What color change is exhibited by phenolphthalein during a titration of aqueous acetic acid with aqueous sodium hydroxide ? a. colorless to pink b. pink to colorless c. no color change d. yellow to blue e blue to yellow

Answer:

32 electron

Thus,the fourth level can hold up to 32 electrons,2 in the s orbital,6 in the three p orbitals,10 in the five d orbitals,and 14 in the seven f orbitals.

The freezing point of the silver nitrate solution is - 12.6 degrees Celsius.

We know that freezing point is a colligative property. This implies that it depends on the amount of the substance that is present . We should also know that when we dissolve the  silver nitrate in water, the particles of the substance would decrease the freezing point of the water.

Freezing point of water = 0 degrees Celsius

Molality of the solution = 3.40 m

Freezing constant of water =  1.86∘C/m

We now have;

ΔT = K m i

ΔT =  1.86∘C/m *  3.40 m * 2

ΔT = 12.6 degrees

Temperature of the solution = 0 - 12.6 = - 12.6 degrees Celsius

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Answer:

log = ( - 0.51 z 2) / ( 1 + ( / 305)

Explanation:

Answer:

number of carbon-carbon single (C - C) bonds: 1

number of carbon-hydrogen single (C H) bonds: 5

number of nitrogen-hydrogen sing le (N H) bonds:2

number of lone pairs: 1

Explanation:

Ethanamine is a colourless gas having a strong 'ammonia- like' odour. It contains the -NH2 group which makes it an amine. It contains one carbon-carbon bond, five carbon-hydrogen bonds and two nitrogen-hydrogen bonds.

Nitrogen, being sp3 hybridized in the compound has a lone pair of electrons localized on one of the sp3 hybridized orbitals of nitrogen while one sp3 hybridized orbital of nitrogen is used to form a carbon-nitrogen bond. The other two sp3 hybridized orbitals on nitrogen are used to form the two nitrogen-hydrogen bonds.

The element of lowest atomic number whose electron configuration has 4 completely filled p orbitals is, Xenon, Xe with electron configuration:1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶.

According to the question, we are required to identify the element with the lowest atomic number whose electronic configuration has four completely filled p sub-shells.

Evidently, the shell with energy level one has no p orbital.

p(x) , p(y) and p(z) with two electrons of opposing spin in each sub orbital.

In essence, the element in question should have electron configuration;

The electron configuration above contains 54 electrons and has atomic number, 54.

In essence, the element of lowest atomic number whose electron configuration has 4 completely filled p orbitals is, Xenon, Xe.

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Answer:

b

Explanation:

Answer:

X: mechanical energy

Y: electrical energy( C)

Explanation:

Answer

False

Explanation:

Answer:

% NiCl2 = 24.13%

% water = 78.57%

Explanation:

Mass percentage = mass of solute/mass of solution × 100

According to this question, a solution contains 159 g of NiCl2 in 500 g of water. Hence, mass of the solution is calculated as follows:

Mass of solution = 159g + 500g

Mass of solution = 659g

Therefore;

A) % Mass of NiCl2 in solution = mass of NiCl2/mass of solution × 100

% Mass of NiCl2 in solution = 159/659 × 100

% Mass of NiCl2 in solution = 0.2413 × 100

= 24.13%

B) % Mass of water in solution = mass of water/mass of solution × 100

% Mass of water in solution = 500/659 × 100

% Mass of water in solution = 0.7587 × 100

% Mass of water in solution = 75.87%

Answer:

100 rbed  KJ |0| +2k

Explanation:

Answer:

6.022 x 10²³ electrons

Explanation:

Answer:

At earlier times elements were arrangrd on the basis of their atomic masses to study their properties easily but there were various problems like isotopes needs different position in perodic table.

After discovery of atomic number modern periodic table was created on the basis of atomic number (number of proton) that is unique for each element and varies regularly. So study of a group of elements is much easier than each element seperately that is why modern periodic table was formed.

Explanation:

Answer:

The ration of molar concentration is "2.5".

Explanation:

The given values are:

Average density of salt water,

= \(1.03 \ g/cm^3\)

Net pressure,

= \(2.00 \ atm\)

Increase in pressure,

= \(1.00 \ atm\)

Now,

The under water pressure will be:

=  \(\frac{15 \ m}{10}\times 1 \ atm +1 \ atm\)

=  \(1.5\times 1+1\)

=  \(1.5+1\)

=  \(2.5 \ atm\)

hence,

The ratio will be:

=  \(\frac{(\frac{n}{V})_{15m} }{(\frac{n}{V})_{surface} }\)

or,

=  \(\frac{P}{P_s}\)

=  \(\frac{2.5}{1}\)

=  \(2.5\)

Answer: -2 because it gains 2 electrons

Explanation:

An ion is considered to be an atom which is formed by gain or loss of electrons.

