For the reaction O2 (g) + 2F2 (g) ⇌ 2OF2 (g), Kp = 41.0. If the...
For the reaction O2 (g) + 2F2 (g) ⇌ 2OF2 (g), Kp = 41.0. If the partial pressure of O2 is 0.116 atm and the partial pressure of F2 is 0.0461 atm at equilibrium, what is the pressure of OF2 at equilibrium?
Homework Answers
The reaction 2OF2(g) 2F2(g) + O2(g) has an equilibrium constant Kp (in terms of pressures) at...
The reaction 2OF2(g) 2F2(g) + O2(g) has an equilibrium constant Kp (in terms of pressures) at 25 °C of 6.19×10-4. Calculate the concentration of F2 that will be present at 25 °C in equilibrium with OF2 (at a concentration of 3.46×10-2 mol L-1) and O2 (at a concentration of 1.96×10-3 mol L-1). [F2] = mol L-1
Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies:...
Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies: F2= 159 kJ/mol; O2 (double bond) = 498 kJ/mol Calculate the bond strength of the O-F bonds in OF2.
At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP...
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) = .
The equilibrium constant, Kp, for the following reaction is 2.74 at 1.15x103K. 2803(g) 22502(g) + O2(g)...
The equilibrium constant, Kp, for the following reaction is 2.74 at 1.15x103K. 2803(g) 22502(g) + O2(g) + If an equilibrium mixture of the three gases in a 10.9 L container at 1.15*10²K contains SO3 at a pressure of 1.77 atm and SO2 at a pressure of 0.926 atm, the equilibrium partial pressure of O2 is atm.
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to...
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to form SO3 is 0.365 at 1.15×103 K: SO2(g) + O2(g) = 2SO3(g) A sample of SO3 is introduced into an evacuated container at 298 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.867 atm. Calculate the equilibrium partial pressures of SO2 and O2 in the container. PSO2 = PO2 =
The equilibrium constant Kp of the reaction below is 7.69 at 830°C. 2S0,(g) 2S0,(g) +0,(g) 1st...
The equilibrium constant Kp of the reaction below is 7.69 at 830°C. 2S0,(g) 2S0,(g) +0,(g) 1st attempt ad See Periodic Table See Hint If a vessel at this temperature initially contains pure SO, and if the partial pressure partial pressure of O2 in the flask at equilibrium? of SO3 at equilibrium is 0.100 atm, what is the atm
At 900 K the following reaction has Kp=0.345: 2SO2(g)+O2(g)???2SO3(g) In an equilibrium mixture the partial pressures...
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?
At 7075 °C the equilibrium constant for the reaction: 2 NO(g) N2(g) + 02(9) is Kp...
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)
At 400K, the equilibrium constant for the reaction Br2(g) + Cl2(g) ⇌ 2BrCl(g) is KP =...
At 400K, the equilibrium constant for the reaction Br2(g) + Cl2(g) ⇌ 2BrCl(g) is KP = 7.0. A closed vessel at 400K is charged with 1.00 atm of Br2(g), 1.00 atm of Cl2(g), and 2.00 atm of BrCl(g). Use Q to determine which of the statements below is true. A. The equilibrium partial pressure of BrCl(g) will be less than 2.00 atm B. The reaction will go to completion since there are equal amounts of Br2 and Cl2 C. At...
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?
The equilibrium constant, Kp, for the following reaction is 2.74 at 1.15x103K. 2803(g) 22502(g) + O2(g) + If an equilibrium mixture of the three gases in a 10.9 L container at 1.15*10²K contains SO3 at a pressure of 1.77 atm and SO2 at a pressure of 0.926 atm, the equilibrium partial pressure of O2 is atm.
The equilibrium constant Kp of the reaction below is 7.69 at 830°C. 2S0,(g) 2S0,(g) +0,(g) 1st attempt ad See Periodic Table See Hint If a vessel at this temperature initially contains pure SO, and if the partial pressure partial pressure of O2 in the flask at equilibrium? of SO3 at equilibrium is 0.100 atm, what is the 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)
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