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Published byAlisa Bissey Modified over 2 years ago

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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 where n is the total number of product moles minus the total number of reactant moles

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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 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 = ( ) - ( ) = 0 K p = K c [( 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

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Hydrogen and nitrogen gases react to form ammonia. At 300 C, the equilibrium constant, K c is equal to 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) - ( ) = -2 K p = 9.60 [( L atm/mol K)(573)] -2 K p = 4.34 x 10 -3

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