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🔥Unit 6

5 min read•june 1, 2021

Anika P

Dalia Savy

Dylan Black

A **pathway** is the route that a process takes. Typically, pathway dependency/independency is applied to **functions. **Essentially, if the result of something depends on the order in which you did it, it is **pathway dependent** and if it is not, it is **pathway independent**.

For example, the change in elevation of a mountain climber is **pathway independent🧗**. You could walk in a straight line or a zig-zagged line up the mountain but regardless, you both end up at the top of the mountain⛰️.

A **state function** is a property whose value does not depend on the path taken to reach that specific value. In basic terms, state functions are **pathway independent**, just like our elevation example.

A **pathway dependent** function is called a path function, though we'll only be dealing with state functions.

Hess's Law is stated as simply: **enthalpy is a state function**. No matter what way you go from reactants to products, you will end up with the same enthalpy of reaction for the reaction. This means that if we know the enthalpy of formation for different reactions and you can manipulate them to get a single reaction, and you can find the enthalpy of reaction of that single reaction. It's like magic✨, and it's kinda fun!

- When a reaction is reversed, the enthalpy change stays constant in magnitude but becomes reversed in mathematical sign (Flipping the reaction flips the sign on ΔH🔁).
- If an equation is multiplied by n, ΔH has to also be multiplied✖️ by n.
- When two (or more) reactions are added to obtain an overall reaction➕, the individual enthalpy changes of each reaction are added to obtain the net change of enthalpy of the overall reaction ΔH).

Our general strategy is going to be manipulating these three reactions and then adding them together to form the overall reaction. This is using Hess's Law to find the enthalpy.

Thought Process

When I approach a Hess's Law question, I always find the reactants and products in the given thermochemical equations. This is what I would note🤔:

- C(s) is on the reactants side like it is supposed to be, but there should be 2 atoms of carbon so we have to manipulate the second equation.❌
- H2 is on the reactants side like it is supposed to be, so we shouldn't manipulate the third equation.✔️
- C2H2 is on the reactants side when it should be on the products side, so we have to manipulate the first equation.❌

Steps to Take

Whatever you do to the equation, you have to do the same to the enthalpy.

Results of Steps

After doing these things, we are left with:

Now the equations are set up properly to create the overall equation, but what happens with the extra compounds?

You could think of these as spectator compounds; they cancel out since they are present on both sides of the equation when all 3 equations are added together.

With this being said, the O2s cancel out, H2O cancels out, and the CO2s cancel out.

👉We then add the reactions together to find the original reaction and that ΔH = +1299.5 kJ + (−787 kJ) + (−285.8 kJ) = **+226.7 kJ**.

Calculate the value of ΔHreaction for the following reaction using the listed thermochemical equations.

Thought Process

Let's note a few things🤔:

- P4O10 is on the wrong side of the equation, so we have to manipulate equation 2❌.
- PCl5 is also on the wrong side of the equation and it doesn't have a coefficient of 6, so we have to manipulate equation 3❌.
- Cl3PO is on the right side of the equation, but it doesn't have a coefficient of 10 so we have to manipulate equation 4❌.

Steps to Take

This problem has a lot more steps! Let's go through the manipulations we have to make:

Results of Steps

After doing these things, we are left with:

Now we have everything on the right side of the equation and they all have the proper coefficients. Our last step is to check if all the spectators cancel out, so let's count them up!

Compound | Reactant Side | Product Side | Manipulation Necessary? |

P4 | 1/4 | 1 | ✔️ |

Cl2 | 3/2 | 6 | ✔️ |

PCl3 | 10 | 7 | ✔️ |

O2 | 5 | 5 | ❌ |

Luckily, all 3 compounds that we have to balance are in equation 1, meaning we now have to manipulate it in order for the equations to add up to the overall equation.

🤔What should be multiply equation 1 by? In order to get the same amount of each compound, we have to multiply equation 1 by 4 and its enthalpy by 4!

Now everything cancels out and we are left with the overall equation🥳! Last step is to add up all the enthalpies.

👉ΔH = -1225.6 kJ + 2967.3 kJ + 505.2 kJ + (−2857 kJ) = **-610.1 kJ**.

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