Question

Sulfur dioxide, so,(g), can react with oxygen to produce sulfur trioxide, so(g), by the reaction 2502(8) 02(8) -> 2503(8) the standard enthalpies of formation for so, (g) and so,(g) are ah; so,(g) =- 296.8 kj/mol ah; so,(g) =-395.7 kj/mol calculate the amount of energy in the form of heat that is produced when a volume of 4.46 l of so,(g) is converted to 4.46 l of so (g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °c. assume ideal gas behavior.

Answer 1

To calculate the heat produced when 4.46 L of SO2 is converted to SO3, we first use the ideal gas law to determine the moles of SO2, then apply the reaction's stoichiometry along with the given enthalpy changes to find the heat energy released.

Step-by-step explanation:

The student is asking how to calculate the amount of heat energy produced when converting 4.46 L of sulfur dioxide, SO2(g), to sulfur trioxide, SO3(g), at a constant pressure and temperature. First, we need to use the ideal gas law to find the number of moles of SO2 that corresponds to a volume of 4.46 L under the given conditions (1.00 bar and 25.0 °C). Then, we can use the reaction's stoichiometry and the given standard enthalpy of formation values to find the heat released during the reaction.

Assuming ideal gas behavior, we know that 1 mole of gas occupies 22.711 L at STP (1 bar pressure and 0°C). Since the temperature here is 25.0 °C, we can adjust using the ideal gas law PV = nRT to account for the non-STP conditions.

After calculating the moles of SO2, we use the reaction stoichiometry to find the enthalpy change for the given volume of SO2. The enthalpy change (ΔH) for the entire reaction is -197.8 kJ as per the reaction:

2SO2(g) + O2(g) → 2SO3(g), ΔH° = -197.8 kJ

Finally, by using the proportion of moles we've calculated to the stoichiometric coefficients in the reaction, we could determine the amount of heat energy released for the 4.46 L volume of SO2.