A couple of chemistry questions?

Posted on 2017-03-14 18:50:00 in Chemistry by DENISE

Ammonia is formed in two experiments... 
a) In #1, a 1.00L container at 727 degrees Celsius, 1.3 mol of N2 and 1.65 mol H2 are added. At equilibrium, 0.1 mol NH3 is present. Calculate equilibrium [N2] and [H2] . Find the Kc for 2NH3(g)<->N2(g)+3H2(g) 
b) In #2, another 1.00L container at 727 degrees Celsius, equilibrium is established with 8.34*10^(02) mol NH3., 1.5 mol N2 and 1.25 mol H2 present. Calculate Kc for the reaction: NH3(g)<->0.5N2(g)+3/2H2(g) 


Write the equilibrium constant expression for the reaction at each temperature... 
a) 100 degrees Celsius: H2(g)+Br2(g)<->2HBr(g) 
b) 0 degrees Celsius: H2(g)+Br2(l)<->2HBr(g) 
c) -100 degrees Celsius: H2(g)+Br2(s)<->2HBr(s) 


One mole of N2O4 is added to a 1.00 L container at equilibrium consisting of a mixture of gases, 0.2 mole NO2 and 2.00 mole N2O4 at equilibrium and 50 degrees Celsius. 
N2O4(g)<->NO2(g) 
a) Calculate the equilibrium constant value at equilibrium, before stress is applied. 
b) Use I.C.E. table. Determine the concentrations at the reestablished equilibrium. 
c) Determine the Kp value.

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