Download presentation

Presentation is loading. Please wait.

Published byAlisa Bissey Modified over 2 years ago

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

Similar presentations

© 2017 SlidePlayer.com Inc.

All rights reserved.

Ads by Google