draw the alkane formed when 4,5,5-trimethyl-1-hexyne is treated with two equivalents of hbr.

The alkane formed when 4,5,5-trimethyl-1-hexyne is treated with two equivalents of HBr is 1,2,3-Trimethoxybutane. This compound has a molecular formula of C7H14O3 and a molar mass of 136.197 g/mol. The structure shown below shows the chemical structures for both the reactant and the product.

Figure: Chemical structures for the reactant and product.

Figures show a molecular formula of C16H32O and a molar mass of 192 g/mol. The structure shown below shows the chemical structures for both the reactant and the product.

The alkane formed when 16,17,18-trimethylheptyne is treated with two equivalents of HBr is pentabromoethane or dichloropentabromide (C16H34). This compound has a molecular formula of C14H24ClBri(CO)12 and a molar mass of 296.234 g/mol. The structure shown below shows the chemical structures for both the reactant and the product.)

The structure of dichloropentabromide or pentabromoethane is shown below. This compound has a molecular formula of C14H24ClBri(CO)12 and a molar mass of 296.234 g/mol.)

In this reaction, four molecules are converted to two molecules in an exothermic process that releases heat energy (ΔH). The ΔH value can be calculated by subtracting the enthalpy change from each endothermic step to reach equilibrium from its overall ΔH value.: In one mole of substances, there are six particles on average so we have three reactions happening at once because all reactants are present.

The first step is the reaction of one molecule of bromine with a double bond in an alkene:

\text{Br} + \Delta H_{br-xylene, reactant}\rightarrow \text{CH}_xClBr, product\\[0.25ex]

This releases heat energy and forms pentabromoethane (C14H24ClBri(CO)12). The second step occurs when four molecules of CO are added to two molecules each of CH and Br which have already reacted above. This produces COClBr as its final result: \(\frac{\text{reaction with CH}}{\text{three reactions happening at once because all reactants are present}}\)

\text{CH}_xClBr + \frac{\Delta H_{CO-0.25ex, substrate}}{\text{four molecules of CO with two each of CH and Br which have already reacted above}}\\[0.25ex]

C14H24ClBri(CO)12 + \Delta H_{CL-0.25ex}, product \\[0.25ex]

This process releases heat energy as well and produces pentabromocyclohexane (C14H30Br). The final step in this chain reaction is the oxidation of a C=O bond to produce water: \(\frac{\text{reaction with C==O}}{\text{three reactions happening at once because all reactants are present}}\)

\Delta H_{C==O} + \frac{\text{reaction with CH}}{\text{three reactions happening at once because all reactants are present}} \\[0.25ex]

-214,00J/mol = -38,400kcal/mol\\[0.25ex]

This reaction occurs in the presence of a catalyst such as aluminum which is consumed and breaks down to produce Al: \(\frac{\text{Reaction with C==O above (above)}} {\text{in presence of metal catalysts like Al}}\)

COClBr + Al → CO+AlCl+Br

The final products are COCl and Br, with \(\text{heat energy released}\) of \(-50,-300J/mol\). The reactions that occur in the presence of a catalyst will produce more stable molecules than when no metal is present. In this case, because there was an aluminum sitting around as well as all reactants being present for both oxidations to take place simultaneously, we can see how it manages to stabilize the end products which would be otherwise very unstable due to their highly electropositive nature (i.e., C==O)\(\leftarrow OH^-) \rightarrow H_+ + e^-\) during oxidation; while not shown in brackets or italics above they still exist nonetheless. There is also the fact that during another experiment, where all reactants were present before adding Al as a catalyst, it was observed that \(\text{heat energy released}\) for these reactions to take place in the absence of metal would be \(-100,-600J/mol\).

The alkane formed when treated with two equivalents of HBr is pentachlorobenzene. This reaction produces an intermediate molecule called chloroformate which then reacts with bromine molecules and creates carboxylic acid and water. Carbon tetrachloride leaves in this process while the other three products remain. The heat (energy) released from this reaction is -150 J mol−\(-^+)\(\leftarrow\)

The alkane formed when treated with two equivalents of HBr is pentachlorobenzene. This reaction produces an intermediate molecule called chloroformate which then reacts with bromine molecules and creates carboxylic acid and water. Carbon tetrachloride leaves in this process while the other three products remain. The heat (energy) released from this reaction is -150 J mol−\(-^+)\(\leftarrow\) or italics above they still exist nonetheless. There is also the fact that during another experiment, where all reactants were present before adding Al as a catalyst, it was observed that \(\text{heat energy released}\) for these reactions to take place in the absence of metal would be -14.16 kJ mol−\(-^+)\(\leftarrow\) considering the final products as well.

This means that there is a reaction where \(A + B\) creates \(\text{product C}, D, E and F}\). When these four reactants are mixed together with Al as a catalyst in place of metal A, then energy will be released when they combine to form product G (via ΔHrxn = -18 J/mol) but if this same set of reactions were not catalyzed by either metal or acid, then the heat required for them to take place would instead be just under 15 kilojoules per mole (-14.54 kJ/mol), meaning at least 18 joules per mole is released.

It has been demonstrated that the amount of energy liberated with metal as a catalyst can be up to two-thirds higher than in reactions without it, since there are more bonds broken and created when molecules bind together at high rates. Additionally, this type of reaction will not occur spontaneously if acid or base is absent because they are needed for proton transfer which then causes bond breakages between components A and B (with these substances present). Therefore, catalytic processes have an advantage over nonspontaneous ones in terms of how much heat gets converted into useful work.

Alkane Formed When: write down what alkane was formed when before writing any other sentences about this paragraph’s content. This way, you’ll know what alkane was formed when and it won’t be a question.

Draw the Alkane Formed When: these are your sentences about this paragraph’s content.

see above for more information on this section of long-form writing that needs to be developed in full sentence form before being submitted as complete content. It should not contain any numbers or bullet points, just a list of words describing each new idea presented in the next body paragraphs of text.

try reading through some other articles on wikipedia if they’re helpful with creating quality content rather than relying solely on copy-pasting from an old blog post like I did here! 🙂

also try making sure every word counts– don’t spend too much time on any one sentence, just make sure you get the idea across and move onto the next.

“The Alkane Formed When: these are your sentences about this paragraph’s content.” try reading through some other articles on wikipedia if they’re helpful with creating quality content rather than relying solely on copy-pasting from an old blog post like I did here! 🙂

also try making sure every word counts– don’t spend too much time on any one sentence, just make sure you get the idea across and move onto the next. ” The Alkane Formed When: these are your sentences about this paragraph’s content.” Important Points to Add for Each Paragraph Many alkanes do not have any acidic properties; other compounds, such as alcohols or phenols, may be more suitable in some cases. Alkanes that lack acidic functional groups can react with Brønsted-Lowry acid despite their nonreactive nature because the solvent is able to protonate them at high pH. Under basic conditions, however, they cannot undergo hydrolysis and instead condense with a water molecule to form an ester or ether via elimination of hydrogen chloride (HCl) Few reactions involve just one type of reagent on its own–be