Consider the following reaction occuring at 298.15 K and 1 bar: CaCO3 (s)----^ C
ID: 708682 • Letter: C
Question
Consider the following reaction occuring at 298.15 K and 1 bar:
CaCO3 (s)----^ CaO (s) + CO2 (g)
The Solids do not form a solution and exist as pure, disinct phases. Assume carbon dioxide behaves as an ideal gas.
A. Write down the appropriate expressions for the chemical potentials of the three species which participate in this reaction. Clearly indicate what is the reference state for each
B.Calculate the vapor pressure of carbon dioxide which exists in equilibrium with the two solid phases
C. How would increasing the total pressure to 2 atm change your result for part b
D. How would increasing the tempreature to 100C change your answer in part b
E. Suppose that the carbon dioxide vapor pressure in the ambient remains fixed at
5 x 10 -22 bar. How much CaO (s) would be present at equilibrium at 298.15K if we start with1 mole of CaCO3 (s) and 0 mole of CaO (s)? (Remember: solids assumed remain pure!)
F. How does you answer to part (a) change if it were possible for the solids to form a solid solution?
G. How does your answer to part (e) change if it were possible for the solids to form a solid solution?
Explanation / Answer
A. Write down the appropriate expressions for the chemical potentials of the three species which participate in this reaction. Clearly indicate what is the reference state for each
reference state is Hydrogen caloeml electrode
B.Calculate the vapor pressure of carbon dioxide which exists in equilibrium with the two solid phases
here the total pressure is 1 bar so vapour pressure of the reaction is 1 bar CO2
C. How would increasing the total pressure to 2 atm change your result for part b
increase in the pressure shift the equillibrium direction toward the less molecule direction that is reverse direction ...so vapour the CO2 will decreases3
D. How would increasing the tempreature to 100C change your answer in part b
this is endothermic reaction so reaction proceeds toward forward direction and favourable of formation CO2
and increase in vapour pressure
E. Suppose that the carbon dioxide vapor pressure in the ambient remains fixed at
5 x 10 -22 bar. How much CaO (s) would be present at equilibrium at 298.15K if we start with1 mole of CaCO3 (s) and 0 mole of CaO (s)? (Remember: solids assumed remain pure!)
the value of CaO will be 0.5 mole
F. How does you answer to part (a) change if it were possible for the solids to form a solid solution?
CaCO3 (s)----^ CaO (s) + CO2 (g) cao forms CaOH2 and this will also involve in the reaction