Assume that the following reaction is a single step reaction...

Assume that the following reaction is a single step reaction in which a $\mathrm{C}-\mathrm{Br}$ bond is broken as the $\mathrm{C}-\mathrm{I}$ bond is formed. The heat of reaction is $+38 \mathrm{~kJ} / \mathrm{mol}$. $$ \mathrm{I}^{-}(\mathrm{aq})+\mathrm{CH}_3 \mathrm{Br}(\mathrm{aq})+38 \mathrm{~kJ} \rightarrow \mathrm{CH}_3 \mathrm{I}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq}) $$ Figure Can't Copy a. With reference to collision theory, describe the general process that takes place as this reaction moves from reactants to products. b. List the three requirements that must be met before a reaction between $\mathrm{I}^{-}$ and $\mathrm{CH}_3 \mathrm{Br}$ is likely to take place. c. Explain why an $\mathrm{I}^{-}$ion and a $\mathrm{CH}_3 \mathrm{Br}$ molecule must collide before a reaction can take place. d. Explain why, in the process of this reaction, it is usually necessary for the new $\mathrm{C}-\mathrm{I}$ bonds to form at the same time as the $\mathrm{C}-\mathrm{Br}$ bonds are broken. e. Draw a rough sketch of the activated complex. (You do not need to show bond angles. Be sure to show the bond that is breaking and the bond that is being formed.) f. Explain why a collision between an $\mathrm{I}^{-}$ion and a $\mathrm{CH}_3 \mathrm{Br}$ molecule must have a certain minimum energy (activation energy) in order to proceed to products. g. The activation energy for this reaction is $76 \mathrm{~kJ} / \mathrm{mol}$. Draw an energy diagram for this reaction, showing the relative energies of the reactants, the activated complex, and the products. Using arrows show the activation energy and heat of reaction. h. Is this reaction exothermic or endothermic? i. Explain why an $\mathrm{I}^{-}$ion and a $\mathrm{CH}_3 \mathrm{Br}$ molecule must collide with the correct orientation if a reaction between them is going to be likely to take place.

Assume that the following reaction is a single step reaction in which a $\mathrm{C}-\mathrm{Br}$ bond is broken as the $\mathrm{C}-\mathrm{I}$ bond is formed. The heat of reaction is $+38 \mathrm{~kJ} / \mathrm{mol}$.

$$
\mathrm{I}^{-}(\mathrm{aq})+\mathrm{CH}_3 \mathrm{Br}(\mathrm{aq})+38 \mathrm{~kJ} \rightarrow \mathrm{CH}_3 \mathrm{I}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq})
$$

Figure Can't Copy
a. With reference to collision theory, describe the general process that takes place as this reaction moves from reactants to products.
b. List the three requirements that must be met before a reaction between $\mathrm{I}^{-}$ and $\mathrm{CH}_3 \mathrm{Br}$ is likely to take place.
c. Explain why an $\mathrm{I}^{-}$ion and a $\mathrm{CH}_3 \mathrm{Br}$ molecule must collide before a reaction can take place.
d. Explain why, in the process of this reaction, it is usually necessary for the new $\mathrm{C}-\mathrm{I}$ bonds to form at the same time as the $\mathrm{C}-\mathrm{Br}$ bonds are broken.
e. Draw a rough sketch of the activated complex. (You do not need to show bond angles. Be sure to show the bond that is breaking and the bond that is being formed.)
f. Explain why a collision between an $\mathrm{I}^{-}$ion and a $\mathrm{CH}_3 \mathrm{Br}$ molecule must have a certain minimum energy (activation energy) in order to proceed to products.
g. The activation energy for this reaction is $76 \mathrm{~kJ} / \mathrm{mol}$. Draw an energy diagram for this reaction, showing the relative energies of the reactants, the activated complex, and the products. Using arrows show the activation energy and heat of reaction.
h. Is this reaction exothermic or endothermic?
i. Explain why an $\mathrm{I}^{-}$ion and a $\mathrm{CH}_3 \mathrm{Br}$ molecule must collide with the correct orientation if a reaction between them is going to be likely to take place.

Thanks for your feedback!

Play audio

Feedback

Please give Ace some feedback