Lanthanum oxalate decomposes when heated to lanthanum(III) oxide, CO, and CO2.
La2(C2O4)3(s) ⇄ La2CO3(s) + 3 CO(g) + 3 CO2(g)
- (a) If, at equilibrium, the total pressure in a 10.0-L flask is 0.200 atm, what is the value of Kp?
- (b) Suppose 0.100 mol of La2(C2O4)3 was originally placed in the 10.0-L flask. What quantity of La2(C2O4)3 remains unreacted at equilibrium at 373 K?
a.
Interpretation:
The value of
Concept Introduction:
Equilibrium constant in terms of pressure
The activity of solid substance will not appear in equilibrium and numerically it is considered as one.
Answer to Problem 54GQ
The value of
Explanation of Solution
To determine:
The value of
Given:
In the given reaction lanthanum oxalate and lanthanum oxide are in solid state and thus its pressure can be taken as unity. There is no role of lanthanum oxalate and lanthanum oxide in the equilibrium expression.
From the equation
Number of moles of
Mole fraction of
The value of
(b)
Interpretation:
The value of
Concept Introduction:
Equilibrium constant in terms of pressure
The activity of solid substance will not appear in equilibrium and numerically it is considered as one.
Answer to Problem 54GQ
The quantity of lanthanum oxalate remain unreacted if
Explanation of Solution
To determine:
The quantity of lanthanum oxalate remains unreacted if
Using the equation
Given that initially
For the reaction
Conclusion:
The value of
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