why are different products obtained when molten and aqueous nacl is electrolyzed

In compound A, the best leaving group is the O –OH group, and the worst leaving group is the –OH group.

The correct ranking from best to worst leaving group is O –OH, > –NH, > –OH.

To explain this step-by-step:

1. A good leaving group is one that can easily dissociate from the molecule, stabilizing the negative charge it acquires upon leaving.
2. The O –OH group, being an alkoxide ion, is a better leaving group because it can stabilize the negative charge through resonance.
3. The –NH group is the next best leaving group, as it can somewhat stabilize the negative charge through its lone pair of electrons.
4. Finally, the –OH group is the worst leaving group among the given options, as it is less capable of stabilizing the negative charge upon leaving the molecule.

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The addition of hydrogen (H2/Pt) to alkenes takes place with syn stereospecificity, meaning that the two hydrogen atoms are added to the same side of the double bond. Therefore, the correct answer is d. Hydrogenation (H2/Pt).

The other reactions listed do not have stereospecificity:a. Addition of HBr results in the formation of both the syn and anti addition products, meaning that the H and Br can add to either the same side or opposite sides of the double bond.b. Acid-catalyzed hydration (H2O/H2SO4) also does not have stereospecificity because the water molecule can add to either side of the double bond, leading to the formation of both the syn and anti addition products.

c. Addition of bromine (Br2) also does not have stereospecificity, as the two Br atoms can add to either side of the double bond, leading to the formation of both the syn and anti addition products.

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There are created around 125.8 grammes of magnesium metal.

By running electricity through molten magnesium chloride, magnesium metal may be produced. At the cathode, magnesium metal is produced, and at the anode, chlorine gas is developed. Therefore, the appropriate metal is formed at the cathode during the electrolytic reduction of molten salts (the negative electrode).

moles of substance = (electric charge in coulombs) / (Faraday's constant)

where Faraday's constant is the amount of electric charge carried by one mole of electrons, which is 96,485 C/mol.

electric charge = current x time = 65.7 A x 4.50 hr x 3600 s/hr = 1.00 x 10⁶ C

Next, we can calculate the moles of magnesium produced:

moles of Mg = electric charge / (Faraday's constant x 2)

(we divide by 2 because the balanced equation shows that 2 electrons are required to produce 1 mole of Mg)

moles of Mg = 1.00 x 10⁶ C / (96,485 C/mol x 2) = 5.18 mol

Finally, we can calculate the mass of magnesium produced using its molar mass, which is 24.31 g/mol:

mass of Mg = moles of Mg x molar mass of Mg

mass of Mg = 5.18 mol x 24.31 g/mol = 125.8 g

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The reason why acetyl chloride reacts with water almost violently, but you have to warm and shake the mixture of water and benzoyl chloride is due to the difference in their reactivity and molecular structure.

Acetyl chloride (CH3COCl) is a more reactive compound than benzoyl chloride (C6H5COCl). This higher reactivity is due to the presence of an electron-donating methyl group (CH3) in acetyl chloride, which increases the electrophilicity of the carbonyl carbon (C=O) and makes it more susceptible to nucleophilic attack by water.

On the other hand, benzoyl chloride has an electron-withdrawing phenyl group (C6H5), which reduces the electrophilicity of the carbonyl carbon, making it less reactive towards nucleophilic attack by water.

As a result, acetyl chloride reacts with water almost violently, forming acetic acid (CH3COOH) and hydrogen chloride (HCl) gas. In contrast, benzoyl chloride requires warming and shaking to facilitate the reaction with water, ultimately producing benzoic acid (C6H5COOH) and hydrogen chloride (HCl) gas.

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Explanation:

pH+pOH=14

pH=14-pOH

=14-5.039e-3

=13.9

The pH after the addition of 38.0 mL of 0.50 M KOH to the 76.0 mL of 0.25 M HBr is 7.

To find the pH after the addition of 38.0 mL of 0.50 M KOH to the 76.0 mL of 0.25 M HBr:

1. Calculate the moles of HBr and KOH before the reaction.
2. Determine the limiting reactant and the remaining moles of the excess reactant.
3. Calculate the concentration of the remaining reactant.
4. Determine the pH using the concentration of the remaining reactant.

Calculate moles of HBr and KOH
Moles of HBr = volume (L) × concentration (M)
Moles of HBr = 0.076 L × 0.25 M = 0.019 moles

Moles of KOH = volume (L) × concentration (M)
Moles of KOH = 0.038 L × 0.50 M = 0.019 moles

Determine the limiting reactant
In this case, both HBr and KOH have the same moles (0.019 moles), so they will react completely with each other, leaving no excess reactant.

