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
3A(g)+3B(g)âC(g)
Kc = 95.8 at a temperature of 283 âC .
Calculate the value of Kp.
Express your answer numerically.
Part B
For the reaction
X(g)+2Y(g)â3Z(g)
Kp = 2.37Ã10â2 at a temperature of 83 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 reaction
N2(g)+3H2(g)â2NH3(g)
for which În=2â(1+3)=â2.
Part A
For the reaction
3A(g)+3B(g)âC(g)
Kc = 95.8 at a temperature of 283 âC .
Calculate the value of Kp.
Express your answer numerically.
Part B
For the reaction
X(g)+2Y(g)â3Z(g)
Kp = 2.37Ã10â2 at a temperature of 83 âC .
Calculate the value of Kc.
Express your answer numerically.