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Amanda [17]
3 years ago
15

The compound 1-butene is modeled here. What would need to happen for molecules of this compound to transform into polybutene? A.

Covalent bonds would need to form between the molecules. B. Each molecule would need to gain at least one oxygen atom. C. More double bonds would need to form in each molecule. D. Hydrogen atoms would need to be transferred between molecules.
Chemistry
1 answer:
kompoz [17]3 years ago
4 0
In order to form polymers, we need to chain molecules together. This involves making bonds between them.

Shifting H’s around doesn’t accomplish anything.

Forming more double bonds will have the opposite result, as it would make the molecules more stable and less likely to react with each other.

Adding oxygen to the molecule no longer makes it polybutene. That would likely result in the formation of some sort of ether, as hey would react to form a C-O-C Bond.

The only answer left is A. In order to form polyalkenes, we have to break a double bond so that it’s available to form more covalent bonds.

Hope this helps
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Lina20 [59]

The number of mole of copper in the sample is 0.008 mole.

Mole is simply defined as the unit of amount in a substance.

The mole of a substance can be obtained by dividing the mass of the subtance by its molar mass i.e

Mole = mass / molar mass

With the above information, we can obtain the mole of copper in the compound as follow:

Mass of copper = 0.5066 g

Molar mass of copper = 63.5 g/mol

<h3>Mole of copper =? </h3>

Mole = mass / molar mass

Mole of copper = 0.5066 / 63.5

<h3>Mole of copper = 0.008 mole </h3>

Therefore, 0.008 mole of copper was initially present in the compound.

Learn more: brainly.com/question/14295066

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3 years ago
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BabaBlast [244]
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3 years ago
Determine the electrical work required to produce one mole of hydrogen in the electrolysis of liquid water at 298°K and 1 atm. T
Ostrovityanka [42]

Explanation:

The given data is as follows.

          \Delta H = 286 kJ = 286 kJ \times \frac{1000 J}{1 kJ}

                            = 286000 J

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Hence, formula to calculate entropy change of the reaction is as follows.

          \Delta S_{rxn} = \sum \nu_{i}S_{i}_(products) - \sum \nu_{i}S_{i}_(reactants)

                     = [(\frac{1}{2} \times S_{O_{2}}) - (1 \times S_{H_{2}})] - [1 \times S_{H_{2}O}]

                    = [(\frac{1}{2} \times 205) + (1 \times 131)] - [(1 \times 70)]

                    = 163.5 J/K

Therefore, formula to calculate electric work energy required is as follows.

             \Delta G_{rxn} = \Delta H_{rxn} - T \Delta S_{rxn}

                            = 286000 J - (163.5 J/K \times 298 K)

                            = 237.277 kJ

Thus, we can conclude that the electrical work required for given situation is 237.277 kJ.

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