A student adds 7.00 g of dry ice (solid co2) to an empty balloon. what will be the volume of the balloon at stp after all the dry ice sublimes (converts to gaseous co2)

The mass of the silver sample is approximately 77.9 grams.

To solve this problem, we can utilize the equation for heat transfer:

q = m * c * ΔT

where q represents the heat transferred, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.

Initially, we calculate the heat transferred from the silver to the water:

q silver = m silver * c silver * ΔT silver

q water = m water * c water * ΔT water

For thermal equilibrium between the silver and water, we equate the two equations as they reach the same temperature:

q silver = q water

m silver * c silver * ΔT silver = m water * c water * ΔT water

Rearranging the equation allows us to solve for the mass of the silver:

m silver = (m water * c water * ΔT water) / (c silver * ΔT silver)

Substituting the given values:

m silver = (250g * 4.184 J/g°C * (23.35°C - 6.5°C)) / (0.235 J/g°C * (98.75°C - 23.35°C))

As a result:

m silver = 77.9 g

Thus, the mass of the silver sample is approximately 77.9 grams.

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The difference in the chemical potential for liquid and crystalline water at 270.15 K is -0.97 J/mol.


1. Convert given pressures to atm: initial partial pressure of water vapor (P1) = 489 Pa / 101325 Pa/atm = 0.00482 atm, and new partial pressure (P2) = 475 Pa / 101325 Pa/atm = 0.00469 atm.

2. Use the Clausius-Clapeyron equation: ln(P2/P1) = -(ΔH_sub/R)(1/T2 - 1/T1), where ΔH_sub is the enthalpy of sublimation, R is the gas constant, and T1 and T2 are the initial and final temperatures, both equal to 270.15 K.

3. Rearrange the equation to solve for ΔH_sub: ΔH_sub = R * (ln(P2/P1))/(1/T2 - 1/T1), and substitute the values: ΔH_sub = 8.314 J/mol K * (ln(0.00469/0.00482))/(0 - 0) = -0.97 J/mol.

4. The negative sign makes sense as the system moves to a new equilibrium with a lower chemical potential for crystalline water, indicating a more stable phase.

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When the balloon is submerged in water at a depth where the pressure is 4.7 atm and the temperature is 15 °C, its volume will be approximately 0.995 L.

From the ideal gas equation, we can use the combined gas law formula, which is:

(P1 × V1) / T1 = (P2 × V2) / T2

Here, P1 = 1.1 atm (initial pressure), V1 = 3.7 L (initial volume), T1 = 30 °C (initial temperature), P2 = 4.7 atm (final pressure), and T2 = 15 °C (final temperature). We need to find V2 (final volume).

First, convert the temperatures to Kelvin by adding 273.15:

T1 = 30 + 273.15 = 303.15 K

T2 = 15 + 273.15 = 288.15 K

Now, plug in the values into the combined gas law formula and solve for V2:

        (P1 × V1) / T1 = (P2 × V2) / T2

(1.1 × 3.7) / 303.15 = (4.7 × V2) / 288.15

    (4.07) / 303.15 = (4.7 × V2) / 288.15

Now, solve for V2:

V2 = (4.07 × 288.15) / (303.15 × 4.7)

V2 ≈ 0.995 L

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654 grams of Zn metal will completely react with 730 grams of HCl

The balanced chemical equation for this reaction is:
Zn + 2HCl → ZnCl2 + H2

From the equation, we can see that for every 1 mole of Zn, 2 moles of HCl are required for a complete reaction. This means the mole ratio of Zn to HCl is 1:2.

To determine the number of moles of HCl used, we need to convert the given mass of HCl to moles. The molar mass of HCl is 36.5 g/mol, so:

730 g HCl x (1 mol HCl/36.5 g HCl) = 20 moles HCl

Using the mole ratio from the balanced equation, we can determine the number of moles of Zn required:

20 moles HCl x (1 mol Zn/2 mol HCl) = 10 moles Zn

Finally, we can convert the number of moles of Zn to grams using its molar mass of 65.4 g/mol:

10 moles Zn x (65.4 g Zn/mol) = 654 grams of Zn

Therefore, 654 grams of Zn metal will completely react with 730 grams of HCl to produce ZnCl2 and H2.

