I want to thank you for making this equilibrium video as well as the concepts of how to get to equilibrium by demonstrating the “seesaw” visual. I’m the type of student (sometimes, not always) who needs that extra explanation or “visual” to get the point of steps. From the bottom of my heart, I can’t thank you and the teacher who put the extra effort for students such as my self to get the grasp of what we’re actually learning. It’s teachers like you and alike who are the real MVP’s! ❤ God bless you!
H MGloria, I am so glad the videos were helpful. It makes me very happy. I am proud of your extra work and effort searching for videos to better understand the content. God bless you!! Thanks:)
Hi, I am not sure if I am understanding this incorrectly but in my calculator when I input (0.035)(0.035)/(0.015) I am getting 0.81666...7, I might have missed a step or misunderstood, could you explain if I missed a calculation or misunderstood the calculation pls. Btw, love your videos, never have I understood chem so well, thank you using your time to make these videos.
K is not unitless is it? Here wouldn’t it have units of M? In general, it would depend on the degree of the numerator minus the degree of the denominator.
It is a ratio of product and reactant concentrations which are both M. You are correct, based on exponents, mathematically it can have a final M to the x power. However, because it is concentration divided by concentration it is considered unitless. It is just a ratio of concentrations at equilibrium for K. Thanks!
@@chiararomano1818 Hi Chiara, It is one of the main differences between the equilibrium constant (K) and rate constant (k). It is so great you noticed that!
