Part A For the reaction 2CH4( g )C2H2( g )+3H2( g ) K c =0.155 mol2 L2 at 1732 C
ID: 904793 • Letter: P
Question
Part A
For the reaction
2CH4(g)C2H2(g)+3H2(g)
Kc=0.155 mol2 L2 at 1732 C . What is Kp for the reaction at this temperature?
Enter your answer numerically.
Part B
What is the unitless thermodynamic equilibrium constant K for the reaction in part A?
Express your answer numerically.
Part C
For the reaction
N2(g)+3H2(g)2NH3(g)
Kp=3.05×103 bar2 at 258 C . What is Kc for the reaction at this temperature?
Enter your answer numerically.
Part D
What is the unitless thermodynamic equilibrium constant K for the reaction in part C?
Express your answer numerically.
Explanation / Answer
A)
delta n = number of gas in product - number of gas in reactant
=3+1 - 2
= 2
T=1732 oC = (1732+273) K=2005 K
use:
Kp = Kc * (RT)^(delta n)
= 0.155 * (0.0821*2005)^2
=4200
Answer: 4200 atm^2
B)
I dont understant this question
There is no unitless thermodynamic equilibrium constant
C)
delta n = number of gas in product - number of gas in reactant
=2 - (1 + 3)
= -2
T=258 oC = (258+273) K=531 K
R=8.314*10^-2 L bar k-1 mol-1
use:
Kp = Kc * (RT)^(delta n)
3.05*10^-3 = Kc* (8.314*10^-2*531)^-2
Kc = 4.59*10^-4 L^2 mol-2
D)
I dont understant this question
There is no unitless thermodynamic equilibrium constant