Data: SO2(g) + ¨öO2(g) ¡æ SO3 (g) ¥ÄH = -99.1 kJ Given the above data, calculate the enthalpy change ¥ÄH when 89.6 g of SO2 is converted to SO3.

You need to work on these symbols. I assume the reaction is

2SO2 + O2 ==> 2SO3 DH = -99.1 kJ.

Then -99.1 kJ x (89.4/128) = ?

To calculate the enthalpy change (ΔH) when 89.6 g of SO2 is converted to SO3, we can use the concept of stoichiometry and the given data.

1. Calculate the moles of SO2:
Number of moles = mass / molar mass

The molar mass of SO2 is 64.07 g/mol.
Number of moles of SO2 = 89.6 g / 64.07 g/mol

2. Balance the chemical equation and determine the mole ratio between SO2 and SO3:
2SO2 + O2 → 2SO3

From the balanced equation, we can see that 2 moles of SO2 are reacting to form 2 moles of SO3. So, the mole ratio is 2:2 or 1:1.

3. Calculate the heat released or absorbed:
ΔH = (ΔH of the reaction) * (moles of SO2)

Given: ΔH = -99.1 kJ
moles of SO2 = (89.6 g / 64.07 g/mol) = 1.398 mol

ΔH = -99.1 kJ/mol * 1.398 mol

4. Calculate the enthalpy change:
ΔH = -99.1 kJ/mol * 1.398 mol = -138.46 kJ

Therefore, the enthalpy change (ΔH) when 89.6 g of SO2 is converted to SO3 is -138.46 kJ.

To calculate the enthalpy change (ΔH) when 89.6 g of SO2 is converted to SO3, we can use the concept of stoichiometry and the given data for the reaction.

First, we need to determine the moles of SO2 used in the reaction. We can use the molar mass of SO2 to convert grams to moles:

Molar mass of SO2 = 32.06 g/mol

Moles of SO2 = 89.6 g / (32.06 g/mol) = 2.795 mol

Next, we use the stoichiometric coefficients from the balanced chemical equation to relate the moles of SO2 to the moles of SO3.

From the balanced equation:
2 moles of SO2 react to produce 2 moles of SO3.

Since the stoichiometric coefficients are 1:1, the number of moles of SO3 produced will also be 2.795 mol.

Now, we can calculate the enthalpy change (ΔH) using the given data:

Given: ΔH = -99.1 kJ

To calculate the enthalpy change for the given amount of SO2, we can use the following equation:

ΔH = (ΔH per mole) × (moles of SO2 reacted)

ΔH = (-99.1 kJ/mol) × (2.795 mol)

ΔH = -276.7 kJ

Therefore, the enthalpy change (ΔH) when 89.6 g of SO2 is converted to SO3 is -276.7 kJ.