The ions are classified into two which are called the cation and anion.

The cation is classified as the positive charge formed by loss of electrons.

The anion is classified as the negative charge ion formed by gain of electrons.

On gaining two electrons, the atom would occupy -2 charge.

The energy of combustion for one mole of butane to be approximately 2888.81 kJ/mol.

To calculate the energy of combustion for one mole of butane (C4H10), we need to use the information provided and apply the principle of calorimetry.

First, we need to convert the mass of the butane sample from grams to moles. The molar mass of butane (C4H10) can be calculated as follows:

C: 12.01 g/mol

H: 1.01 g/mol

Molar mass of C4H10 = (12.01 * 4) + (1.01 * 10) = 58.12 g/mol

Next, we calculate the moles of butane in the sample:

moles of butane = mass of butane sample / molar mass of butane

moles of butane = 0.367 g / 58.12 g/mol ≈ 0.00631 mol

Now, we can calculate the heat released by the combustion of the butane sample using the equation:

q = C * ΔT

where q is the heat released, C is the heat capacity of the calorimeter, and ΔT is the change in temperature.

Given that the heat capacity of the bomb calorimeter is 2.36 kJ/°C and the change in temperature is 7.73 °C, we can substitute these values into the equation:

q = (2.36 kJ/°C) * 7.73 °C = 18.2078 kJ

Since the heat released by the combustion of the butane sample is equal to the heat absorbed by the calorimeter, we can equate this value to the energy of combustion for one mole of butane.

Energy of combustion for one mole of butane = q / moles of butane

Energy of combustion for one mole of butane = 18.2078 kJ / 0.00631 mol ≈ 2888.81 kJ/mol

Therefore, the energy of combustion for one mole of butane is approximately 2888.81 kJ/mol.

In conclusion, by applying the principles of calorimetry and using the given data, we have calculated the energy of combustion for one mole of butane to be approximately 2888.81 kJ/mol.

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24. The IUPAC name of the compound is 2,4-dimethyl-1-pentanal (Option B)

25. The IUPAC name of the compound is 5-methyl-3-octanone (Option C)

The international union of pure and applied chemistry (IUPAC) standard for naming organic compounds is given below:

24. The name of the compound is given as follow:

Thus, the IUPAC name of the compound is:

2,4-dimethyl-1-pentanal (Option B)

25. The name of the compound is given as follow:

Thus, the IUPAC name of the compound is:

5-methyl-3-octanone (Option C)

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Answer:

91.224 gram

Explanation:

Answer:

3.64896 grams Zr

Explanation:

Given: amount of moles of Zr: 0.040

Find: the amount of grams of Zr

1. Find molar mass of Zr

- after looking at the periodic table, you can tell it's 91.224 g/mol

2. Solve

(\(\frac{0.040 mol Zr}{1}\))( \(\frac{91.224 g Zr}{1 mol Zr}\))

- the mol units get cancelled out, and you're left with 0.040 x 91.224 g

3. Multiply that out: 3.64896 grams of zirconium

An example of heterogeneous equilibrium is:

Heterogeneous equilibrium refers to an equilibrium state in a chemical reaction where the reactants and products exist in different physical states or phases. It occurs when substances in different phases, such as solids, liquids, and gases, are involved in a chemical reaction.

Considering the given equations:

The equation I: FeO(s) + CO(g) ⇌ Fe(s) + CO₂(g) represents a heterogeneous equilibrium.

This is because the reactants and products involve different phases (solid and gas). FeO is a solid (s), CO is a gas (g), Fe is a solid (s), and CO₂ is a gas (g). The reaction involves the conversion of a solid and a gas to another solid and a gas, and the equilibrium is established between these different phases.

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true because I asked my sister

Answer:

false

Explanation:

yep

Answer:

9.43 L Br₂ (g)

Explanation:

First, write a balanced reaction equation. Then use dimensional analysis to convert from grams of aluminum chloride to moles of aluminum chloride (with molar mass from the periodic table), from moles of aluminum chloride to moles of bromine gas (using the balanced equation), and from moles of bromine gas to liters of bromine gas (remember at STP, 1 mol = 22.4 L). See the attached image for the work out. Finally, account for sig figs to get 9.43 L of bromine gas

While being made from natural resources, electricity does not constitute a natural resource because it goes through several procedures to produce it.

Oil, coke, nat gas, metals, stone, or sand are examples of natural resources. Other natural resources include water, soil, sunlight, air, and so on. Natural resources have value because they enable life and provide for human needs.

