Pressure-Based versus Concentration-Based Equilibrium Constants The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)În where R=0.08206 Lâ atm/(Kâ mol), T is the absolute temperature, and În is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)â2NH3(g) for which În=2â(1+3)=â2.
Part A
For the reaction 2A(g)+3B(g)âC(g) Kc = 64.8 at a temperature of 107 âC . Calculate the value of Kp. Express your answer numerically.
Part Part B
For the reaction X(g)+2Y(g)â3Z(g) Kp = 2.77Ã10â2 at a temperature of 337 âC . Calculate the value of Kc. Express your answer numerically.
Pressure-Based versus Concentration-Based Equilibrium Constants The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)În where R=0.08206 Lâ atm/(Kâ mol), T is the absolute temperature, and În is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)â2NH3(g) for which În=2â(1+3)=â2.
Part A
For the reaction 2A(g)+3B(g)âC(g) Kc = 64.8 at a temperature of 107 âC . Calculate the value of Kp. Express your answer numerically.
Part Part B
For the reaction X(g)+2Y(g)â3Z(g) Kp = 2.77Ã10â2 at a temperature of 337 âC . Calculate the value of Kc. Express your answer numerically.
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