The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism: H 2 O 2 (aq) + I - (aq) → H 2 O(l) + IO - (aq) (slow) IO - (aq) + H 2 O 2 (aq) → H 2 O(l) + O 2 (g) + I - (aq) (fast) (a) Write the chemical equation for the overall process.

Hello everyone today. We are being asked to write an overall equation for the overall reaction using the above mechanism. So we have step one, step two and step three. So the first thing you want to do is you want to write these steps out? So we'll do just that will say we have to gas reacting to form two most of bromine bromine gas. We also have that bro mean gas forming with methane in the gas form to form hbr which is a strong acid in the gas form and Methane or methyl group in the gas form. And then we have that CH three reacting with our roaming from earlier To form this CH three be our product. And so we want to remember a couple of rules. The first one is that the same species? On the same side they're going to add and the same species this is going to be the reverse on different sides. So different sides, they are going to go ahead and subtract using that rule we can go ahead and proceed, we see that we have a we have one bro man on the right on the first equation and we have one brunette on the left for the second equation. Therefore they're going to cancel out. We also see in a second equation we have a CH three on the right of the arrow and we also have a CH three on the left of the arrow. Of the subsequent reaction? We were left with one bro mean in the first equation since we had to and only got rid of one. However, notice how the third reaction also has a bro mean, so we can go ahead and get rid of that second bro mean, and thus we are left with the remaining equation that we have our bro mean, gas, BR two gas plus our methane CH four, also in the gas, and that is going to go ahead and form CH three B are in our gas form as well as H. B. R. In the gas form as well. I hope this helped, and until next time.

Ch.14 - Chemical Kinetics

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Brown 14th Edition

Ch.14 - Chemical Kinetics

Problem 72a

Chapter 14, Problem 72a

The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:
H₂O₂(aq) + I^-(aq) → H₂O(l) + IO^-(aq) (slow)
IO^-(aq) + H₂O₂(aq) → H₂O(l) + O₂(g) + I^-(aq) (fast)
(a) Write the chemical equation for the overall process.

Verified step by step guidance

Identify the reactants and products in each step of the mechanism. In the first step, the reactants are H$_2$O$_2$ and I$^-$, and the products are H$_2$O and IO$^-$. In the second step, the reactants are IO$^-$ and H$_2$O$_2$, and the products are H$_2$O, O$_2$, and I$^-$.

Notice that IO$^-$ is produced in the first step and consumed in the second step, and I$^-$ is consumed in the first step and regenerated in the second step. These species are intermediates and do not appear in the overall equation.

Add the equations for the two steps together, canceling out the intermediates (IO$^-$ and I$^-$) that appear on both sides of the equation.

Sum up the remaining reactants and products. The reactants that appear are H$_2$O$_2$ from both steps, and the products are H$_2$O from both steps, along with O$_2$ from the second step.

Write the overall balanced chemical equation for the process, ensuring that the number of atoms for each element is the same on both sides of the equation.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Chemical Equations

A chemical equation represents a chemical reaction using symbols and formulas. It shows the reactants on the left side and the products on the right, separated by an arrow indicating the direction of the reaction. Balancing the equation is crucial to obey the law of conservation of mass, ensuring that the number of atoms for each element is the same on both sides.

Reaction Mechanisms

A reaction mechanism describes the step-by-step sequence of elementary reactions by which overall chemical change occurs. Understanding the mechanism helps in identifying the rate-determining step, which is the slowest step that controls the speed of the overall reaction. In this case, the two-step mechanism illustrates how iodide ion facilitates the decomposition of hydrogen peroxide.

Catalysis

Catalysis involves the acceleration of a chemical reaction by a substance called a catalyst, which is not consumed in the reaction. Catalysts work by providing an alternative pathway with a lower activation energy for the reaction. In the given question, iodide ion acts as a catalyst, facilitating the breakdown of hydrogen peroxide into water and oxygen without being permanently altered.

The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)(a) Write the chemical equation for the overall process.

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Key Concepts

Chemical Equations

Reaction Mechanisms

Catalysis