For the following hypothetical reaction, 2 C(g) ↔ D(g) + E(g) determine what the system will do given P(C) = 1.58 atm, P(D) =0.15 atm, P(E) = 0.050 atm and Kp = 3×10-3.
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For the following hypothetical reaction, 2 C(g) ↔ D(g) + E(g) determine what the system will...
30. For a reaction: A (g) + B (g) ↔ C (g) + D (s), 6.0 atm of A and 5.0 atm of B are initially added to a container. When equilibrium is reached, there are 4.0 atm of C. What is the Kp for the reaction?
The equilibrium partial pressures for the reaction Cl2 (g) + PCl3 (g) ↔ PCl5 (g) at 300 K are PCl2 = 0.75 atm, PPCl3 = 0.45 atm, and PPCl5 = 0.73 atm. The value of Kp is __________. A. 0.15 B. 0.048 C. 4.7 D. 2.16
Given the reaction at a certain temperature: H2(g) + I2(g) ↔ 2 HI(g). At equilibrium, the partial pressure of HI is 3.8×10–3 atm and the partial pressures of H2 and I2 are 0.20 atm each. The Kp of this reaction is [X]. (Fill in the blank; report with correct number of significant figures.
Consider the following reaction. N2(g) + O2(g) 2 NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm, and 0.050 atm, respectively, at 2200°C, what is KP?
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ mol-1) at 22 °C given that ∆rG° = -103.7 kJ mol-1, P(C2H4) = 2.66×10-2 bar, P(H2) = 8.50×10-3 bar, and P(C2H6) = 2.50×10-1 bar.
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ mol-1) at 20 °C given that ∆rG° = -92.2 kJ mol-1, P(C2H4) = 1.41×10-2 bar, P(H2) = 1.47×10-2 bar, and P(C2H6) = 3.00×10-1 bar.
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ mol-1) at 29 °C given that ∆rG° = -116.4 kJ mol-1, P(C2H4) = 1.53×10-2 bar, P(H2) = 1.09×10-2 bar, and P(C2H6) = 3.30×10-1 bar
For the reaction 2 A(g) + 3 B(g) ↔ 2 C(g) + 2 D(g), the equilibrium constant at 298 K is 1.409×10-11. If the initial partial pressures of A, and B are 0.500 bar, and 0.718 bar, respectively, determine the partial pressure of D (in bar) once equilibrium has been reached at 298 K.
Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) + Cl2(g) at 291 K given the following information, 2 N2(g) + 2 O2(g) ↔ 4 NO(g); K = 5.397×10-61 NO + 1/2 Cl2(g) ↔ NOCl(g); K = 2.432×104
The equilibrium constant expression K p for the reaction 2NH 3 (g) ↔ N2 (g) + 3H2 (g) is __________. A. Kp = PN2(3PH2)3/(2PNH3)2 B. Kp = PNH32/PN2PH23 C. Kp = (2PNH3)2/PN2(3PH2)3 D. Kp = PN2PH23/PNH32