Financially referred to it as land and raw materials, land resources (also known as natural resources) are found naturally within ecosystems that are mostly unaltered by civilization. A natural resource's biodiversity levels across different habitats are frequently used to describe it.

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0.171moles

According to the ideal gas equation;

where:

• P is the, pressure ,in atm

• V is the ,volume ,in litres

• n is the ,number of moles ,of gas

• R is the, boltzmann constant

• T is the, temperature ,in Kelvin

Given the following parameters

P = 2.5atm

V = 1.67L

T = 25.0°C = 25 + 273 = 298K

R = 0.08205Latm/molK

Substitute the given parameters into the formula

Hence the amount of moles of nitrous oxide gas used is 0.171moles

Answer:

0.0032mm

Explanation:

Given dimension:

Measurement  = 3.2 x 10⁻³mm

Unknown:

Write in standard notation from scientific notation = ?

Solution:

The standard notation is the way we normally write.

   For example;   standard notation of 1 million is 1000000

Now;

        3.2 x 10⁻³  =   \(\frac{3.2}{1000}\)    = 0.0032mm

3.2x10⁻³ mm in standard notation is 0.0032 mm. The normal or generally accepted manner of representing or expressing anything is referred to as standard notation.

Standard notation refers to the conventional or widely accepted way of representing or expressing something. In mathematics, for example, standard notation refers to the commonly used symbols and formats for writing mathematical expressions, equations, or numbers. The use of standard notation ensures uniformity, ease of understanding, and communication among mathematicians and students. Powers of 10 are used in scientific notation to express extremely large or extremely small quantities. 3.2x10⁻³ mm in standard notation is 0.0032 mm.

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Answer:

Kr- Dispersion Forces

H2O- Hydrogen Bonding

CHCI3- Dipole-Dipole Forces

HF- Hydrogen Bonding

C2H6- Dispersion Forces

HBr- Hydrogen Bonding Forces

Explanation:

Dispersion forces occurs in all substances. They are the dominant intermolecular interaction in all non polar substances such as C2H6 and Kr.

Hydrogen bonding occurs when hydrogen is bonded to a highly electronegative atom such as Cl, Br, O etc. It is the dominant intermolecular interaction in HF, HBr and H2O.

Dipole-Dipole interactions occur when a permanent dipole exists in a molecule such as in CHCI3

Answer:

"[Temperature is a measurement of the average kinetic energy of the molecules in an object or a system. Kinetic energy is the energy that an object has because of its motion. The molecules in a substance have a range of kinetic energies because they don't all move at the same speed.]"

Answer:

Temperature is directly proportional to the average translational kinetic energy of molecules in an ideal gas

Explanation:

Answer:

By analyzing the potential energy diagrams and calculating ΔH using bond energies, we can determine whether a reaction is exothermic (ΔH < 0) or endothermic (ΔH > 0).

To create potential energy diagrams for chemical reactions and determine the value of ΔH (the change in enthalpy) for each reaction, we need to understand the basic concepts and steps involved.

Potential Energy Diagram: A potential energy diagram is a graphical representation of the energy changes that occur during a chemical reaction. The vertical axis represents the potential energy, while the horizontal axis represents the progress of the reaction.

Reactants and Products: Identify the reactants and products involved in each reaction. Assign them appropriate labels on the potential energy diagram.

Activation Energy: Determine the activation energy (Ea) for each reaction. It represents the energy barrier that must be overcome for the reaction to occur. On the diagram, the reactants' energy level is typically higher than the products' energy level, with the activation energy peak in between.

Transition State: Locate the highest point on the potential energy diagram, which represents the transition state or activated complex. This point indicates the highest energy level during the reaction.

ΔH Determination: ΔH represents the difference in enthalpy between the reactants and products. It can be determined by examining the vertical distance between the reactants' energy level and the products' energy level on the potential energy diagram.

ΔH Calculation: ΔH can be calculated using the formula ΔH = Σ (bond energies of reactants) - Σ (bond energies of products). The bond energies are the energy required to break a particular bond or released when a bond is formed.

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Answer:

30 ml

Explanation:

We study the reactions that chemists utilise to create bizarre carbon-based structures in organic chemistry.

The study of the makeup, properties, and responses of organic compounds including organic materials, or matter in any of its many forms that contains carbon atoms, is the subject of the branch of science known as organic chemistry. Their structural formula is determined by study of structure.

We will study the reactions that chemists utilise to create bizarre carbon-based structures in organic chemistry, in addition to the analytical techniques used to characterise them. We'll also consider the molecular reaction mechanisms that are driving those reactions.

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