a. CaCO3 decreases
b. CaCO3 increases
<h3>Further explanation
</h3>
The equilibrium constant is based on the concentration (Kc) in a reaction
pA + qB -----> mC + nD
To find out the reaction reaches equilibrium and the direction of the reaction, the value of the reaction quotient, Qc
-
Qc = Kc, the reaction equilibrium ---> reactant ⇌ product
- Qc <Kc, reaction from left to right (product) until it reaches equilibrium (Qc = Kc) ---> reactant → product
- Qc> Kc, the reaction from right to left (reactant) until it reaches equilibrium (Qc = Kc). If Qc> Kc, reactant ← product
equilibrium constants of heterogeneous reactions (more than 1 phase), liquid (L = liquid) and solid (S = solid) phases are ignored and not counted, only gas (G = gas) and solution (Aq = aqueous) phases so that the price of Kc for the reaction of CaCO₃ (s) → - → CaO (s) + CO₂ (g) is only based on concentration [CO₂]
Kc = [CO₂] = 0.0108
Similarly, the determination of Qc is also based on [CO₂]
We determine the mole and concentration of CO₂
molar mass of CO₂ = 44, and a volume of 10 L
a) 15.0 g CaCO₃, 15.0 g CaO, and 4.25g CO₂
4.25 g CO₂ (ignore masses of CaCO₃ and CaO)
mole CO₂= mass: molar mass
mole of CO₂ = 4.25: 44 = 0.0965
concentration = 0.0965: 10 = 0.00965 M
Because Qc = [CO₂] = 0.00965 and Qc <Kc, the reaction is more to the right (product), so CaCO₃ decreases
b) 2.50g CaCO₃, 25.0 g CaO, and 5.66 g CO₂
5.66 g CO₂
mole CO₂ = mass: molar mass
mole of CO₂ = 5.66: 44 = 0.1286
concentration = 0.1286: 10 = 0.01286 M
Because Qc = [CO₂] = 0.01286 and Qc> Kc, the reaction is more towards the left (reactant), so CaCO₃ increases
<h3>Learn more
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