Give an example of a two phase mixture and describe how you would separate the substances

Final answer:

To find the empirical formula of fructose from combustion data, calculate the moles of C from CO₂ and H from H₂O. Then, adjust for oxygen in both products to find the total oxygen. The result is a 1:2:1 ratio, giving an empirical formula of CH₂O.

Explanation:

Determining the Empirical Formula of Fructose

When 1.50 g of fructose is combusted, it produces 2.20 g of carbon dioxide (CO₂) and 0.900 g of water (H₂O). To find the empirical formula, we need to determine the amount of carbon, hydrogen, and oxygen in the original fructose sample.

Note that in each of these cases, we are assuming that all of the carbon and hydrogen in fructose end up in CO₂ and H₂O, respectively, and we adjust for the presence of oxygen in both CO₂ and H₂O to find the total oxygen in the original sample.

A molecule is formed when two or more atoms are held together by covalent bonds. These bonds are based on the sharing of electron pairs between atoms. Water (H2O) is an example of a molecule formed through covalent bonding.

When two or more atoms are held together by covalent bonds, a molecule is formed. Covalent bonds are a type of chemical bond that involves the sharing of electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs. An example of a molecule formed through covalent bonding is water (H2O), where one oxygen atom shares electron pairs with two hydrogen atoms.

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There are two types of chemical compound one is covalent compound and other is ionic compound, covalent compound formed by sharing of electron and ionic compound formed by complete transfer of electron. Therefore, the correct option is option A.

Chemical Compound is a combination of molecule, Molecule forms by combination of element and element forms by combination of atoms in fixed proportion.

An ionic compound is a metal and nonmetal combined compound.  Ionic compound are very hard. They have high melting and boiling point because of strong ion bond. The color of cobalt-oxide is blue-violet. The CoO is a metallic coloring oxide that produces blue in glazes at all temperatures.

Therefore, the correct option is option A.

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Let us assume that all gases are ideal. So we can use the formula:

PV = nRT

The reaction is:

CH4(g) + H2O(g) → CO(g) + 3H2(g)

First we determine what the limiting reactant is. This can be done by calculating for the number of moles (n) for each reactant.

For CH4:

nCH4 = (734 torr) (25.5 L) / (62.36367 L torr / mol K) (298.15 K)

nCH4 = 1 mol

For H2O:

nH2O = (704 torr) (22.6 L) / (62.36367 L torr / mol K) (398.15 K)

nH2O = 0.64 mol

Therefore H2O is the limiting reactant therefore the theoretical moles of H2 produced is:

nH2(theo) = 0.64 mol * (3 mol H2 / 1 mol H2O) = 1.92 mol

The actual moles of H2 is:

nH2(actual) = (750 torr) (26.4 L) / (62.36367 L torr / mol K) (273.15 K) = 1.16 mol

Therefore the yield is:

% yield = 1.16 / 1.92 * 100%

% yield = 60.42%

In the reaction of methane with water, each mole of methane produces three moles of hydrogen gas. Although the question is missing some key details to allow full calculations, we can infer from the provided volumes that the reactants and products are following this predicted mole ratio.

The reaction of methane with water to produce hydrogen and carbon monoxide gas is represented by the equation: CH4(g) + H2O(g) → CO(g) + 3H2(g). The question provides the volumes, pressures, and temperatures of the reactants (methane and water vapor), and asks about the volume of the produced hydrogen gas measured at STP (Standard Temperature and Pressure).

To derive the ratio of reactant quantities, we would ideally use the ideal gas law, but this question seems to be missing certain key details to perform the calculation (like the final pressure and/or temperature). However, given the balanced chemical reaction, we can say that for every mole of methane reacted, three moles of hydrogen is produced, which explains the production volume of hydrogen being greater than the initially contributed volume of methane.

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The number of oxygen atoms on the given formula  Al₂(Cr₂O₇)₃ is equal to 21.

