What volume (mL)of sulfur dioxide can be produced by the complete reaction of 3.82 g of calcium sulfite with excess HCl (aq),when the final SO₂ pressure is 827 torr at 44.0 °C? A)7.60 × 10² B)1.39 × 10^-4 C)1.00 × 10^-3 D)0.106 E)5.78 × 10²

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To solve this problem, we first need to understand the chemical reaction involved and then apply the ideal gas law. The reaction between calcium sulfite (CaSO3) and hydrochloric acid (HCl) produces calcium chloride (CaCl2), water (H2O), and sulfur dioxide (SO2) gas. The balanced chemical equation is:$$ \text{CaSO}_3(s) + 2\text{HCl}(aq) \rightarrow \text{CaCl}_2(aq) + \text{H}_2\text{O}(l) + \text{SO}_2(g) $$Given:- Mass of CaSO3 = 3.82 g- Final pressure = 827 torr (1 atm = 760 torr, so pressure in atm = 827 / 760)- Temperature = 44.0 °C (Temperature in Kelvin = 44.0 + 273.15)First, we calculate the moles of CaSO3 using its molar mass (CaSO3 = 40.08 (Ca) + 32.06 (S) + 3*16.00 (O) = 120.14 g/mol):$$ \text{Moles of CaSO}_3 = \frac{3.82 \text{ g}}{120.14 \text{ g/mol}} $$Since the reaction is a 1:1 mole ratio between CaSO3 and SO2, the moles of SO2 produced will be equal to the moles of CaSO3.Next, we use the ideal gas law to find the volume of SO2 produced:$$ PV = nRT $$Where:- $P$ = pressure in atm- $V$ = volume in liters (to convert to mL, we'll multiply by 1000)- $n$ = moles of SO2- $R$ = ideal gas constant (0.0821 L·atm/(mol·K))- $T$ = temperature in KelvinRearranging the ideal gas law to solve for $V$ and substituting the values (including converting pressure to atm and temperature to Kelvin), we can calculate the volume of SO2 produced in liters and then convert it to mL. The calculation will show that the correct answer is the one that corresponds to the volume of SO2 gas produced under the given conditions, which is choice A.

What Volume (ML)of Sulfur Dioxide Can Be Produced by the Complete