium. [PCl5]= ? M [PCl3]= ? M
Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5(g)↽−−⇀PCl3(g)+Cl2(g) A 13.5 g13.5 g sample of PCl5PCl5 is...
Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5(g)↽−−⇀PCl3(g)+Cl2(g) A 13.5 g13.5 g sample of PCl5PCl5 is added to a sealed 1.50 L1.50 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 34.8%34.8% of the PCl5PCl5 remains. What is the equilibrium constant, ?cKc , for the reaction? ?c=Kc=
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Consider the reaction. PCl5(g)−⇀↽−PCl3(g)+Cl2(g)Kc=0.0420 The concentrations of the products at equilibrium are [PCl3]=0.180 M and [Cl2]=0.280 M. What is the concentration of the reactant, PCl5, at equilibrium?
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250 ∘CPCl5(g)↽−−⇀PCl3(g)+Cl2(g)Kc=1.80 at 250 ∘C A...
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250 ∘CPCl5(g)↽−−⇀PCl3(g)+Cl2(g)Kc=1.80 at 250 ∘C A 0.252 mol0.252 mol sample of PCl5(g)PCl5(g) is injected into an empty 3.40 L3.40 L reaction vessel held at 250 ∘C.250 ∘C. Calculate the concentrations of PCl5(g)PCl5(g) and PCl3(g)PCl3(g) at equilibrium.
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