Consider the reaction
N2(g) + O2(g) ⇌ 2NO(g)
If the equilibrium partial pressures of N2, O2, and NO are 0.20, 0.35, and 0.030 atm, respectively, at 2200° C, what is KP?
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) If the equilibrium partial pressures of N2, O2,...
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.26, 0.36, and 0.030 atm, respectively, at 2200°C, what is KP?
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?
) Consider the following reaction a 25 oC: N2(g) + 2 O2(g) D N2O4(g) An equilibrium mixture contains O2(g) and N2O4(g) at partial pressures of 2.5 atm and 4.5 atm, respectively. Determine the equilibrium partial pressure of N2 in the mixture.
At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 7.16. If the initial pressure of NO is 0.00663 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) = . p(N2) = . p(O2) = .
At 900 K the following reaction has Kp=0.345: 2SO2(g)+O2(g)???2SO3(g) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.150atm and 0.465atm , respectively. What is the equilibrium partial pressure of SO3 in the mixture?
Consider the reaction N2(g) + O2(g)2NO(g) Use the standard thermodynamic data in the tables linked above. Calculate G for this reaction at 298.15K if the pressure of NO(g) is reduced to 20.24 mm Hg, while the pressures of N2(g) and O2(g) remain at 1 atm.
At 7075 °C the equilibrium constant for the reaction: 2 NO(g) N2(g) + 02(9) is Kp 0.983. If the initial pressure of NO is 0.00863 atm, what are the equilibrium partial pressures of NO, N2, and O2? P(NO) P(N2) p(02)
Be sure to answer all parts. At 430°C, the equilibrium constant (Kp) for the reaction 2NO(g)+O2()s 2NO2(g) is 1.5 x 105. In one experiment, the initial pressures of NO, O2, and NO are 6.3 x 103 atm, 1.9 x 10-2 atm, and 0.18 atm, respectively. Calculate Op and predict the direction that the net reaction will shift to reach equilibrium. What is Qp for the experiment? 4.29 In which direction will the system proceed to reach equilibrium? The reaction will...
Consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and Bfor each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. A.)Kp= 2.0 B.) Kp= 1.6×10−4 C.)Kp= 1.4×105
Consider the reaction: 2 HI (g) ⇌ H₂ (g) + I₂ (g) At equilibrium, the partial pressure of HI is 1.9 atm and the partial pressures of H₂ and I₂ are 7.9 and 2.3 respectively. What is Kp for this equilibrium?