For the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g)...
For the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g) Kp = 8210 At 298 K in a 10.0 L vessel, the known equilibrium values are as follows: 0.087 atm of A, 0.22 mol of B, and 10.5 mol of C. What is the equilibrium partial pressure of D?
Homework Answers
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K: NH4HS(s) ->NH3(g) +...
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K: NH4HS(s) ->NH3(g) + H2S(g) Calculate the partial pressure of each gas and the total pressure at equilibrium when 0.581 moles of NH4HS(s) is introduced into a 1.00 L vessel at 298 K. Assume that the volume occupied by the solid is negligible. PNH3 = atm PH2S = atm Ptotal = atm
For the reaction 2 A (g) – B (g), Kp = 0.00565 at 298 K. When...
For the reaction 2 A (g) – B (g), Kp = 0.00565 at 298 K. When AG = 8.35 kJ/mol, what is the partial pressure of B when the partial pressure of A is 2.00 atm for this reaction at 298 K.
For the reaction 2 A (9) -B (g), Kp = 0.00711 at 298 K. When AG...
For the reaction 2 A (9) -B (g), Kp = 0.00711 at 298 K. When AG = 8.35 kJ/mol, what is the partial pressure of B when the partial pressure of A is 2.00 atm for this reaction at 298 K.
The squares in the equation are equilibrium signs. The equilibrium constant, Ky, for the following reaction...
The squares in the equation are equilibrium signs.
The equilibrium constant, Ky, for the following reaction is 0.110 at 298 K: NH_HS(s) NH3(g) + H2S(g) Calculate the equilibrium partial pressure of H2S when 0.416 moles of NH_HS(s) is introduced into a 1.00 L vessel at 298 K. Phys= c atm The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PC15(g) PC13(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PC15(g) is introduced into...
(1). The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698K. 2HI(g) =H2(g) +...
(1). The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698K. 2HI(g) =H2(g) + I2(g) If an equilibrium mixture of the three gases in a 15.5 L container at 698K contains HI at a pressure of 0.399 atm and H2 at a pressure of 0.562 atm, the equilibrium partial pressure of I2 is atm. (2). Consider the following reaction: PCl5(g) =PCl3(g) + Cl2(g) If 1.17×10-3 moles of PCl5, 0.217 moles of PCl3, and 0.351 moles of Cl2 are at...
1. calculate Kp for the reaction C(s) + Co2(g) = 2Co(g at 1300 k and 1...
1. calculate Kp for the reaction C(s) + Co2(g) = 2Co(g at 1300 k and 1 atm, the equilibrium mixture contains 85% co and 10.5% co2 by volume. 2. calculate the partial pressure of Co2 if Pco is changed to 10^-3 ATM.
1. The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <---->...
1. The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <----> PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.00 atm at 500 K. PPCl5 = atm PPCl3 = atm PCl2 = atm 2. The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K: NH4I(s) <----> NH3(g) + HI(g) Calculate the equilibrium partial pressure of HI when...
The gas arsine AsHs decomposes as follows: 2AsH3 (g) 2As(s) + 3 H2 (g) In an...
The gas arsine AsHs decomposes as follows: 2AsH3 (g) 2As(s) + 3 H2 (g) In an experiment, pure AsHs (g) was placed in an empty, rigid, sealed flask at an initial pressure of 0.6168 atm and 298 K. After 48 hours, the system had come to equilibrium, and the final total pressure in the flask was measured to be 0.7431 atm (a) Fill in the following LC.E. table. 2 As (S) 3 H2(g) Initial (atm) Change (atm) Equilibrium (atm) (b)...
The equilibrium constant, Kp , for the following reaction is 1.04×10-2 at 548 K. NH4Cl(s) NH3(g)...
The equilibrium constant, Kp , for the following reaction is 1.04×10-2 at 548 K. NH4Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 4.51 L container at 548 K contains 1.31 mol of NH4Cl(s) and 0.103 mol of NH3(g), the partial pressure of HCl(g) is __ atm.
For the reaction 2 A(g) + 3 B(g) <-->2 C(g) + 2 D(g), the equilibrium constant...
For the reaction 2 A(g) + 3 B(g) <-->2 C(g) + 2 D(g), the equilibrium constant at 298 K is 1.605×10-11. If the initial partial pressures of A, and B are 0.564 bar, and 0.728 bar, respectively, determine the partial pressure of D (in bar) once equilibrium has been reached at 298 K.
For the reaction 2 A (g) – B (g), Kp = 0.00565 at 298 K. When AG = 8.35 kJ/mol, what is the partial pressure of B when the partial pressure of A is 2.00 atm for this reaction at 298 K.
For the reaction 2 A (9) -B (g), Kp = 0.00711 at 298 K. When AG = 8.35 kJ/mol, what is the partial pressure of B when the partial pressure of A is 2.00 atm for this reaction at 298 K.
The squares in the equation are equilibrium signs.
The equilibrium constant, Ky, for the following reaction is 0.110 at 298 K: NH_HS(s) NH3(g) + H2S(g) Calculate the equilibrium partial pressure of H2S when 0.416 moles of NH_HS(s) is introduced into a 1.00 L vessel at 298 K. Phys= c atm The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PC15(g) PC13(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PC15(g) is introduced into...
The gas arsine AsHs decomposes as follows: 2AsH3 (g) 2As(s) + 3 H2 (g) In an experiment, pure AsHs (g) was placed in an empty, rigid, sealed flask at an initial pressure of 0.6168 atm and 298 K. After 48 hours, the system had come to equilibrium, and the final total pressure in the flask was measured to be 0.7431 atm (a) Fill in the following LC.E. table. 2 As (S) 3 H2(g) Initial (atm) Change (atm) Equilibrium (atm) (b)...
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