In this video I learned how to figure out if an integrated rate law is a first order process, second order process, or a zero order reaction. I also learned about half life, which is the time when the initial concentration has decreased by half.
In this video, we go into further detail into Kinetics and learned integrated rate laws for the first and second process as well as apply half-life to first order reactions.
Q: How come in the integrated second order process we don’t use the opposite of k for the slope but we do in first order?
In this lesson I learned about rate laws for first order processes, second order processes, and zero order processes. These all have straight lines. We have to do some calculations with natural log (ln) to determine which order process it is.
In these videos I learned that the integrated rate law of a first order process is the “natural log of concentration of A at time t is equal to negative rate constant times time plus the natural log of the initial rate of A”. Since this is in the form y = mx + b we know that the y is the natural log of concentration A at time t, the slope is negative K and the y-intercept is the natural log of the initial concentration of A. Applying this information we learn that when looking at a graph of ln[a]t compared to time, if it is a straight line, we know that the process is first order. The intergrated rate law for second order processes is 1/[A]t = kt + 1/[A]0. If the graph of 1/[A]t compared to time is a straight line, then we know that that process is a second order process. Zero order reactions are due to circumstance and have to at some point change to a first or second order process, however, while they are zero order processes, their rate law is independent of concentration. I also learned that the half life of first order is not dependent on concentration, but instead on the rate constant, I learned how to take half life information of solve for the rate constant.
In these three videos, I have learned about the integrated laws of zero order, first order and second order, as well as the integrated laws of half life of first order and second order. I learned that zero order reactions are not dependent on the concentration of the substance. I learned that I can determine whether a reaction is first or second order by graphing the data and the order is based on which formula I used to graph the data into a straight line. I also learned that the half life of first order is not dependent on the concentration, but on the constant instead, and the half life of second order is dependent on both the initial concentration and the constant.
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In this video I learned how to figure out if an integrated rate law is a first order process, second order process, or a zero order reaction. I also learned about half life, which is the time when the initial concentration has decreased by half.
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In this video, we go into further detail into Kinetics and learned integrated rate laws for the first and second process as well as apply half-life to first order reactions.
Q: How come in the integrated second order process we don’t use the opposite of k for the slope but we do in first order?
LikeLike
In this lesson I learned about rate laws for first order processes, second order processes, and zero order processes. These all have straight lines. We have to do some calculations with natural log (ln) to determine which order process it is.
LikeLike
In these videos I learned that the integrated rate law of a first order process is the “natural log of concentration of A at time t is equal to negative rate constant times time plus the natural log of the initial rate of A”. Since this is in the form y = mx + b we know that the y is the natural log of concentration A at time t, the slope is negative K and the y-intercept is the natural log of the initial concentration of A. Applying this information we learn that when looking at a graph of ln[a]t compared to time, if it is a straight line, we know that the process is first order. The intergrated rate law for second order processes is 1/[A]t = kt + 1/[A]0. If the graph of 1/[A]t compared to time is a straight line, then we know that that process is a second order process. Zero order reactions are due to circumstance and have to at some point change to a first or second order process, however, while they are zero order processes, their rate law is independent of concentration. I also learned that the half life of first order is not dependent on concentration, but instead on the rate constant, I learned how to take half life information of solve for the rate constant.
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In these three videos, I have learned about the integrated laws of zero order, first order and second order, as well as the integrated laws of half life of first order and second order. I learned that zero order reactions are not dependent on the concentration of the substance. I learned that I can determine whether a reaction is first or second order by graphing the data and the order is based on which formula I used to graph the data into a straight line. I also learned that the half life of first order is not dependent on the concentration, but on the constant instead, and the half life of second order is dependent on both the initial concentration and the constant.
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