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
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The reaction 2OF2(g) 2F2(g) + O2(g) has an equilibrium constant
Kp (in terms of pressures) at...
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?
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 =
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.
Write the expression for the equilibrium constant Kp for the following reaction. Enclose pressures in parentheses...
Write the expression for the equilibrium constant Kp for the following reaction. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3 )2 as (P NH3)2 . If either the numerator or denominator is 1, please enter 1 2 F2(g) + O2(g) ↔ 2 OF2(g)
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400...
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2and O2to form SO3is...
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2and O2to form SO3is 0.365 at 1.15×103K: 2 SO2( g ) + O2( g ) --> 2 SO3( g ) A sample of SO3is introduced into an evacuated container at 1150 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.879atm. Calculate the equilibrium partial pressures of SO2and O2in the container.
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 in terms of pressures for the reduction of tungsten(IV) oxide to tungsten at...
The equilibrium constant in terms of pressures for the reduction of tungsten(IV) oxide to tungsten at 25 °C is Kp = 3.82×10-4, corresponding to the reaction WO2(s) + 2CO(g) <--> W(s) + 2CO2(g) If the total pressure of an equilibrium system at 25 °C is 2.82 atm, calculate the partial pressures of CO(g) and CO2(g). PCO = _____atm PCO2 = ______atm
The equilibrium constant in terms of pressures for the reaction SnO2(s) + 2CO(g) Sn(s) + 2CO2(g)...
The equilibrium constant in terms of pressures for the reaction SnO2(s) + 2CO(g) Sn(s) + 2CO2(g) at 25 °C is Kp = 0.124. Calculate the reaction quotient Q for each of the following conditions and determine whether solid Sn is consumed or produced as the reaction comes to equilibrium. (A) PCO = 0.249 atm; PCO2 = 0.108 atm; Sn is a) consumed b) produced (B) PCO = 6.34×10-2 atm; PCO2 = 0.174 atm; Sn is a)consumed b) produced
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?
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...
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