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3.86 grams of chlorine would exert a pressure of 610 torr in a 3.26-liter container at standard temperature.

To calculate the number of grams of chlorine required to exert a pressure of 610 torr in a 3.26-liter container at standard temperature, we need to use the ideal gas law equation: PV = nRT.

Where,

P = pressure = 610 torr

V = volume = 3.26 L

n = number of moles

R = gas constant = 0.0821 Latm/(molK) (standard value)

T = temperature = 273 K (standard temperature)

n = PV ÷ RT

Substituting the given values, we get:

n = (610 torr × 3.26 L) ÷ (0.0821 Latm/(molK) × 273 K)

n = 0.109 mol

Now, to convert moles to grams, we need to use the molar mass of chlorine, which is 35.45 g/mol.

Thus, number of grams of chlorine required is:

0.109 mol × 35.45 g/mol = 3.86 g

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Approximately 108,066 J of heat is required to heat 352 g of water from 20.0°C to 93.7°C in an electric kettle.

To determine the quantity of heat required to heat 352 g of water from 20.0°C to 93.7°C, we need to use the specific heat capacity of water and the equation:

q = m × c × ΔT

ΔT = change in temperature (in °C)

First, we need to calculate the change in temperature:

ΔT = final temperature - initial temperature

ΔT = 93.7°C - 20.0°C

ΔT = 73.7°C

Substituting the given values into the equation, we get:

q = 352 g × 4.184 J/g·°C × 73.7°C

q = 108,066.496 J

q ≈ 108,066 J (rounded to three significant figures)

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There are 0.1474 moles of hydrogen atoms in 0.0737 mol of N2H4.

What is Mole?

In chemistry, a mole is a unit used to express the amount of a substance. One mole of a substance is defined as the amount of that substance that contains as many elementary entities (atoms, molecules, or other particles) as there are atoms in 12 grams of carbon-12.

To determine the mass of lead in PbCO3, we need to use the molar mass of PbCO3 and the stoichiometric relationship between Pb and PbCO3. The molar mass of PbCO3 is 267.21 g/mol, and the stoichiometric relationship between Pb and PbCO3 is 1:1.

Thus, the mass of Pb in 1.25x10^4 g of PbCO3 can be calculated as follows:

Mass of Pb = (1.25x10^4 g PbCO3) x (1 mol PbCO3/267.21 g PbCO3) x (1 mol Pb/1 mol PbCO3) x (207.2 g Pb/mol Pb)

= 1.02x10^4 g Pb

Therefore, 1.02x10^4 g of Pb is contained in 1.25x10^4 g of PbCO3.

The formula for N2H4 indicates that there are two hydrogen atoms for every molecule of N2H4. Therefore, we can calculate the number of moles of hydrogen atoms in 0.0737 mol of N2H4 as follows:

Number of moles of H atoms = (0.0737 mol N2H4) x (2 mol H atoms/1 mol N2H4)

= 0.1474 mol H

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The question does not provide a specific nuclear chemical equation to work with, so it is difficult to provide a direct answer. However, I can provide some general information about nuclear chemical equations.

Nuclear chemical equations are used to represent nuclear reactions. These reactions involve changes in the nucleus of an atom, typically involving the addition or removal of protons and/or neutrons. Unlike chemical reactions, which involve the sharing or transfer of electrons, nuclear reactions involve changes in the core of the atom.

A typical nuclear chemical equation includes a reactant on the left side of the equation and a product on the right side. The reactant and product are both represented by chemical symbols, such as H for hydrogen or O for oxygen. The number of protons and neutrons in the reactant and product may differ, indicating a change in the nucleus.