Calculate the concentration of the remaining reactant
Since both reactants have been completely consumed in the reaction, there are no remaining reactants. The reaction produces the salt KBr and water.

Determine the pH
As there are no remaining acidic or basic reactants in the solution, the pH of the resulting solution is neutral, with a pH of 7.

Therefore, 7 is the pH after the addition of 38.0 mL of 0.50 M KOH to the 76.0 mL of 0.25 M HBr.

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The Keg for the overall reaction is [tex]2.01 x 10^21[/tex]. Once the concentration of ammonia (aq) in the solution has been determined, the equilibrium constant Keg for the entire process can be computed using equation.

Temperature-dependent The quantity of a reaction, the presence of a catalyst, or the presence of inert materials have no impact on equilibrium constants. It is also unaffected by the amounts, pressures, or concentrations of the reactants. The equilibrium constant's degree of temperature dependence is, in general, determined by the reaction.

The equilibrium constant is temperature-dependent and unaffected by the precise ratios of reactants to products, the presence of a catalyst, or the presence of inert substances. The volumes, pressures, and concentrations of the reactants and products have no impact on it either.

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The statement "Draw an arrow pushing mechanism for the formation of the acylium ion when acetic anhydride reacts with phosphoric acid" is true.

To draw an arrow pushing mechanism for the formation of the acylium ion when acetic anhydride reacts with phosphoric acid, follow these steps:

1. Draw the structures of acetic anhydride and phosphoric acid.

2. Locate the electrophilic carbonyl carbon in acetic anhydride and the nucleophilic oxygen atom in phosphoric acid.

3. Draw an arrow from the lone pair of electrons on the oxygen atom of phosphoric acid to the electrophilic carbonyl carbon in acetic anhydride, indicating nucleophilic attack.

4. Draw an arrow from the pi bond between the carbonyl carbon and oxygen in acetic anhydride to the carbonyl oxygen, representing the movement of electrons and formation of a negatively charged oxygen atom.
5. Draw the intermediate structure formed after the nucleophilic attack.

6. Draw an arrow from the negatively charged oxygen atom to reform the carbonyl double bond and simultaneously break the carbon-oxygen bond adjacent to the carbonyl carbon, pushing electrons to the neighboring oxygen atom.

7. Draw the final acylium ion and byproduct formed in the reaction.

This mechanism illustrates how the acylium ion is formed when acetic anhydride reacts with phosphoric acid.

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The proper IUPAC names of tert-Butyl alcohol is 2-methylpropan-2-ol and of tert-Butyl chloride is 2-chloro-2-methylpropane.

The common names, tert-butyl alcohol and tert-butyl chloride, can be represented by their proper IUPAC names as follows:

1. tert-Butyl alcohol, also known as tert-butanol, has the IUPAC name 2-methylpropan-2-ol. This name is derived from its structure, where a methyl group (CH3) is attached to the second carbon of a three-carbon chain (propane). The alcohol functional group (-OH) is also attached to the second carbon, hence the "-2-ol" suffix.

2. tert-Butyl chloride, also known as tert-butylchloride or t-BuCl, has the IUPAC name 2-chloro-2-methylpropane. Similar to the alcohol, its structure consists of a methyl group (CH3) attached to the second carbon of a three-carbon chain (propane). Instead of an alcohol functional group, there is a chlorine atom (Cl) attached to the same second carbon, hence the "2-chloro" prefix in the name.

These IUPAC names provide a more systematic and descriptive way to identify the chemical structures of these compounds compared to their common names.

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The standard enthalpy change for the reverse reaction is the negative of the given enthalpy change. Therefore, the standard enthalpy change for the reaction  K(s) + 1/2 I2(s) → KI(s) is -656 kJ at 328K.

To find the standard enthalpy change for the given reaction at 298 K, we can manipulate the original reaction and divide its enthalpy change by 2.

The original reaction is:
2 KI(s) → 2 K(s) + I2(s) ΔH° = 656 kJ

Divide the entire reaction by 2:
KI(s) → K(s) + 1/2 I2(s)

Now, divide the enthalpy change by 2:
ΔH° = 656 kJ / 2 = 328 kJ

So, the standard enthalpy change for the reaction K(s) + 1/2 I2(s) → KI(s) at 298 K is 328 kJ.

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An ambidentate ligand is a type of ligand that can bond through two different atoms or groups in the same molecule.

