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2 years ago

Which of the following statements is true for a system at chemical equilibrium?

Chemistry

1 answer:

ZanzabumX [31]2 years ago

4 0

Answer:

Option B is true: The system can do no work

Explanation:

a. The system releases energy at a steady rate. False

In thermodynamic equilibrium there are no net macroscopic flows of matter or of energy, either within a system or between systems.

b. The system can do no work. True

If the connection between the systems allows transfer of energy as heat but does not allow transfer of matter or transfer of energy as work, the two systems may reach thermal equilibrium without reaching thermodynamic equilibrium.

c. The system consumes energy at a steady rate. False.

In thermodynamic equilibrium there are no net macroscopic flows of matter or of energy, either within a system or between systems.

d. The kinetic energy of the system is zero. False.

At maximum displacement from the equilibrium point, potential energy is a maximum while kinetic energy is zero. At the equilibrium point the potential energy is zero and the kinetic energy is a maximum. At other points in the motion the oscillating body has differing values of both kinetic and potential energy.

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The highest energy occupied molecular orbital in the f-f bond of the f2 molecule is _____

Morgarella [4.7K]

The basis of finding the answer to this problem is to know the electronic configuration of Fluorine. That would be: [He] 2s² 2p⁵. The valence electrons, which are the outermost electrons of the atom, are the ones that participate in bonding. Since the highest orbital for F is 2p, that means the highest energy occupied would be 2.

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2 years ago

Which choice(s) correctly rank(s) the bonds in terms of increasing polarity?

Marina CMI [18]

Answer:

(II) only correctly rank the bonds in terms of increasing polarity.

Explanation:

Bond polarity is proportional to difference in electronegativity between bonded atoms.

Atoms Electronegativity Bond Electronegativity difference

Cl 3.0 Cl-F 1.0

Br 2.8 Br-Cl 0.2

F 4.0 Cl-Cl 0

H 2.1 H-C 0.4

C 2.5 H-N 0.9

N 3.0 H-O 1.4

O 3.5 Br-F 1.2

I 2.7 I-F 1.3

Si 1.9 Cl-F 1.0

P 2.2 Si-Cl 1.1

Si-P 0.3

Si-C 0.6

Si-F 2.1

So, clearly, order of increasing polarity : O-H > N-H > C-H

So, (II) only correctly rank the bonds in terms of increasing polarity

4 0

2 years ago

The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.

natima [27]

The valence electrons are as follows for these groups of elements:

Halogen- SEVEN (halogens are group 7 elements that need one electron for the octet rule to be achieved)

Alkali Metals - ONE (these are group one elements that lose a single electron to form an octet and cation)

Alkaline Earth Metals - TWO (group two elements that lose two electrons to form 2+ cations)

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2 years ago

ethylene glycol used in automobile antifreeze and in the production of polyester. The name glycol stems from the sweet taste of

Luden [163]

Answer: The empirical and molecular formula for the given organic compound is $CH_3O$ and $C_4H_{12}O_4$

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of $CO_2=9.06g$

Mass of $H_2O=5.58g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 9.06 g of carbon dioxide, $\frac{12}{44}\times 9.06=2.47g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 5.58 g of water, $\frac{2}{18}\times 5.58=0.62g$ of hydrogen will be contained.

Mass of oxygen in the compound = (6.38) - (2.47 + 0.62) = 3.29 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{2.47g}{12g/mole}=0.206moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.62g}{1g/mole}=0.62moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{3.29g}{16g/mole}=0.206moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.206 moles.

For Carbon = $\frac{0.206}{0.206}=1$

For Hydrogen = $\frac{0.62}{0.206}=3$

For Oxygen = $\frac{0.206}{0.206}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 1 : 3 : 1

Hence, the empirical formula for the given compound is $C_1H_{3}O_1=CH_3O$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

We are given:

Mass of molecular formula = 124 amu = 124 g/mol

Mass of empirical formula = 31 g/mol

Putting values in above equation, we get:

$n=\frac{124g/mol}{31g/mol}=4$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{(1\times 4)}H_{(3\times 4)}O_{(1\times 4)}=C_4H_{12}O_4$

Thus, the empirical and molecular formula for the given organic compound is $CH_3O$ and $C_4H_{12}O_4$

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2 years ago

Under which conditions will sugar most likely dissolve fastest in a cup of water? A. a sugar cube with stirring at 5oC B. a suga

OverLord2011 [107]

I believe the answer is sugar crystals with stirring at 15 degrees Celsius.
Solubility is the maximum amount of a substance that will dissolve in a given amount of solvent at a specific temperature. There are two major factors that affect solubility are temperature and pressure. Temperature affects solubility of both solids and gases, but pressure only affects the solubility of gases. Increasing the surface area of solutes also increases the solubility.

5 0

2 years ago

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