In some cases, the nuclear chemical equation may be missing a symbol. This could indicate that the product is unknown or has not been determined. It is also possible that the missing symbol represents a hypothetical or theoretical product, rather than an actual substance.

In summary, nuclear chemical equations are used to represent nuclear reactions, which involve changes in the nucleus of an atom. The equations include reactants and products represented by chemical symbols, and may occasionally include missing symbols indicating an unknown or theoretical product.

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The structure of product is shown.

When pentanedioic (glutaric) anhydride reacts with ammonia at high temperature, it undergoes an amide formation reaction to produce a compound with the molecular formula C₅H₇NO₂. The amide formation reaction involves the nucleophilic attack of the ammonia molecule on one of the carbonyl carbon atoms of the anhydride, leading to the formation of an intermediate product called an amide.

This amide then undergoes further reactions to form the final product with the given molecular formula. The presence of both carboxylic acid and amide functional groups in the molecule indicates that it contains both the original anhydride and the product of its reaction with ammonia.

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The balanced chemical equation for the reaction of nitrogen and oxygen to produce nitrogen dioxide is:

2NO + O2 → 2NO2

According to the equation, 1 mole of nitrogen reacts with 0.5 moles of oxygen to produce 1 mole of nitrogen dioxide.

To determine the volume of nitrogen required to react with 33.6 L of oxygen, we need to convert the volume of oxygen to moles, and then use the mole ratio to find the moles of nitrogen required, and finally convert to volume of nitrogen.

Using the ideal gas law, we can convert the given volume of oxygen to moles:

n(O2) = PV/RT

where P is the pressure, V is the volume, R is the gas constant, and T is the temperature in Kelvin.

Assuming standard temperature and pressure (STP) conditions of 1 atm and 273 K, we get:

n(O2) = (1 atm) × (33.6 L) / [(0.0821 L·atm/mol·K) × (273 K)] = 1.37 moles of O2

Using the mole ratio from the balanced chemical equation, we know that 2 moles of NO react with 1 mole of O2. So the number of moles of NO required to react with 1.37 moles of O2 is:

n(NO) = 2 × (1.37 moles of O2) = 2.74 moles of NO

Finally, we can convert the moles of NO to volume using the ideal gas law:

V(NO) = n(NO)RT/P

Assuming STP conditions again, we get:

V(NO) = (2.74 mol) × (0.0821 L·atm/mol·K) × (273 K) / (1 atm) ≈ 60.4 L

Therefore, approximately 60.4 L of nitrogen would be required to react with 33.6 L of oxygen to produce nitrogen dioxide, under the given conditions.

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One potential difference between ice that Dr. Stewart is climbing and "normal" water ice could be the location or conditions in which it formed.

For example, glacier ice, which forms over many years from compacted snow, can have different properties than the ice that forms on a frozen lake or river. Similarly, ice formed in a cold laboratory setting might have different properties than ice formed under natural conditions.

Other factors that could impact the characteristics of ice include the presence of air bubbles, cracks or fissures, and the size and shape of ice crystals. Ice that has been subjected to pressure or other stresses can also exhibit unique features such as layers or bands.

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The equation q = mHΔv is used to calculate the amount of heat required to vaporize a certain amount of substance. In this case, the substance is water and the latent heat of vaporization is 2260 kJ/kg.

The variable q represents the amount of heat required to vaporize the substance, which is measured in joules (J) or kilojoules (kJ). The variable m represents the mass of the substance being vaporized, which is measured in kilograms (kg). Finally, the variable HΔv represents the latent heat of vaporization, which is a property of the substance and is measured in joules per kilogram (J/kg).

When water is heated, it will begin to evaporate, or turn into a gas. This process requires energy in the form of heat. The amount of heat required to vaporize a certain amount of water can be calculated using the equation q = mHΔv. For example, if we want to vaporize 1 kg of water, we can calculate the amount of heat required by multiplying the mass by the latent heat of vaporization:

q = 1 kg x 2260 kJ/kg
q = 2260 kJ

Therefore, it would require 2260 kJ of heat to vaporize 1 kg of water.