An ambidentate ligand is a ligand that can bind to a central metal atom/ion through two different donor atoms present within the same molecule, but only one donor atom can bind at a time. This means that it can bond to a metal ion through either of these two atoms or groups. Two examples of ambidentate ligands, other than NO2, are:

1. SCN- (thiocyanate): This ligand can bind to the metal through either the sulfur (S) or the nitrogen (N) atom.
2. OCN- (cyanate): This ligand can bind to the metal through either the oxygen (O) or the nitrogen (N) atom.

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A minimum of 25.6 mL of 3.5 M HI is needed to thoroughly dissolve 2.42 g of silver.

The less active metals, including zinc and magnesium, are easily dissolved by hydrochloric acid. Iron, copper, and other harder metals are less easily or completely disintegrated by it. While hydrochloric acid won't dissolve some metals, other chemicals, such nitric acid, will.

The chemical equation for the reaction of copper with HI is balanced as follows:

Cu(s) + 2HI(aq) → CuI2(aq) + H2(g)

The following formula can be used to determine the minimum volume of 3.5 M HI needed to completely dissolve 4.85 g Cu:

Moles of Cu = 4.85 g / 63.55 g/mol = 0.0763 mol

Moles of HI required = 2 × moles of Cu = 0.1526 mol

Volume of 3.5 M HI required = moles of HI required / 3.5 M = 0.0436 L or 43.6 mL

Therefore, 43.6 mL of 3.5 M HI is the lowest amount needed to thoroughly dissolve 4.85 g of copper. The chemical equation for the silver-HI reaction is balanced as follows:

2Ag(s) + 4HI(aq) → 2AgI(s) + 2H2(g)

The following formula can be used to determine the minimum volume of 3.5 M HI needed to completely dissolve 2.42 g of Ag:

Moles of Ag = 2.42 g / 107.87 g/mol = 0.0224 mol

Moles of HI required = 4 × moles of Ag = 0.0896 mol

Volume of 3.5 M HI required = moles of HI required / 3.5 M = 0.0256 L or 25.6 mL

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The theoretical yield of NaCl when you mix 2.00g of Na2CO3 is 2.21g.  Use the balanced equation's stoichiometry to determine the NaCl moles produced. To calculate the theoretical yield of NaCl when mixing 2.00g of Na2CO3, we need to first consider the balanced chemical equation for the reaction between Na2CO3 and HCl:

Na2CO3 + 2HCl -> 2NaCl + CO2 + H2O

This equation shows that one mole of Na2CO3 reacts with two moles of HCl to produce two moles of NaCl. We can use this information to calculate the theoretical yield of NaCl by following these steps:

1. Convert 2.00g of Na2CO3 to moles by dividing by its molar mass (105.99 g/mol).

2. Use stoichiometry to determine the moles of NaCl produced. Since the reaction produces two moles of NaCl for every mole of Na2CO3, we can multiply the moles of Na2CO3 by 2 to get the moles of NaCl.

3. Convert the moles of NaCl to grams by multiplying by its molar mass (58.44 g/mol).

The calculation looks like this:

2.00g Na2CO3 x (1 mol Na2CO3/105.99 g Na2CO3) x (2 mol NaCl/1 mol Na2CO3) x (58.44 g NaCl/1 mol NaCl) = 2.78g NaCl (theoretical yield)

Therefore, the theoretical yield of NaCl when mixing 2.00g of Na2CO3 is 2.78g.

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As a buffer, ammonium acetate in water can be used. Ammonium acetate is a salt solution that can function as a buffer by itself.

As we now know, p K a ​=−logK a K a =1.34 x 10 -5 (Given) pK a =log(1.34 x 10 - 5) pK a =5 x 0.127 =4.873 pH is now calculated as pH=pK a + log( [acid] [salt] )

Given:- [salt]=[acid]=0.5M ∴pH=4.87+log

0.5 0.5​=4.873

As a result, the solution's pH is 4.873.

Drive Me Tile Online has a concentration of 0.075 and Try Metal Ammonium Chloride has a concentration of 0.13 M I.

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The ways that the brightness of the flame can be increased are shown below.

By boosting the airflow into the burner, the flame's brilliance can be improved. Increasing the gas flow rate or changing the air intake valve can do this.

Using a gas that generates a brighter flame, like propane or butane, will increase the brightness of the flame. These gases produce a yellow flame because they have a higher carbon to hydrogen ratio than natural gas.

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If all the mitochondria within intestinal cells were destroyed, glucose absorption would decrease.

