Answer:
The partial pressure of CO₂ will decrease.
Explanation:
The reaction:
2CO (g) + O₂ (g) ⇄ 2CO₂ (g) has a ΔH = –566 kJ/mol. As ΔH<0, the reaction is exothermic.
Le Chatelier's principle says that if a system in chemical equilibrium is subjected to a disturbance it tends to change in a way that opposes this disturbance.
In this case, with increasing of the temperature, the system will produce less heat, doing the equilibrium shifts to the left.
Thus, the partial pressure of both CO and O₂ will increase. And<em> partial pressure of CO₂ will decrease.</em>
I hope it helps!
Answer:
2.73 is the equilibrium constant for the dissociation of 
gas at 840 degree Celsius.
Explanation:
Initial
0.600 atm 0
Equilibrium
(0.600 atm - p) 2p
Total pressure at equilibrium = P = 0.984 atm
P= 0.600 atm - p)+2p=0.984 atm
p = 0.384 atm
Partial pressure of the gas , 
= (0.600 atm - 0.384 atm)=0.216 atm
Partial pressure of the 
gas, 
= 2(0.384 atm)=0.768 atm
2.73 is the equilibrium constant for the dissociation of gas at 840 degree Celsius.
Ability to move up through thin tunes because a physical property is something you can observe about the matter. Out of all of them this one does not fit.
The answer would be D. because when an acid and base mix the start to cancel each other out causing it to neutralize