In summary, the equation q = mHΔv is a useful tool for calculating the amount of heat required to vaporize a substance, such as water. The latent heat of vaporization is a property of the substance and is required in order to make these calculations.

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The mass of KI needed to prepare 500 mL of a 0. 750 M solution is 62.25 grams

To compute the mass of KI needed to prepare 500 mL of a 0.750 M solution, use the formula:

Molarity (M) = moles of solute / volume of solution in liters

First, convert the volume to liters: 500 mL = 0.5 L

Next, rearrange the formula to find the moles of solute:

moles of solute = Molarity × volume of solution in liters
moles of KI = 0.750 M × 0.5 L
moles of KI = 0.375 moles

Now, find the molar mass of KI (Potassium Iodide):
K (Potassium) = 39.10 g/mol
I (Iodine) = 126.90 g/mol
Molar mass of KI = 39.10 g/mol + 126.90 g/mol = 166.00 g/mol

Finally, calculate the mass of KI needed:

mass of KI = moles of KI × molar mass of KI
mass of KI = 0.375 moles × 166.00 g/mol
mass of KI = 62.25 g

Therefore, you will need 62.25 grams of KI to prepare 500 mL of a 0.750 M solution.

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An advantageous trait describes the brown scales in fish living in a muddy lake environment, providing them with a better chance of survival and reproductive success by blending in with their surroundings and making it harder for predators to see them.

The term that best describes the brown scales in this scenario is advantageous trait. An advantageous trait is a characteristic that provides an organism with a greater chance of survival and reproductive success in a specific environment. In this case, the brown scales provide an advantage to the fish living in the muddy lake environment as they blend in better with their surroundings, making it harder for predators to see them. As a result, fish with brown scales are more likely to survive and reproduce, passing on this trait to their offspring. The silver scales are the predominant phenotype, meaning they are the most common physical expression of the fish's genotype. The brown scales may have arisen through a new mutation, but their persistence in the population suggests they have become a part of the fish's genetic makeup. There is no indication that an inactivated gene is responsible for the brown scales.

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The Haber process involves the following steps:

Preparation of reactants; Compression of gases; Mixing of gases; Reaction; Separation of ammonia; Separation of ammonia

The Haber process is a method used to manufacture ammonia (NH3) from nitrogen gas (N2) and hydrogen gas (H2). The process is named after its inventor, German chemist Fritz Haber, who developed the process in the early 20th century.

The Haber process involves the following steps

The Haber process is an important industrial process for the production of ammonia, which is a vital ingredient in the production of fertilizers and many other chemical compounds.

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In this sample there are 1.51 x 10^24 molecules of sucrose present in it.

To determine the number of molecules of sucrose present in the sample, we need to first calculate the number of moles of carbon present in the sample.

The molecular formula of sucrose (C12H22O11) contains 12 carbon atoms.

So, 3.6 x 10^24 atoms of carbon is equal to 3.6 x 1024/12 = 3 x 1023 moles of carbon.

Now, we can use the Avogadro's number (6.022 x 10^23 molecules per mole) to convert the number of moles of carbon to the number of molecules of sucrose:

Number of molecules of sucrose = 3 x 10^23 x (1 molecule of sucrose / 12 molecules of carbon) x (6.022 x 10^23 molecules per mole)

Number of molecules of sucrose = 1.51 x 10^24 molecules

Therefore, there are 1.51 x 10^24 molecules of sucrose present in the sample.

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16.128 grams of hydrogen gas would need to react in order to produce 972 kJ of heat energy.