If all the mitochondria within the intestinal cells were destroyed, glucose absorption would decrease due to the lack of ATP production. Active transport is responsible for the absorption of glucose in intestinal cells, and this process requires energy in the form of ATP. Mitochondria are the main organelles responsible for ATP production in cells, and without them, the energy supply for active transport would be insufficient. This would lead to a decrease in glucose absorption by the intestinal cells. Since glucose is an important source of energy for the body, reduced glucose absorption can have negative consequences on the overall health and well-being of an individual.

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The concentration of Allura Red in the undiluted unknown is 0.00556 mg/mL.

To determine the concentration of Allura Red in the undiluted unknown, we can use the diluted equation, which relates the concentration of the diluted solution with the concentration of the undiluted solution, as well as the dilution factor:

C1V1 = C2V2

where:

C1 is the concentration of the undiluted solution (what we want to find)

V1 is the volume of the undiluted solution

C2 is the concentration of the diluted solution (known)

V2 is the volume of the diluted solution (known)

the dilution factor is V1/V2

Assuming we know the concentration and volume of the diluted solution, as well as the dilution factor, we can rearrange the diluted equation to solve for the concentration of the undiluted solution:

C1 = C2 x V2/V1

Let's say we have a diluted solution of Allura Red with a concentration of 0.05 mg/mL and a volume of 10 mL, and we diluted it 1:10 (meaning we added 90 mL of solvent to make a total volume of 100 mL). We can use the diluted equation to calculate the concentration of Allura Red in the undiluted solution:

C1 = 0.05 mg/mL x 10 mL / 90 mL

C1 = 0.00556 mg/mL

Therefore, the concentration of Allura Red in the undiluted unknown is 0.00556 mg/mL.

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The greener choice in a chemical process between a reaction that can be run at 300 K for 1 hour with a catalyst (Option A).

In terms of green chemistry, the reaction that can be run at 300 K for 1 hour with a catalyst is the greener choice. This is because using a catalyst can increase the reaction rate and efficiency, thus reducing the amount of energy and resources needed to run the reaction. Additionally, running the reaction at a lower temperature can reduce energy consumption and decrease the carbon footprint of the process. Overall, using a catalyst and optimizing reaction conditions for efficiency and sustainability is a key aspect of green chemistry.

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2 NH₄⁺(aq) + 3 Zn²⁺(aq) + 2 PO₄³⁻(aq) → Zn₃(PO₄)₂(s) + 6 NH₄⁺(aq) is the net ionic equation.

The balanced net ionic equation for the reaction when aqueous (NH₄)₃PO₄ and aqueous Zn(NO₃)₂ are mixed in solution to form solid Zn₃(PO₄)₂ and aqueous NH₄NO₃ is:

2 NH₄⁺(aq) + 3 Zn²⁺(aq) + 2 PO₄³⁻(aq) → Zn₃(PO₄)₂(s) + 6 NH₄⁺(aq)

The nitrate ions (NO₃⁻) do not participate in the reaction and are therefore not included in the net ionic equation. Additionally, the ammonium ions (NH₄⁺) are spectator ions and are therefore also not included in the net ionic equation.

Therefore, The phases for each species in the equation are:

NH₄⁺(aq) - ammonium ion, aqueous

Zn²⁺(aq) - zinc ion, aqueous

PO₄³⁻(aq) - phosphate ion, aqueous

Zn₃(PO₄)₂(s) - zinc phosphate, solid

NH₄⁺(aq) - ammonium ion, aqueous

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Answer:

2) It is less than before the tax was imposed.

A portion of the tax that is levied on a commodity must be paid by the seller, which lowers their profit margin. Sellers will raise the cost of the good and pass this cost onto purchasers in order to preserve their profit. This causes the market price that buyers must pay to rise as a result of taxation.

To determine the most effective buffer made by HNO2 and NaNO2 with a pH of 3.15, we need to calculate the ratio of the concentrations of the conjugate acid-base pair (HNO2 and NO2-) that will give the desired pH.

The pH of the buffer solution can be calculated using the Henderson-Hasselbalch equation:

pH = pKa + log([A-]/[HA])

where pKa is the acid dissociation constant of the weak acid, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid.

Substituting the given values:

pH = -log(7.11 x 10^-4) + log([NO2-]/[HNO2])

3.15 = 3.15 + log([NO2-]/[HNO2])

log([NO2-]/[HNO2]) = 0

[NO2-]/[HNO2] = 1

Therefore, the most effective buffer will be made by mixing HNO2 and NaNO2 in a 1:1 molar ratio. This will give a pH of 3.15 and will be able to resist changes in pH when small amounts of acid or base are added to the solution.

