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11 Nov 2019
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)+2B(g)âC(g)
Kc = 84.2 at a temperature of 163 âC .
Calculate the value of Kp. Express your answer numerically.
View Available Hint(s)
Kp = 1.68â¢10â51.68{\cdot}10^{-5}
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Incorrect; Try Again; 5 attempts remaining
Part B
For the reaction X(g)+3Y(g)â3Z(g)
Kp = 1.11Ã10â2 at a temperature of 153 âC .
Calculate the value of Kc. Express your answer numerically.
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 reactionN2(g)+3H2(g)â2NH3(g) for which În=2â(1+3)=â2. | Part A For the reaction2A(g)+2B(g)âC(g) Kc = 84.2 at a temperature of 163 âC . Calculate the value of Kp.Express your answer numerically. View Available Hint(s)
SubmitPrevious Answers Incorrect; Try Again; 5 attempts remaining Part B For the reactionX(g)+3Y(g)â3Z(g) Kp = 1.11Ã10â2 at a temperature of 153 âC . Calculate the value of Kc.Express your answer numerically. |
Irving HeathcoteLv2
12 Jul 2019