Sulfur dioxide SO2 is released in the combustion of coal. Scrubbers use aqueous slurries of Ca(OH)2 to remove the sulfur dioxide from the flue gases. Write a balanced equation for this reaction and calculate delta So at 298 K (So for CaSO3(s) = 101.4 J/{mol*K}).
include the states of all reactant and products in the equation..
thanks.
Ca(OH)2(aq) + SO2(g) ==> CaSO3(s) + H2O(l)
You will need So for each component, then
dSo rxn = (n*dSo products) - (n*dSo reactants)
The balanced equation for the reaction between sulfur dioxide (SO2) and aqueous slurries of calcium hydroxide (Ca(OH)2) to form calcium sulfite (CaSO3) is:
SO2(g) + Ca(OH)2(aq) → CaSO3(s) + H2O(l)
To calculate ΔS° at 298 K, we need to consider the change in entropy for the reaction.
The standard entropy change, ΔS°, can be calculated using the formula:
ΔS° = ΣnS°(products) - ΣmS°(reactants)
where n is the stoichiometric coefficient of the products and m is the stoichiometric coefficient of the reactants.
In this case, the stoichiometric coefficients are:
SO2(g): 1
Ca(OH)2(aq): 1
CaSO3(s): 1
H2O(l): 1
The standard entropy values (ΔS°) can be found in a table of thermodynamic data. The values are typically given in J/(mol·K). For this calculation, we have:
ΔS° = (1 * 101.4 J/(mol·K)) - (1 * 0) - (1 * 0) - (1 * 69.9 J/(mol·K))
= 101.4 J/(mol·K) - 0 - 0 - 69.9 J/(mol·K)
= 31.5 J/(mol·K)
Therefore, the ΔS° for this reaction at 298 K is 31.5 J/(mol·K).
To write a balanced equation for the reaction between sulfur dioxide (SO2) and calcium hydroxide (Ca(OH)2) to form calcium sulfite (CaSO3), we need to consider the chemical formulas and their respective states.
The balanced equation is as follows:
SO2(g) + Ca(OH)2(aq) → CaSO3(s) + H2O(l)
Note that SO2 is a gas, Ca(OH)2 is an aqueous solution, CaSO3 is a solid precipitate, and H2O is liquid water.
To calculate ΔSo (the standard entropy change) at 298 K for the formation of CaSO3(s), we can use the equation:
ΔSo = ΣnSo(products) - ΣnSo(reactants)
Here, ΣnSo represents the sum of the standard molar entropies of the products and reactants, respectively.
For the reaction:
ΔSo = (1 mol x So(CaSO3(s))) - (1 mol x So(SO2(g)) + 1 mol x So(Ca(OH)2(aq)) + 1 mol x So(H2O(l)))
Using the given value for So(CaSO3(s)) = 101.4 J/(mol·K), we can substitute it into the equation:
ΔSo = 101.4 J/(mol·K) - ΣnSo(SO2(g)) - ΣnSo(Ca(OH)2(aq)) - ΣnSo(H2O(l))
To obtain the values of ΣnSo for SO2(g), Ca(OH)2(aq), and H2O(l), you can refer to a thermodynamic data source or a chemistry textbook. These values represent the standard molar entropies for each component under standard conditions.