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The element in period 3 with successive ionization energies (IE1 = 578, IE2 = 1820, IE3 = 2740, IE4 = 11,500, and IE5 = 13,000) is Magnesium (Mg).

The very minimum energy required to remove one electron from a gaseous atom in isolation is referred to as ionization energy. Because these atoms are more stable and have orbitals that are partially and completely occupied, it takes more energy to remove an electron from them. In the case of such atoms, the ionization enthalpy is thus larger than the expected value.

To identify the element in period 3 with the successive ionization energies (IEs) in kJ/mol (IE1 = 578, IE2 = 1820, IE3 = 2740, IE4 = 11,500, and IE5 = 13,000), we need to follow these steps:

1. Locate the period 3 elements on the periodic table. Period 3 elements are those in the third row, and they include Na, Mg, Al, Si, P, S, and Cl.
2. Compare the given ionization energies with the known ionization energies of the period 3 elements.

After comparing the given ionization energies with the known values, we can identify the element as Magnesium (Mg).
The element in period 3 with successive ionization energies (IE1 = 578, IE2 = 1820, IE3 = 2740, IE4 = 11,500, and IE5 = 13,000) is Magnesium (Mg).

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The molar mass of P4 is 4 times the molar mass of a single phosphorus atom, which is approximately 30.974 g/mol. Therefore, the molar mass of P4 is: there are 8.41 x [tex]10^{23}[/tex] phosphorus atoms present in 0.350 mol of P4.

4 x 30.974 g/mol = 123.896 g/mol

To calculate the number of moles of P4 in 0.350 mol, we can use the following equation:

moles = mass / molar mass

mass = moles x molar mass

mass of P4 = 0.350 mol x 123.896 g/mol = 43.3676 g

Since each P4 molecule contains 4 phosphorus atoms, we can calculate the total number of phosphorus atoms in 0.350 mol of P4 as follows:

number of P atoms = number of P4 molecules x 4

number of P atoms = 0.350 mol x 6.022 x 10^23 molecules/mol x 4 atoms/molecule

number of P atoms = 8.41 x [tex]10^{23}[/tex] atoms

Therefore, there are 8.41 x [tex]10^{23}[/tex] phosphorus atoms present in 0.350 mol of P4.

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Comparing the amounts of product produced, we can see that reactant B produces the least amount of product (0.30 mol of D), while reactants A and C produce more than that. Therefore, reactant B is the limiting reactant in this scenario.

To determine the limiting reactant, we need to compare the amount of each reactant to the stoichiometric coefficients in the balanced equation. The reactant that produces the least amount of product, or runs out first, is the limiting reactant.

Let's start by calculating the amount of product that each reactant can produce:

For reactant A:
- 0.20 mol A produces 2 × 0.20 mol = 0.40 mol of D
- 0.20 mol A produces 1 × 0.20 mol = 0.20 mol of E

For reactant B:
- 0.60 mol B produces 1/2 × 0.60 mol = 0.30 mol of D
- 0.60 mol B produces 1/3 × 0.60 mol = 0.20 mol of E

For reactant C:
- 0.75 mol C produces 1/3 × 0.75 mol = 0.25 mol of D
- 0.75 mol C produces 1/3 × 0.75 mol = 0.25 mol of E

The limiting reactant is the one that produces the least amount of product. Comparing the amounts of product produced, we can see that reactant B produces the least amount of product (0.30 mol of D), while reactants A and C produce more than that. Therefore, reactant B is the limiting reactant in this scenario.

So the answer is (E) B only.

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When an action potential reaches a neuromuscular junction, it triggers the release of acetylcholine into the synaptic cleft.

The acetylcholine then binds to the nicotinic receptors, which are concentrated on the motor end plate of the muscle fiber's post-synaptic membrane. This binding causes the opening of ion channels and the influx of positively charged ions, which results in depolarization of the muscle fiber's membrane. This depolarization then spreads through the muscle fiber, ultimately leading to muscle contraction. The action of acetylcholine at the neuromuscular junction is critical for normal muscle function and is targeted by many drugs used to treat neuromuscular disorders.

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As scientific knowledge and technology advance, instrumentation also changes and evolves to better support scientific research and experimentation.

What is Science?

Science is a systematic and evidence-based approach to studying the natural world, including physical, biological, and social phenomena. It involves formulating hypotheses, conducting experiments, and analyzing data to generate knowledge and understanding about how the world works.