So, first, we can calculate the amount of heat energy released per mole of [tex]H_2[/tex] reacted:

243 kJ of heat / 2 moles of [tex]H_2[/tex] = 121.5 kJ/mol of [tex]H_2[/tex]

We can use the following equation to calculate the amount of hydrogen gas required:

Amount of [tex]H_2[/tex]  = Energy released / Heat of reaction per mole of [tex]H_2[/tex]

Amount of [tex]H_2[/tex] = 972 kJ / 121.5 kJ/mol = 8 moles of [tex]H_2[/tex]

Finally, we can calculate the mass of [tex]H_2[/tex] required using its molar mass:

Mass of [tex]H_2[/tex] = Number of moles of[tex]H_2[/tex]x Molar mass of [tex]H_2[/tex]

Mass of [tex]H_2[/tex] = 8 moles x 2.016 g/mol = 16.128 g of [tex]H_2[/tex]

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The amount of heat required to convert 46.0 g of ethanol at 25° C to vapor phase is ≅ 44.2 KJ total heat .

Using the mass , evaluating the moles of ethanol :

                              46.0 g × [tex]\frac{1 Mol}{46.07 g}[/tex] = 0.998 mol

                                        ≅ 1.0 mol

The heat required to convert 46.0 g ethanol from 25° C at 78° C is evaluated :

                                     q₁ = m[tex]C_{liquid }[/tex]ΔT

                                   = 46.0 g × [tex]\frac{2.3 J}{g. K}[/tex] × 78° C - 25°C

                                 =     5607.47J × 1 KJ /1000 J

                                           = 5.607 KJ

So, the heat required in conversion of 1.0 mol of ethanol at 78 ° C  to 1.0 mol ethanol vapour is expressed as :

                           q₂ = moles × Δ[tex]H_{vap}[/tex]

                            = 1.0 mol × 38.56 KJ /mol

                                = 38.56 kJ/ mol

The total heat requirement conversion of 46 .0 g of ethanol at 25° C to the vapour state at 78° C :

                           Total heat = q₁ + q₂

                                         = 5.607 KJ + 38.56 KJ

                                            = 44.167 KJ

                                        ≅ 44.2 KJ

Fume alludes to a gas stage at a temperature where a similar substance can likewise exist in the fluid or strong state, beneath the basic temperature of the substance. As a result of their tendency to be volatile, liquids will enter the vapor phase when the temperature is raised sufficiently. At the specified temperature, a liquid is considered to be volatile if it exhibits a significant vapor pressure.

Transferring a substance from a vapor to a solid by desorbing it using a desorbent or carrier gas and passing the vapor sample through a stationary phase (such as silica particles).

Incomplete question :

Determine the amount of heat required to convert 46. 0 g of ethanol at 25°c to the vapor phase at 78°c. Based on the melting and boiling points, ethanol is a liquid at 25°c. Consider the heating curve when organizing your thoughts and answering the question. Use the information about ethanol CH₃CH₂OH given in the table below.

Use the following information about ethanol CH₃CH₂OH.

Tmelt = –114°C

Tboil = 78°C

∆Hfus = 5.02 kJ/mol

∆Hvap = 38.56 kJ/mol

C solid = 0.97 J/g-K

C liquid = 2.3 J/g-K

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Answer: Friction causes kinetic energy (rubbing your hands together) to convert to heat energy.

Explanation:

The freezing point of the lithium bromide solution is approximately -1.06°C.

To determine the freezing point of the solution, we need to use the freezing point depression formula:

ΔTf = Kf * molality

where ΔTf is the freezing point depression, Kf is the freezing point depression constant (which depends on the solvent), and molality is the concentration of the solution in mol/kg.

