Calculate the amount of energy (in kJ) necessary to convert 450g of liquid water from 38°C to water vapor at 125 C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g C, and for steam is 1.99 J/g C. (Assume that the specific heat values do not change over the range of temperatures in the problem.)

Answer: \(\Delta S\) = 473.92J/K.mol

Explanation: In physics, Entropy is defined as a degree of disorder in a system. Entropy change is given by the sum of all the products multiplied by their respective coeficients minus the sum of all the reagents multiplied by their respective coeficients:

\(\Delta S = m\Sigma product - n\Sigma reagent\)

The balanced reaction:

\(H_{2}S_{(g)}+2H_{2}O_{(l)}=>3H_{2}_{(g)}+SO_{2}_{(g)}\)

gives the proportion reagents react to form products, so, if 1.6 moles of \(H_{2}S_{(g)}\):

3.2 moles of water is used;

4.8 moles of hydrogen gas is formed;

1.6 moles of sulfur dioxide is also formed;

Calculating entropy change:

\(\Delta S = (4.8*131+1.6*248.8)-(1.6*205.6+3.2*70)\)

\(\Delta S=628.8+398.08-328.96-224\)

\(\Delta S\) = 473.92J/K.mol

Entropy change for the given chemical reaction is \(\Delta S\) = 473.92J/K.mol

The correct answer is option D, It can affect the AH value.

A phase change is a physical change in a substance in which the substance's state of matter is changed, such as from a gas to a liquid or from a liquid to a solid. It is also known as a phase transition.

Phase changes also involve changes in energy, temperature, and pressure. For example, when a solid melts to become a liquid, it absorbs energy and the temperature rises. When a liquid boils to become a gas, energy is released and the temperature decreases. Similarly, when a gas condenses to become a liquid, energy is released and the pressure increases.

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Complete question is;

A certain chemical reaction 444 kj releases of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 4.68 J of heat energy to raise the temperature of this calorimeter by 6.9 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by . How would you calculate the number of moles of reactant that were consumed

Answer:

7.27 × 10^(-5) moles

Explanation:

We are given;

Heat energy = 444 kJ/mol

Final Temperature = 6.9 °C

Heat capacity = 4.68 J/°C

Let's calculate the heat generated from the formula;

Heat generated = heat capacity × final temperature

Heat generated = 4.68 × 6.9 = 32.292 J = 32.292 × 10^(-3) KJ

Now, the number of moles of reactant that were consumed is gotten from;

No_ of moles of rctnt consumed = heat energy generated/heat energy used = (32.292 × 10^(-3))/444 = 7.27 × 10^(-5) moles

The name of the metal ion is sodium (Na+).

The name of the nonmetal ion is chlorine (Cl-).

Add them together and drop "ion"s to find the name of the compound is: sodium chloride.

Answer:

2812.6 g of H₂SO₄

Explanation:

From the question given above, the following data were obtained:

Mole of H₂SO₄ = 28.7 moles

Mass of H₂SO₄ =?

Next, we shall determine the molar mass of H₂SO₄. This can be obtained as follow:

Molar mass of H₂SO₄ = (1×2) + 32 + (16×4)

= 2 + 32 + 64

= 98 g/mol

Finally, we shall determine the mass of H₂SO₄. This can be obtained as follow:

Mole of H₂SO₄ = 28.7 moles

Molar mass of H₂SO₄ =

Mass of H₂SO₄ =?

Mole = mass / Molar mass

28.7 = Mass of H₂SO₄ / 98

Cross multiply

Mass of H₂SO₄ = 28.7 × 98

Mass of H₂SO₄ = 2812.6 g

Thus, 28.7 mole of H₂SO₄ is equivalent to 2812.6 g of H₂SO₄

Answer:

B<Ga<Al

Explanation:

Hope this helps

Answer:

4 mol KOH

Explanation:

Step 1: Write the balanced neutralization reaction.