Advances in fields such as materials science, electronics, and computing have allowed for the development of more sophisticated and precise instruments, leading to new discoveries and greater understanding of the natural world.

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An ambidentate ligand is a ligand that can bind to a metal ion (M) through two different donor atoms.

Two examples of ambidentate ligands (other than NO₂) are SCN⁻ and NCS⁻. SCN⁻ can bind through the sulfur atom (S) or the nitrogen atom (N), forming [M-SCN] or [M-NCS] complexes. The IUPAC names for these ligands are thiocyanato (SCN⁻) and isothiocyanato (NCS⁻).

A polydentate ligand is a ligand that can bind to a metal ion (M) through multiple donor atoms simultaneously. Two examples are ethylenediamine (en) and ethylenediaminetetraacetic acid (EDTA).

The chelate effect occurs when a polydentate ligand forms a ring with a metal ion, which stabilizes the complex and lowers its overall energy. The IUPAC names for these ligands are ethane-1,2-diamine (en) and (ethylenedinitrilo)tetraacetate (EDTA).

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Tetrodotoxin blocks sodium channels, which prevents the influx of sodium ions and inhibits the generation and propagation of action potentials, leading to a loss of excitatory conduction in neurons.

Sodium channels are responsible for the rapid depolarization phase of the action potential in neurons. When an action potential is initiated, voltage-gated sodium channels open and allow an influx of sodium ions into the neuron, which depolarizes the membrane potential and triggers the propagation of the action potential down the axon.

Tetrodotoxin works by binding to the extracellular pore of the sodium channel and blocking the flow of sodium ions through the channel. This prevents the rapid depolarization of the membrane potential, which is necessary for the generation of action potentials. As a result, neurons are unable to generate action potentials and their ability to conduct electrical impulses is greatly diminished.

In summary, tetrodotoxin inhibits excitatory conduction in neurons by blocking sodium channels and preventing the generation and propagation of action potentials. This can lead to a range of neurological symptoms, including muscle weakness, paralysis, and respiratory failure, and can be fatal in high enough doses.

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To make sweet tea, a cook dissolved 152.395 grams of sugar  in 5.19 l of water at 32.34 °c. The molality of this sugar solution 0.275 mol/kg

To find the molality of the sugar solution, we need to first calculate the moles of sugar and the mass of solvent (water) in kilograms:

We know that molar mass of sugar= 110 g/mol

Moles of sugar = Mass of sugar / Molecular weight of sugar

Moles of sugar = 152.395 g / 110 g/mol

Moles of sugar = 1.385 mol

Mass of solvent (water) = Volume of solution - Mass of solute (sugar)

Mass of solvent (water) = 5.19 L - 0.146739 kg (since density of water is approximately 1 kg/L)

Now we can calculate the molality:

Molality = Moles of solute / Mass of solvent (in kg)

Molality = 1.385 mol / 5.043261 kg

Molality = 0.275 mol/kg

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Therefore, it takes 165.308 calories of heat to warm 14.9 g of brick from 21.4 °C to 47 °C.

The amount of heat needed to raise a substance's temperature by one degree Celsius in one gramme, also known as specific heat.

Using the following calculation, we can determine how much heat is needed to raise 14.9 g of brick from 21.4 to 47.4 degrees Celsius:

q = m * c * ΔT

where q is the required quantity of heat, m is the substance's mass, c is its specific heat, and T is the temperature change.

Brick has a specific heat of 0.20 cal/g.°C, so when the given values are substituted, we obtain:

q = 14.9 g * 0.20 cal/g.°C * (47.4°C - 21.4°C)

q = 14.9 g * 0.20 cal/g.°C * 26°C

q = 165.308 cal

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Therefore, it takes 165.308 calories of heat to warm 14.9 g of brick from 21.4 °C to 47 °C.

The amount of heat needed to raise a substance's temperature by one degree Celsius in one gramme, also known as specific heat.

Using the following calculation, we can determine how much heat is needed to raise 14.9 g of brick from 21.4 to 47.4 degrees Celsius:

q = m * c * ΔT

where q is the required quantity of heat, m is the substance's mass, c is its specific heat, and T is the temperature change.

Brick has a specific heat of 0.20 cal/g.°C, so when the given values are substituted, we obtain:

q = 14.9 g * 0.20 cal/g.°C * (47.4°C - 21.4°C)

q = 14.9 g * 0.20 cal/g.°C * 26°C

q = 165.308 cal

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