Sapling Question

[Isis_DW_3G]

how did we determine that reactant C was a zero-order reactant?
Thanks!

[Kayla Law 2D]

Hi! To determine the order of C, look for two experiments where the initial concentrations of A and B are the same, but the initial concentration of C is different. Therefore, we look at experiments 1 and 4 since the initial concentrations of A and B are the same between both experiments, but the initial concentration of C is different. Even though the initial concentration of C differs from experiment 1 to 4, the initial rate of the reaction is the same which suggests that the concentration of C does not affect the reaction rate. Therefore, C is a zero-order reactant. Hope this helps! :)

[Shrinidhy Srinivas 3L]

If we are trying to determine the order of the reactant, C, we want to look at the two data rows where A and B remain constant, but C changes. As such, we want to look at Rows 1 and 4. We can see that even when the concentration of C changes, the rate remains the same. This is indicative of a zero-order process, meaning that Reactant C is zero-order.

[darchen3G]

Look at experiments 1 and 4. Since A and B were the same and C was different, the change in the rate would be the order of C. SInce the rate didn't change then C is 0 order.

[Stephanie Zhang 2K]

Hi! To determine any reactant's order, you want to choose to compare between 2 reactions where the only value that changes is the reactant's concentration.
Looking at the reactions given, we can see that for Experiment 1 and 4, the values of A and B stay the same, while the value of C changes. Just quickly looking at it, we see that as the value of C changes, the initial rate does not change. Therefore, we can infer that C does not have any effect on the initial rate, so its order must be 0.
Another (and more reliable) way to do this is to divide rate law of 1 by rate law of 4, or vice versa. each rate law is rate=[A]^n [B]^m [C]^l, and so when dividing rate law 1 by rate law 4, we can plug in the initial rates and the concentrations of each compound. From there, we can see that the concentrations of [A] and [B] cancel each other out, leaving rate1/rate4= [concentration of C1]^l/[concentration of C2]^l, and rate1/rate4 is equal to 0. Then just solve for l, and you should get the same answer. Hope this helped!

[rhettfarmer-3H]

I think the way we are trying to figure out this value for C. Is through a system of equations almost comparing two equation with only C. So equations 1 and 4. Values of A and B are the same which is a form of isolating C. Therefore when comparing the two A, B and k can be canceled out because both equations share these values.
From there we get C^c=12.8 and C^c=12.8 Divide the two and we get C^c/C^c=12.8/12.8 Which gives 1=1 We know that anything to power 0 is 1. So it makes sense that C is in zero order.
Do the same with A and B to isolate and follow some produre. remember C is zero is always 1

[Alan Huang 1E]

In this problem, we found the orders of C by comparing reactions in which A and B were held constant while C changed.

Comparing experiments 1 and 4 which fulfilled these requirements found that while the concentration of C changed, the initial rate did not. This means that changing the concentration of C did not affect the rate.

Therefore, we can conclude that C was zero order.

[John Calonia 1D]

You can see that C changes throughout the experiment at seemingly random intervals while other variables are changing as well, showing that its concentrations has no effect on the rate law

[Cora Chun 2D]

If you compare experiments 1 and 4 where reactants A and B are constant and the concentration of C changes, the rate still stays the same. This means that the concentration of C has no effect on the rate, meaning it is 0th order. [C]^0 in the rate law = 1, so the rate law just depends on the concentrations of A and B!

[Kaleb Tuliau 3E]

Just for clarification, this weeks sapling is due on Friday right?