The equilibrium constant, K c , is calculated using molar concentrations. For ga

Question

The equilibrium constant, K c  , is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, K p  , is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equationK p =K c (RT) ?n    where R=0.08206 L?atm/(K?mol) , T  is the absolute temperature, and ?n  is the change in the number of moles of gas. For example, consider the reactionN 2 (g)+3H 2 (g)?2NH 3 (g)    for which ?n=2?(1+3)=?2 .

Part A

For the reaction3A(g)+3B(g)?C(g)    K c   = 95.2 at a temperature of 309 ? C  .Calculate the value of K p?.

Part B

For the reaction X(g)+3Y(g)?3Z(g) K p   = 3.59

Explanation / Answer

a)

T=309+273.15=582.15 K

Kp=Kc(RT)^-5=3.857*10^-7 atm^-5

b)Kp=Kc(RT)^(-1) where T=(273.15+353)=626.15K

=>Kc=Kp*RT

=3.59*10^-2*8.314*626.16 l/mol=186.91 l/mol

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