A chemical formula can be described as a way of presenting information about the chemical proportions of atoms that are present in a particular molecule or chemical compound. The chemical formula is written by using chemical element symbols, numbers, and also other symbols, such as dashes, brackets, commas, and plus (+) and minus (−) signs.

A chemical formula contains no words but may imply certain simple chemical structures. Chemical formulae are generally more limited in power than structural formulae and chemical names.

In a chemical formula, more than one atom of the same element is represented by subscripts. In the given formula of a chemical compound Al₂(Cr₂O₇)₃ the oxygen has two subscripts that multiply with each other and the total number of oxygen atoms in the formula is 7×3 = 21.

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Mixing an Al(NO₃)₃ solution with a NaOH solution results in the formation of a white precipitate of aluminum hydroxide, Al(OH)₃. The net ionic equation for the reaction is Al³⁺(aq) + 3OH⁻(aq) → Al(OH)₃(s), showing only the ions involved in the formation of the precipitate.

When an Al(NO₃)₃ solution is mixed with a NaOH solution, a precipitate will form. This precipitate is aluminum hydroxide, Al(OH)₃. To write the net ionic equation for this reaction, we first need to consider the full molecular equation:

Al(NO₃)₃(aq) + 3NaOH(aq) → Al(OH)₃(s) + 3NaNO₃(aq)

Now, we can write the complete ionic equation, showing all the ions present in the reaction:

Al³⁺(aq) + 3NO³⁻(aq) + 3Na⁺(aq) + 3OH⁻(aq) → Al(OH)₃(s) + 3Na⁺(aq) + 3NO³⁻(aq)

The net ionic equation only shows the species that actually change during the reaction. Spectator ions (Na⁺ and NO³⁻) are not included:

Al³⁺(aq) + 3OH⁻(aq) → Al(OH)₃(s)

The statements that best describe the structure of the atom according to Rutherford's atomic model are as follows:

Ernest Rutherford was a New Zealand physicist who is known as the father of nuclear physics. He was responsible for a series of discoveries in the field of radioactivity and nuclear physics. He is also known for the discovery of positively charged sub-atomic particles known as protons.

According to Rutherford's atomic model, the positively charged sub-atomic particles are located in the middle portion of the atom which is known as the nucleus while the negatively charged sub-atomic particles are dispersed and revolving the nucleus of an atom.

Therefore, the statements that best describe the structure of the atom according to Rutherford's atomic model are briefly mentioned-above.

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Your question seems incomplete. The most probable complete question is as follows:

Rutherford’s experimental observations, which of the following statements describes the structure of the atom according to Rutherford's atomic model?

Answer is: The molecular mass of sodium oxide is A. 61.97894.

M(Na₂O) = 2 · Ar(Na) + Ar(O).

M(Na₂O) = 2 · 22.98976 + 15.9994.

M(Na₂O) = 61.97894; molecular mass of sodium oxide.

Ar is relative atomic mass (the ratio of the average mass of atoms of a chemical element to one unified atomic mass unit) of an element.

In the given question, [tex]\rm Na_2O[/tex] has a molecular mass of 61.97894 g/mol. The correct answer is option A.

The molecular mass of a compound can be determined by taking the sum of the atomic masses of all the atoms present in the molecule.

In [tex]\rm Na_2O[/tex], there are two sodium (Na) atoms with an atomic mass of 22.98977 g/mol each, and one oxygen (O) atom with an atomic mass of 15.9994 g/mol.

Molecular mass of [tex]\rm Na_2O[/tex]: [tex]2 \times 22.98977[/tex] g/mol + [tex]1 \times 15.9994[/tex] g/mol

= 61.97894 g/mol

Therefore, 61.97894 g/mol is the molecular mass of [tex]\rm Na_2O[/tex]. Option A is the correct answer.

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Water binds to each other with a strong attraction called a hydrogen bond. Water is incredibly cohesive as a result. Every day, water drops and streams provide visual proof of water's cohesion.

Not a covalent link to a hydrogen atom, hydrogen bonding is a unique kind of dipole-dipole interaction between molecules. It comes about as a result of the attraction between two extremely electronegative atoms, such as N, O, or F, and a hydrogen atom that is covalently bound to one of them.