H₂SO₄(aq) + 2 KOH(aq) ⇒ 2 H₂O(l) + K₂SO₄(aq)

Step 2: Establish the appropriate molar ratio

According to the balanced equation, the molar ratio of H₂SO₄to KOH is 1:2.

Step 3: Calculate the number of moles of KOH needed to react with 2 moles of H₂SO₄

We will use the previously established molar ratio.

2 mol H₂SO₄ × 2 mol KOH/1 mol H₂SO₄ = 4 mol KOH

If a strong base is added to a buffer the pH will change only slightly. In the non-buffered solution changing the pH significantly.

If a strong base is added to a buffer, the weak acid will give up its H+ in order to transform the base (OH-) into water (H2O) and the conjugate base: HA + OH- → A- + H2O. Since the added OH- is consumed by this reaction, the pH will change only slightly.

In the non-buffered solution, the added hydronium or hydroxide ions have nothing to react with so the concentrations increase rapidly, changing the pH significantly.  If a base is added to an acidic solution, the solution becomes less acidic and moves toward the middle of the pH scale.

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Answer:

The value is \(k =66\%\)

Explanation:

From the question we are told that

The mass of toluene \( m_t =0.73 \ g \)

The mass of potassium permanganate is \( m =2.0 \ g \)

The volume of potassium hydroxide V = 7.0 mL

The concentration of potassium hydroxide C = 6 M

The mass of benzoic acid is \(m_b = 0.633 \ g\)

Generally the % yield of benzoic acid is mathematically represented as

\(k = \frac{m_b}{Z} * 100\)

Here Z is the theoretical yield which is mathematically represented as

\(Z = \frac{E}{W} * m_t \)

Here W is the molecular weight of product (benzoic acid) with value  

       W  = 92.14 \ g

E is the molecular weight of reactant (toluene)with a constant value  of  

    E =  122.12 g

So

     \(Z =  \frac{122.12 }{92.14}  *  0.73 \)

=>    \(Z = 0.968 \  g  \)

So

     \(k  =  \frac{0.633}{0.968}  * 100\)

=>   \(k  =66\%\)

Answer:

? more info

Explanation:

Give users an example of the reactions you've learned about so we can have more of an idea. I'd be glad to help, if you edited your answer, meanwhile I too have homework in need of finishing.

Answer:

support the plant

hold leaves and buds

store food

In the Dieckmann reaction, the diester undergoes a cyclization reaction to form a beta-keto ester. Two beta-keto esters are formed, one from the carboxyl group at the end of the chain, and one from the carboxyl group at the middle of the chain.

Cyclization is started by the production of a putative cation, typically from a sp3-hybridized carbon, either by electrophilic addition to a double bond or by ionization.

The most frequent cyclization processes take place when an electrophile and a nucleophile interact. Consequently, the following are the most common reaction types: the nucleophilic change in a carbon atom that is saturated. addition by nucleophiles to an unsaturated carbon. Atomic addition-removal nucleophilic.

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The result of the reaction between 2.2 g of Al and 1.8 g of O2 is the formation of 3.89 g of \(Al_{2} O_{3}\).

The given masses of Al and \(O_{2}\) are in a ratio of approximately 1:1. Therefore, we can assume that all the Al reacts with all the O2, and use stoichiometry to determine the products and reactants involved.

The balanced chemical equation for the reaction between Al and O2 is:

                                       4 Al + 3 \(O_{2}\) → 2 \(Al_{2} O_{3}\)

Using the molar masses of Al (26.98 g/mol) and \(O_{2}\) (32.00 g/mol), we can convert the given masses into moles:-

2.2 g Al × (1 mol Al/26.98 g Al) = 0.0815 mol Al

1.8 g \(O_{2}\) × (1 mol \(O_{2}\)/32.00 g \(O_{2}\)) = 0.0563 mol \(O_{2}\)

From the balanced chemical equation, we can see that 4 moles of Al react with 3 moles of \(O_{2}\) to produce 2 moles of Al2O3. Therefore, the limiting reactant is \(O_{2}\), since there are fewer moles of \(O_{2}\) than required by the stoichiometry of the reaction.

