1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Anna11 [10]
3 years ago
8

1,4-Pentadiene has a AHhydro = -254 kJ/mol while trans-1,3-pentadiene has a AHhydra = -226 kJ/mol. Explain this difference in he

at of hydrogenation.
Chemistry
1 answer:
julsineya [31]3 years ago
5 0

Answer:

trans-1,3-pentadiene is more stable than 1,4-pentadiene due to presence of a conjugated double bond.

Explanation:

Here, \Delta H_{hydro}=H(hydrogenated pdt.)-H(diene)

H(hydrogenated pdt.) is same for both 1,4-pentadiene and 1,3-pentadiene as they both produce pentane after hydrogenation

H(diene) depends on stability of diene.

More stable a diene, lesser will be it's H(diene) value (more neagtive).

trans-1,3-pentadiene is more stable than 1,4-pentadiene due to presence of a conjugated double bond.

Hence, \Delta H_{hydro} is higher (less negative) for trans-1,3-pentadiene

You might be interested in
Oxygen, hydrogen, and water are substances. which of these substances are elements
m_a_m_a [10]
The substances Oxygen and Hydrogen are elements.
8 0
3 years ago
Which describes an element?
sesenic [268]

Answer:

I think it's D one. Because all others are wrong

3 0
2 years ago
A certain AB4 molecule has a square-planar molecular geometry.
harina [27]

Answer:  b). The B−A−B angles between neighboring B atoms are 90∘.

Explanation:  The square planar geometry is the geometry in which the four groups are connected through an angle of 90∘ and all 5 atoms are in one plane.

It is not necessary for the molecule to have two non bonding pair of electrons on atom A but if it does have , then its parent geometry will be distorted octahedral. And if it doesn't have this non bonding pair of electrons then the geometry would be the square planar.

Thus the molecule has four electron domains about the central atom A if the parent geometry is square planar otherwise it would have 8 electron domain in distorted octahedral geometry.

3 0
3 years ago
Calculate the mass % of K in potassium phosphate
Blizzard [7]

Answer:

\large \boxed{\mathbf{1. \, \,55.26 \, \%; \, \,2. \, \,30.15 \, \%  }}

Explanation:

1. Mass percent of K

\begin{array}{cccr}\mathbf{Atoms} & \textbf{Contribution} &   & \textbf{Subtotal}\\\text{3K} & 3 \times 39.10 & = & 117.30\\\text{1P} & 1 \times 30.97 & = & 30.97\\\text{4O} & 4 \times 16.00 & = &64.00\\& \text{TOTAL} & = & \mathbf{212.27}\\\end{array}

\text{Percent K} =  \dfrac{\text{117.30 g}}{\text{212.27 g}} \times \, 100\% =  \mathbf{55.26 \, \%}\\\text{The percent by mass of potassium is $\large \boxed{\mathbf{55.26 \, \% }}$}

2. Mass percent of O

\text{Percent O} =  \dfrac{\text{64.00 g}}{\text{212.27 g}} \times \, 100\% =  \mathbf{30.15 \, \%}\\\text{The percent by mass of oxygen is $\large \boxed{\mathbf{30.15 \, \% }}$}

6 0
3 years ago
How many grams of methanol is formed by the mild oxidation of 64 grams of methane?
Dafna1 [17]

Answer: 1. Introduction

ARTICLE SECTIONSJump To

Currently, there exists no industrial process capable of directly converting methane to methanol. While many processes have been explored, none to date has proven cost-effective. A consequence of the paucity of catalysts for the direct oxidation of methane to methanol is the annual flaring of 140 billion cubic meters of natural gas at remote oil drilling locations around the world, accounting for 1% of global CO2 emissions with no associated energy gains.(1) Two distinct problems are often cited as being responsible for the lack of catalysts available for such a process: the large barriers associated with activating the nonpolar and highly symmetric methane molecule and the higher relative reactivity of the desired products.(2,3) Regarding the first problem, while methane activation barriers on transition metals are generally high (ΔGa(300 K, 1 bar) > 1.2 eV),(4) several publications have highlighted nontransition metal catalysts able to activate methane at low temperatures or with low density functional theory (DFT)-predicted barriers.(5−8) However, solutions to the second problem, that of product reactivity, have proven more elusive. Even if methanol can be locally produced by a catalyst at low temperatures, it is difficult to stop its CH bonds, which have a 0.4 eV lower bond dissociation energy (BDE) than those in methane, from being further oxidized.(3,9) Indeed, an example of a continuous process able to simultaneously achieve both high methane conversion and high methanol selectivity has yet to be established, pointing to a robust selectivity–conversion trade-off.(10)

In light of this challenge, many efforts have shifted focus from catalytic to stepwise processes, in which reactant consumption and product collection are decoupled. These systems bypass the aforementioned selectivity–conversion trade-off by producing a protected methanol derivative that is less prone to further oxidation compared to free methanol. Examples in homogeneous catalysis are often quasi-catalytic, i.e., turnover number (TON) > 1, and proceed through the use of small-molecule protecting groups. For example, Periana et al. oxidized methane to a stable methyl bisulfate product that could later be hydrolyzed to yield methanol and sulfuric acid.(11,12) However, these systems are limited by expensive oxidants and the cost of recycling protecting groups. Similarly, it was found that metal-exchanged zeolites, which had previously achieved methanol yields of ∼3% (64% CH3OH selectivity; 5% CH4 conversion) in the catalytic process,(13) could unlock higher methanol selectivities (∼98%) when used as heterogeneous protecting groups to oxidize methane to methanol stoichiometrically (TON = 1).(14−18) Such processes typically involve three steps: zeolite activation at high temperatures (∼450 °C), stoichiometric methane oxidation at lower temperatures (∼150 °C), and methanol recovery by flowing water (∼150 °C).(15) Unfortunately, this energy-intensive temperature cycling in combination with the expensive oxidizing agents required to reactivate the catalyst and low methanol yields per cycle tend to limit the practical application of these approaches.(10)

Herein, we aim to understand the limitations of direct methane to  

Explanation: Sorry for how long it is

8 0
3 years ago
Other questions:
  • Which career area in chemistry applies new discoveries to practical applications useful for consumers
    14·2 answers
  • X + Y XY + heat What happens as the temperature is increased? [X] remains constant. [X] increases. [X] decreases.
    7·2 answers
  • Determine the molality of ions in a solution formed by dissolving 0.187 moles of NaCl in 456 grams of water. The density of the
    7·1 answer
  • 100 POINTS ANSWER FAST
    13·2 answers
  • Which pair of molecules is not a polar bond?<br> OA. N-O<br> OO<br> B. C-O<br> C.O-H<br> OD. 0-0
    10·1 answer
  • How many moles of methane will react to form 3.2 moles of carbon dioxide?
    6·1 answer
  • Consider two liquids, labeled A and B, that are both pure substances. Liquid A has
    15·1 answer
  • If you placed a piece of hot metal in cold water, the temperature of the metal would ______ while the temperature of the water w
    6·1 answer
  • What are glaze defects or flaws​
    8·1 answer
  • What is chemical change ?​
    5·2 answers
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!