For the equilibrium system: CO 2 ( g ) + H 2 ( g ) <----> CO( g ) + H 2 O( g ) D
ID: 872217 • Letter: F
Question
For the equilibrium system:
CO2(g) + H2(g) <----> CO(g) + H2O(g) DELTA H = +42 kJ/mol
K equals 1.6 at 1260 K. If 0.15 mol each of CO2, H2, CO, and H2O (all at 1260 K) were placed in a 1.0-L thermally insulated vessel that was also at 1260 K, then as the system came to equilibrium:
A)
The temperature would increase and the mass of CO2 would increase.
B)
The temperature would remain constant and the mass of CO2 would increase.
C)
The temperature would decrease and the mass of CO2 would decrease.
D)
The temperature would decrease and the mass of CO2 would increase.
E)
The temperature would increase and the mass of CO2 would decrease.
PLEASE EXPLAIN WHY OR SHOW WORK
For the equilibrium system:
CO2(g) + H2(g) <----> CO(g) + H2O(g) DELTA H = +42 kJ/mol
K equals 1.6 at 1260 K. If 0.15 mol each of CO2, H2, CO, and H2O (all at 1260 K) were placed in a 1.0-L thermally insulated vessel that was also at 1260 K, then as the system came to equilibrium:
A)
The temperature would increase and the mass of CO2 would increase.
B)
The temperature would remain constant and the mass of CO2 would increase.
C)
The temperature would decrease and the mass of CO2 would decrease.
D)
The temperature would decrease and the mass of CO2 would increase.
E)
The temperature would increase and the mass of CO2 would decrease.
Explanation / Answer
The right Answer would be option E and let me tell you why:
The value of Delta H means that this reaction is endothermic, so in order for this system to reach the equilibrium, it needs heat, to absorb heat so the system reach the equilibrium, and hence, the temperature increase. Now the value of K of 1.6 means that the innitial concentrations of each species are higher than 0.15. If we do the calculations under this conditions (with 0.15 for each species) the value of K would decrease (around 1) and ergo, the mass of CO2 decrease as well.
Hope this help you.