Data: SO2(g)+ 1/2O2(gas)forms SO3(g)Delta H = -99.1 kJ.

Given the above data, calculate the enthalpy change when 89.6 g of SO2 is converted to SO3.
Is this a grams to moles conversion or what? I can't find any examples of this type of calculation.

Ah, the enchanting world of chemical reactions and enthalpy changes! It seems you're dealing with a grams to moles conversion, my inquisitive friend. Let's unravel this puzzling scenario step by step, shall we?

First, we need to convert the given mass of SO2 (89.6 g) into moles. To achieve this, we employ everyone's favorite number, the molar mass of SO2. Its molar mass is 64.06 g/mol, since sulfur's atomic mass is approximately 32.07 g/mol and oxygen's atomic mass is roughly 16.00 g/mol.

So, using the formula:

moles = mass / molar mass,

we find:

moles of SO2 = 89.6 g / 64.06 g/mol.

Next, we investigate the stoichiometry (the coefficient of SO2) in the balanced chemical equation:

SO2(g) + 1/2O2(gas) ➡️ SO3(g).

From the equation, we deduce that the enthalpy change (-99.1 kJ) is associated with the formation of 1 mole of SO3. Thus, our ultimate aim is to discover the enthalpy change for the aforementioned moles of SO2.

To achieve this, we employ the concept of ratio, my hilarious friend! We use the ratio from the balanced equation to link the number of moles of SO2 to the enthalpy change. For every 1 mole of SO2, there is an enthalpy change of -99.1 kJ.

Finally, we put all the pieces together and calculate the enthalpy change for the given mass of SO2:

enthalpy change = moles of SO2 * enthalpy change per mole.

And voila! Take a leap of faith, plug in the numbers, and get a delightful answer to your enthalpy conundrum.

To calculate the enthalpy change when 89.6 g of SO2 is converted to SO3, we need to follow a few steps. This problem involves both stoichiometry and energy calculations.

1. First, we convert the given mass of SO2 into moles. To do this, we need to know the molar mass of SO2. The molar mass of sulfur (S) is 32.07 g/mol, and the molar mass of oxygen (O) is 16.00 g/mol. Therefore, the molar mass of SO2 is:

32.07 g/mol + 2 * 16.00 g/mol = 64.07 g/mol

To convert grams to moles, we divide the mass by the molar mass:

89.6 g SO2 / 64.07 g/mol = 1.398 mol SO2

2. The balanced chemical equation shows that the conversion of SO2 to SO3 involves a 1:1 stoichiometric ratio. This means that for every 1 mole of SO2, 1 mole of SO3 is produced. Therefore, the number of moles of SO3 produced is also 1.398 mol.

3. The given enthalpy change is -99.1 kJ for the reaction as written. Because this value is for the formation of 1 mole of SO3, we can directly assign this enthalpy change to the conversion of 1.398 mol of SO2 to SO3.

To calculate the enthalpy change for the conversion of 1.398 mol of SO2 to SO3, we multiply the number of moles by the given enthalpy change:

-99.1 kJ/mol * 1.398 mol = -138.5 kJ

Therefore, the enthalpy change when 89.6 g of SO2 is converted to SO3 is -138.5 kJ.

To calculate the enthalpy change when a given amount of substance is converted to another, you need to use the concept of stoichiometry and the given molar enthalpy change (in this case, ΔH = -99.1 kJ).

Step 1: Convert the given amount of substance (89.6 g) to moles.

To do this, you need to know the molar mass of SO2. The molar mass of SO2 is 64.06 g/mol.

Number of moles of SO2 = Mass of SO2 / Molar mass of SO2
Number of moles of SO2 = 89.6 g / 64.06 g/mol

Step 2: Use the balanced chemical equation to determine the stoichiometric ratios between SO2 and SO3.

From the balanced chemical equation:
SO2(g) + 1/2O2(g) → SO3(g)

The stoichiometric ratio between SO2 and SO3 is 1:1. This means that for every 1 mole of SO2, 1 mole of SO3 is formed.

Step 3: Calculate the enthalpy change using the stoichiometric ratio and the given molar enthalpy change.

ΔH = -99.1 kJ/mol (as given)

Since the stoichiometric ratio is 1:1, the enthalpy change for the given amount of substance is the same as the molar enthalpy change.

Enthalpy change = ΔH × Number of moles of SO2
Enthalpy change = -99.1 kJ/mol × Number of moles of SO2

Step 4: Substitute the value you calculated in Step 1 into the equation.

Enthalpy change = -99.1 kJ/mol × (89.6 g / 64.06 g/mol)

Calculate this expression to find the enthalpy change.

I think the answer to your question is yes although I usually don't do them exactly that way.

I rearrange the question something like this.
Calculate enthalpy change when 89.6 g SO2 is converted to SO3 given that the reaction as written releases 99.1 kJ for 64.0 g SO2.
Then -99.1 kJ x (89.6/64.0) = -?? kJ.