First, we need to calculate the molality of the solution:

molality = moles of solute / mass of solvent (in kg)

The mass of 525 mL of water is:

mass = volume * density = 525 mL * 1 g/mL = 525 g

The number of moles of lithium bromide is:

moles of LiBr = 0.300 mol

Therefore, the molality of the solution is:

molality = 0.300 mol / 0.525 kg = 0.571 mol/kg

The freezing point depression constant for water is 1.86 °C/m. Therefore, the freezing point depression is:

ΔTf = 1.86 °C/m * 0.571 mol/kg = 1.06306 °C

Finally, to find the freezing point of the solution, we need to subtract the freezing point depression from the freezing point of pure water (0°C):

Freezing point = 0°C - 1.06306°C = -1.06306°C

Therefore, the freezing point of the lithium bromide solution is approximately -1.06°C.

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B Answer:

Explanation:

Higher, 1020 mb +, rising pressure and temp are associated with clear skies and low precipitation

The net ionic equation for the equilibrium that is established when sodium cyanide (NaCN) is dissolved in water is:

NaCN + H2O ⇌ CN- + Na+ + H2O

In this equation, the cyanide ion (CN-) is produced by the dissociation of NaCN in water. The sodium ion (Na+) and water (H2O) are spectator ions and do not participate in the reaction. Therefore, they are not included in the net ionic equation.

This solution is basic because the cyanide ion is a weak base and can hydrolyze water to produce hydroxide ions (OH-) according to the following reaction:

CN- + H2O ⇌ HCN + OH-

The equilibrium constant for this reaction is relatively small, but it is enough to make the solution basic.

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3MnO₂ + 4Al → 2Al₂O₃ + 3Mn

A chemical equation is said to be balanced when the number of atoms of each element on both sides of the equation are the same.

According to this question, manganese oxide reacts with aluminum to produce aluminum oxide and manganese. The balanced equation is given above.

49.7 grams of MnO₂ is equivalent to 0.57 moles

If 3 moles of MnO₂ reacts with 4moles of Al, then 0.57 moles of MnO₂ will react with 0.76 moles of Al.

0.76 moles of Al is equivalent to 20.52 grams of Al.

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A solution of potassium hydroxide reacts completely with a solution of nitric acid. Potassium nitrate will remain after the water dissolves in solid mixture.

What is a solid mixture?

This kind of mixture consists of two or more solids. Alloys are what are used when the solids are made of metals. Sand and sugar, stainless steel, etc. are a few examples of solid-solid combinations.

2KOH(aq) + HNO₃(aq) → KNO₃(aq) + 2H₂O(l)

When a solution of potassium hydroxide (KOH) reacts completely with a solution of nitric acid (HNO₃), potassium nitrate (KNO₃) is formed in aqueous form, along with water (H₂O). The solid mixture that will remain after the water evaporates is potassium nitrate (KNO₃).

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The final pressure of the gas sample is 1.09 atm when heated to 50ºC.

The final pressure of a gas sample initially at 1.00 atm and 25ºC when heated to 50ºC can be calculated using the ideal gas law:

P₁ × V₁ ÷ T₁ = P₂ × V₂ ÷ T₂

where P₁, V₁, and T₁ are the initial pressure, volume, and temperature of the gas, respectively, and P₂, V₂, and T₂ are the final pressure, volume, and temperature of the gas, respectively.

Assuming that the volume of the gas remains constant, V₁ = V₂, and rearranging the ideal gas law, we get:

P₂ = P₁ (T₂ ÷ T₁)

Substituting the values, we get:

P₂ = (1.00 atm) × (323 K) ÷ (298 K) = 1.09 atm

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The formulae of the hydroxides are: X(OH), Y(OH)₂, and Z(OH)₃.

The formulae of the sulphates are: XSO₄, YSO₄, and Z(SO₄)₂.

The formulae of the carbonates are: XCO₃, YCO₃, and Z(CO₃)₂.

The formulae of the hydrogen carbonates are: X(HCO₃), Y(HCO₃)₂, and Z(HCO₃)₃.

The formulae of the nitrates are: X(NO₃), Y(NO₃)₂, and Z(NO₃)₃.

The formulae of the phosphates are: X(PO₄), Y(PO₄)₂, and Z(PO₄)₃.