Using the mole ratio from the balanced chemical equation, we can determine the amount of \(Al_{2} O_{3}\) produced:

0.0563 mol \(O_{2}\) × (2 mol \(Al_{2} O_{3}\)/3 mol \(O_{2}\)) × (101.96 g Al2O3/mol) = 3.89 g \(Al_{2} O_{3}\).

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The change in enthalpy when 3 moles of methane react in excess oxygen is -2.67 × 10³ kJ (Option B).

Enthalpy (H) is a thermodynamic property that describes the total heat content of a system at a constant pressure. It is a measure of the energy that is transferred as heat during a chemical reaction or physical change at constant pressure.

Enthalpy is defined mathematically as:

H = U + PV

where U is the internal energy of the system, P is the pressure, and V is the volume. Enthalpy is often measured in units of Joules (J) or kilojoules (kJ).

The given reaction is:

CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) ΔH = -890 kJ

This equation shows that when one mole of methane reacts with two moles of oxygen, it produces one mole of carbon dioxide and two moles of water while releasing 890 kJ of energy.

To determine the change in enthalpy when 3 moles of methane react in excess oxygen, we need to first calculate the amount of heat released when one mole of methane reacts with excess oxygen.

From the balanced chemical equation, we can see that 1 mole of CH4 releases 890 kJ of energy, so the energy released by 3 moles of CH4 would be 3 times that value:

Energy released by 3 moles of CH4 = 3 × (-890 kJ/mol) = -2670 kJ

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The change in enthalpy when 3 moles of methane react in excess oxygen is -2670 kJ.

What is Enthalpy?

Enthalpy is a thermodynamic property of a system that describes the heat content of the system at constant pressure. It is denoted by the symbol "H" and is expressed in units of joules (J) or kilojoules (kJ). Enthalpy is a state function, which means that it depends only on the initial and final states of the system, not on the path taken to reach those states.

The given reaction is: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l), ΔH = −890 kJ

This reaction is for one mole of methane. To find the change in enthalpy when 3 moles of methane react, we need to multiply the enthalpy change by 3:

ΔH = 3 × (-890 kJ/mol) = -2670 kJ

Therefore, the change in enthalpy when 3 moles of methane react in excess oxygen is -2670 kJ.

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Answer:

0.233682161601125

Explanation:

Answer:

1. Dehydration of alcohols

2. Dehydrohalogenation of alkyl halides

3. Decarboxylation of carboxylic acids

4. Pyrolysis of esters

5. Deamination of amino acids

6. Dealkylation of ethers

7. Dehalogenation of aryl halides

8. Dehydration of amides

9. Dehydrogenation of alkanes

10. Dehydrogenation of alkenes.

Explanation:

Single atoms should be done last.

Balancing chemical equations involves trial and error.

Chemical equations are known to be balanced if the total number of elements on the reactant side is equal to the total elements on the product side.

Balancing of chemical equations may not be determined at once, hence the use of trial and method is crucial.

Also, atoms that are in only one of the reactants and only one of the products should be done first while single atoms should be done last.

Based on the information below . The atoms of the same element are Atom A and Atom C .

Atoms of same element have the same atomic number. so the number of protons and electron are same but they have different atomic masses called as Isotopes.  so, the atoms having different number of neutron will have different masses.

In the given case ,

Atom A               Atom B             Atom C

8 protons           10 protons        8 protons

8 neutrons         10 neutrons       10 neutrons

8 electrons         10 electrons      8 electrons

so, In Atom A  and Atom C , the number of protons and electrons are same but  the have different atomic masses means having different no. of neutrons. so Atom A and Atom C are the atoms of same elements.

Hence,Based on the information below . The atoms of the same element are Atom A and Atom C.

