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For an ideal gas, molarity is directly proportional to pressure M = P RT therefore K c is directly related to K c by the equation: K p = K c (RT)  n.

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Presentation on theme: "For an ideal gas, molarity is directly proportional to pressure M = P RT therefore K c is directly related to K c by the equation: K p = K c (RT)  n."— Presentation transcript:

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2 For an ideal gas, molarity is directly proportional to pressure M = P RT therefore K c is directly related to K c by the equation: K p = K c (RT)  n where  n is the total number of product moles minus the total number of reactant moles

3 Hydrogen and carbon dioxide gas react to form water vapor and carbon monoxide at high temperatures. At 420  C, the equilibrium constant, K c is equal to 0.10. What would be the equilibrium constant, K p, if the concentration of the gases were measured in atm? K p = K c (RT)  n where  n is the total number of product moles minus the total number of reactant moles H 2 + CO 2  H 2 O + CO  n = ( 1 + 1 ) - ( 1 + 1 ) = 0 K p = K c [(0.0821 L atm/mol K)(693)] 0 K p = K c = 0.10 If the moles of products equals to moles of reactants, then K p = K c

4 Hydrogen and nitrogen gases react to form ammonia. At 300  C, the equilibrium constant, K c is equal to 9.60. What would be the equilibrium constant, K p, if the concentration of the gases were measured in atm? K p = K c (RT)  n where  n is the total number of product moles minus the total number of reactant moles 3 H 2 + N 2  2 NH 3  n = (2) - ( 3 + 1 ) = -2 K p = 9.60 [(0.0821 L atm/mol K)(573)] -2 K p = 4.34 x 10 -3


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