The valency of a metal tells us how many electrons it can lose or gain in order to form an ion. Using the valencies of metals X, Y, and Z, we can determine the formulae of their compounds with different anions. In each case, we use the appropriate valency of the metal and the valency of the anion to balance the charges of the compound.

For example, in the case of hydroxides, the valency of metal X is 1, which means it can combine with one hydroxide ion (OH⁻) to form a neutral compound, X(OH). Similarly, for metal Y with valency 2, it requires two hydroxide ions to form a neutral compound, Y(OH)₂.

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The concentration of the Ba(OH)₂ solution is 0.1 M.

To find the concentration of the Ba(OH)₂ solution, we can use the balanced equation for the neutralization reaction between Ba(OH)₂ and HNO₃:

Ba(OH)₂ + 2HNO₃ → Ba(NO₃)₂ + 2H₂O

From the equation, we can see that one mole of Ba(OH)₂ reacts with two moles of HNO₃. Therefore, the moles of HNO₃ used in the neutralization reaction can be calculated as follows:

moles of HNO₃ = 1.52 M × 0.0234 L = 0.035568 mol

Since the moles of HNO₃ is equal to the moles of Ba(OH)₂ in the reaction, we can calculate the concentration of the Ba(OH)₂ solution as follows:

concentration of Ba(OH)₂ = moles of Ba(OH)₂ / volume of Ba(OH)₂ solution

moles of Ba(OH)₂ = moles of HNO₃ / 2 = 0.035568 mol / 2 = 0.017784 mol

volume of Ba(OH)₂ solution = 0.063 L

concentration of Ba(OH)₂ = 0.017784 mol / 0.063 L ≈ 0.1 M

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The quantum efficiency (QE) of the radiation of 2530 amstrong incidents is approximately 3.47 x [tex]10^8[/tex].

We have,

Quantum efficiency (QE) is a measure of the number of molecules undergoing a specified reaction per photon absorbed.

In this case, you want to calculate the quantum efficiency based on the given data.

Quantum Efficiency (QE) is given by the formula:

QE = (Number of molecules decomposed) / (Number of photons absorbed)

Given:

Number of molecules decomposed = 1.85 × 10^-2 moles

Number of photons absorbed = Energy absorbed / Energy per photon

The energy of a photon (E) is given by Planck's equation:

E = hc / λ

Where:

h = Planck's constant = 6.626 × 10^-34 J·s

c = Speed of light = 3 × 10^8 m/s

λ = Wavelength of radiation = 2530 Å = 2530 × 10^-10 m

Calculate the energy per photon using the wavelength:

E = (6.626 × [tex]10^{-34}[/tex] J·s * 3 × [tex]10^8[/tex] m/s) / (2530 × [tex]10^{-10}[/tex] m)

= 0.007856 x [tex]10^{-34 + 8 + 10[/tex]

= 0.007856 x [tex]10^{-16}[/tex] J

Now, calculate the energy absorbed:

Energy absorbed = 1000 cal = 1000 * 4.184 J (since 1 cal = 4.184 J)

Number of photons absorbed = Energy absorbed / Energy per photon

Calculate the quantum efficiency using the given formula:

QE = (Number of molecules decomposed) / (Number of photons absorbed)

QE = (1.85 × [tex]10^{-2}[/tex] moles) / (Number of photons absorbed)

Substitute the value of the Number of photons absorbed:

QE = (1.85 × [tex]10^{-2}[/tex] moles) / [(1000 * 4.184 J) / (0.007856 x [tex]10^{-16}[/tex] J)]

QE = (1.85 × [tex]10^{-2}[/tex] moles) / (532586.56 x [tex]10^{16}[/tex] J)

QE = 0.000003474 x [tex]10^{14}[/tex]

QE ≈ 3474 × [tex]10^5[/tex]

QE = 3.47 x [tex]10^8[/tex]

Therefore,

The quantum efficiency (QE) is approximately 3.47 x [tex]10^8[/tex].

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