Respuesta :
Answer:
the initial amount of calcium oxide will decrease as the system moves toward equilibrium
Explanation:
The question should have this variable:
a) 655g CaCO3, 95.0g CaO, P(CO2) = 2.55atm
The reaction formula of dry ice, calcium oxide and calcium carbonate should be:
CaCO3 (s) --> CaO(s) + CO2(g)
With Kp = 1.04 at 900 degrees C
in this tank, only CO2(g) is in gaseous form. The amount of gas will determine the pressure of the tank. When the tank heated, its temperature rise and will also rise the pressure. When pressure higher than Kp, the equilibrium will shift toward side with less gas.
There is only one gas in the reaction, so Kp= P(CO2)
Since P(CO2) is 2.55 atm and its higher than Kp(1.04), the equilibrium will shift to the left. Since the reaction direction to the left, the amount of calcium carbonate will increase while carbon dioxide and calcium oxide will decrease.
The initial amount of calcium oxide will decrease because the system moves toward equilibrium
Reason for decreasing of an initial amount of calcium oxide:
In this tank, only CO2(g) should be in gaseous form. The amount of gas will measure the pressure of the tank. At the time When the tank is heated, its temperature should be increased due to this the pressure is also increased.
Since P(CO2) is 2.55 atm and it's more than Kp(1.04), the equilibrium should shift to the left. The reaction shifted to the left, the amount of calcium carbonate will increase while on the other hand, carbon dioxide and calcium oxide will decrease.
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