When a highly electronegative atom's lone pair interacts with the hydrogen atom in an N-H, O-H, or F-H bond, they form a specific type of dipole-dipole interaction known as hydrogen bonding.

When a hydrogen atom that is connected to an electronegative atom moves toward another electronegative atom nearby, powerful intermolecular forces called hydrogen bonds are produced. The hydrogen bond acceptor's electronegativity will rise, resulting in a stronger hydrogen bond.

Thus, Water binds to each other with a strong attraction called a hydrogen attractive force.

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Answer: Trumpets makes the most sense

The complete balanced reaction of this neutralization reaction is:

 H2SO4  +  2NaHCO3  -->  2CO2  +  2H2O  +  Na2SO4

Then we calculate the moles of H2SO4 that was spilled:

 moles H2SO4 = 7 mole/L * 0.032 L = 0.224 mole

From the reaction, we see that 2 moles of NaHCO3 is required for every mole of H2SO4, hence:

 moles NaHCO3 = 0.224 * 2 = 0.448 mole

The molar mass of NaHCO3 is 84 g/mol. Hence the mass is:

mass NaHCO3 = 0.448 * 84

mass NaHCO3 = 37.632 grams

The minimum mass of NaHCO3 that must be added to neutralize the spilled H2SO4 is 37.632 grams.

To determine the minimum mass of NaHCO3 needed to neutralize the spilled H2SO4, we can use stoichiometry.

The balanced equation for the reaction between H2SO4 and NaHCO3 is:

H2SO4 (aq) + 2NaHCO3(aq) → Na2SO4 (aq) + 2CO2 (g) + 2H2O (l)

From the equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaHCO3. We are given the volume (32 mL) and concentration (7.0 M) of the H2SO4, so we can calculate the number of moles of H2SO4:

Moles H2SO4 = volume (L) x concentration (M) = 32 mL / 1000 mL/L x 7.0 M = 0.224 moles H2SO4

Now, we can use the stoichiometry of the reaction to calculate the minimum mass of NaHCO3 needed to neutralize the acid. Since the molar ratio of H2SO4 to NaHCO3 is 1:2, we can set up the following conversion:

0.224 moles H2SO4 x (2 moles NaHCO3/1 mole H2SO4) x (84.0 g NaHCO3/1 mole NaHCO3) = 37.632 g NaHCO3

Therefore, the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid is 37.632 grams of NaHCO3.

Final answer:

When the temperature of 10.0 grams of water decreases from 15.5°C to 14.5°C, it loses 41.84 Joules of heat, calculated using the specific heat capacity of water.

Explanation:

When the temperature of 10.0 grams of water is changed from 15.5 degrees Celsius to 14.5 degrees Celsius, the process involves a decrease in the water's thermal energy. To compute the amount of heat lost, the specific heat capacity of water is applied, which is 4.184 J/(g °C). The equation used is Q = mcΔT, where Q is the heat transferred, m is the mass of the water, c is the specific heat capacity, and ΔT is the change in temperature.

By plugging the values into the equation: Q = (10.0 g)(4.184 J/(g °C))(14.5°C - 15.5°C) = -41.84 J. This result indicates that the water loses 41.84 Joules of heat as its temperature decreases by 1 degree Celsius.

Answer:

The ratio of aluminium to sulfur is 2:3

Explanation:

The ratio of the elements of the neutral compound can be computed from the ionic charges that makes up the compound. The element that makes up the compound is aluminium and sulfur.  From the ions aluminium is the cation with a charge of 3+ . The  aluminium ion is the cations because it loses 3 electrons from the bonding between it and sulfur. The sulfur is the anion as it gains electrons from the cations.

Aluminium has a charge of 3+ and sulfur has a charge of 2- . The atom of element that makes up the neutral compound can be computed when you cross multiply the charges.

Al3+ and S2-

cross multiply the charges

Al2S3.

The ratio of aluminium to sulfur is 2:3