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Answer:

Isomers of hydrocarbons have the molecular formula but structural formula.

Explanation:

Molecules with the same structural formula, but different molecular geometries (spatial arrangement) are called isomers. These differences in the arrangement of the various atoms confer certain differences in chemical properties to the resulting hydrocarbons, even though their chemical composition is the same. There are two types of isomers:

Structural isomers: Here, each atom are connected or bonded in different ways, hence structural isomers may contain different functional groups or pattern of bonding. structural isomers are further divided into: chain, position, and functional group isomers.

Stereoisomers: Here, the connections of the atoms are the same, but the difference is in their orientation in space

The change in the internal energy of the system is +69 J, indicating that the system has gained energy.

The change in internal energy of the system can be calculated using the First Law of Thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system on its surroundings.

In this case, the system receives 57 J of energy as heat, which means that the heat is added to the system, and the value is positive (+57 J). On the other hand, the system does 12 J of work on the surroundings, which means that the work is done by the system, and the value is negative (-12 J).

Using the First Law of Thermodynamics, we can calculate the change in internal energy of the system as:

ΔU = Q - W

ΔU = (+57 J) - (-12 J)

ΔU = 69 J

Therefore, the change in the internal energy of the system is +69 J, indicating that the system has gained energy.

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The volume of \(N_2O_5\) needed to produce 9.64 L of \(NO_2\) is 4.97 L, calculated using stoichiometry and the ideal gas equation.

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De Broglie contributed to the development of the modern model of atoms by describing the wave properties of particles. Option E.

Louis de Broglie was a French physicist who made significant contributions to the development of quantum mechanics.

In his doctoral thesis, he proposed that particles, such as electrons, have both particle-like and wave-like properties. This idea became known as wave-particle duality and laid the foundation for the development of the modern model of the atom.

According to de Broglie's theory, particles can exhibit wave-like behavior and have a wavelength that is inversely proportional to their momentum.

This theory was later experimentally confirmed in a series of experiments that demonstrated the diffraction of electrons and other particles.

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Answer : The net ionic equation will be,

\(Ba^{2+}(aq)+SO_4^{2-}(aq)\rightarrow BaSO_4(s)\)

Explanation :

In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

The given balanced ionic equation will be,

\(Ba(OH)_2(aq)+H_2SO_4(aq)\rightarrow 2H_2O(aq)+BaSO_4(s)\)

The ionic equation in separated aqueous solution will be,

\(Ba^{2+}(aq)+2OH^-(aq)+2H^{+}(aq)+SO_4^{2-}(aq)\rightarrow BaSO_4(s)+2H^+(aq)+2OH^{-}(aq)\)

In this equation, \(H^+\text{ and }OH^-\) are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

\(Ba^{2+}(aq)+SO_4^{2-}(aq)\rightarrow BaSO_4(s)\)

The temperature in kelvin (K) in which the reaction occurs spontaneously is given as  349 K

Entropy is simply defined as the measure of the degree of the disorderliness of a system. Mathematically, it can be expressed as:

ΔS = ΔH / T

Where

ΔS = ΔH / T

1.64 = 573 m T

Cross multiply

1.64 × T = 573

Divide both side by 1.64

T = 573 / 1.64

T = 349 K

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The average atomic mass of her sample is 114.54 amu

Let the 1st isotope be A

Let the 2nd isotope be B

From the question given above, the following data were obtained:

The average atomic mass of the sample can be obtained as follow:

\(Average \: atomic \: mass \: = \frac{mass \: of \: A \times A\%}{100} + \frac{mass \: of \: B \times B\%}{100} \\ \\ Average \: atomic \: mass \: = \frac{113.6459\times 59.34}{100} + \frac{115.8488\times 40.66}{100} \\ \\ Average \: atomic \: mass \: = 114.54 \: amu \\ \\ \)

Thus, the average atomic mass of the sample is 114.54 amu

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Answer:

Explanation: