Propane (C3H8) burns according to the following balanced equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Part A Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/mol .) Express the enthalpy in kilojoules to four significant figures.

Well, well, well, looks like we have a burning question here! Don't worry, I've got the perfect formula for a fiery response.

First things first, we need to find the change in enthalpy (∆H∘rxn) for this reaction. To do that, we'll use the standard enthalpies of formation. Now, the standard enthalpy of formation for gaseous propane (C3H8) is -103.9 kJ/mol, which is colder than a penguin's beak!

Now, let's take a look at the balanced equation:
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

According to this equation, we need 1 mole of propane to produce 3 moles of carbon dioxide and 4 moles of water.

So, using this equation, we can calculate the ∆H∘rxn by adding up the standard enthalpies of formation for the products and subtracting the standard enthalpies of formation of the reactants.

Let's do some math magic:
∆H∘rxn = (3 moles of CO2 × ∆H∘f of CO2) + (4 moles of H2O × ∆H∘f of H2O) - (1 mole of C3H8 × ∆H∘f of C3H8)

Plug in the values:
∆H∘rxn = (3 mol CO2 × ∆H∘f CO2) + (4 mol H2O × ∆H∘f H2O) - (1 mol C3H8 × -103.9 kJ/mol)

Now, I'm not gonna spoil the fun by giving you the exact answer, but I'll tell you this. Remember to express the enthalpy in kilojoules to four significant figures. Just keep chopping those decimal places until you reach four, and you'll get your answer.

Go on, my fiery friend, ignite those calculations and let's see the heat of this propane party!

To calculate the enthalpy change for the reaction using standard enthalpies of formation, we need to use the following formula:

ΔH∘rxn = ΣnΔH∘f(products) - ΣmΔH∘f(reactants)

where ΔH∘rxn is the enthalpy change for the reaction, ΣnΔH∘f(products) is the sum of the standard enthalpies of formation of the products, and ΣmΔH∘f(reactants) is the sum of the standard enthalpies of formation of the reactants.

Given that the standard enthalpy of formation of gaseous propane (C3H8) is -103.9 kJ/mol, and the balanced equation is:

C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g)

Let's calculate the enthalpy change now.

ΔH∘rxn = [3ΔH∘f(CO2) + 4ΔH∘f(H2O)] - [1ΔH∘f(C3H8) + 5ΔH∘f(O2)]

Since the enthalpies of formation for carbon dioxide (CO2) and water (H2O) are both zero, we can simplify the equation:

ΔH∘rxn = [3(0 kJ/mol) + 4(0 kJ/mol)] - [-103.9 kJ/mol]
= 0 kJ/mol + 0 kJ/mol + 103.9 kJ/mol
= 103.9 kJ/mol

So, the enthalpy change for the reaction is 103.9 kJ/mol.

To calculate the standard reaction enthalpy (ΔH∘rxn) using standard enthalpies of formation, you need to use the following equation:

ΔH∘rxn = Σ(nΔH∘f(products)) - Σ(mΔH∘f(reactants))

Where:
- ΔH∘rxn is the standard reaction enthalpy
- Σ(nΔH∘f(products)) is the sum of the products' standard enthalpies of formation, each multiplied by its coefficient (n)
- Σ(mΔH∘f(reactants)) is the sum of the reactants' standard enthalpies of formation, each multiplied by its coefficient (m)

In this case, the balanced equation is:
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

The given standard enthalpy of formation is -103.9 kJ/mol for gaseous propane (C3H8). Now, you need to look up the standard enthalpies of formation for carbon dioxide (CO2) and water (H2O).

- The standard enthalpy of formation of carbon dioxide (ΔH∘f(CO2)) is -393.5 kJ/mol.
- The standard enthalpy of formation of water (ΔH∘f(H2O)) is -285.8 kJ/mol.

Now, plug the values into the equation:

ΔH∘rxn = (3 × ΔH∘f(CO2)) + (4 × ΔH∘f(H2O)) - (1 × ΔH∘f(C3H8)) - (5 × 0)

ΔH∘rxn = (3 × -393.5) + (4 × -285.8) - (-103.9) - (0)

Calculating the values:

ΔH∘rxn = -1180.5 + -1143.2 + 103.9

ΔH∘rxn = -2219.8 kJ/mol

Therefore, the standard reaction enthalpy (ΔH∘rxn) for the given balanced equation is -2219.8 kJ/mol.

C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)

dHrxn = (n*dHo formation proeducts) - (n*dHo formation reactants)
You are given the dH for C3H8. You will need to look up dHo formation for H2O (g) and CO2(g) and plug them into the equation above. Post your work if you get stuck.
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