the cis ketone a is isomerized to the trans ketone b with aqueous naoh. a similar isomerization reaction does not occur with the cis ketone c. explain this difference in reactivity. be sure to answer all parts.

Theo watches the Moon every night for four weeks, he notices that how the Moon's position in the sky changes over time.

Here are some things that Theo might observe or learn about the Moon:

The Moon's phases: By watching the Moon every night for four weeks, Theo would likely observe the changing phases of the Moon as it orbits the Earth. The Moon goes through a complete cycle of phases roughly once a month, which includes the new moon, waxing crescent, first quarter, waxing gibbous, full moon, waning gibbous, third quarter, and waning crescent.

The Moon's position in the sky: Theo might also notice how the Moon's position in the sky changes over time. The Moon rises and sets at different times each night, and its position in the sky also changes depending on its phase and location relative to the horizon.

The Moon's motion: By observing the Moon's position in the sky each night, Theo might notice that the Moon appears to move relative to the stars.

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it would take 3.16 litres of water to make a 0.19 M solution of NaI from 0.60 moles of NaI.

To calculate the volume of water needed to make a 0.19 M solution of NaI, we need to use the formula:

Moles of solute = Molarity x Volume (in liters)

We can rearrange this formula to solve for the volume of water:

Volume (in liters) = Moles of solute / Molarity

First, let's calculate the number of moles of NaI in 0.60 moles:

Moles of NaI = 0.60 moles

Now, we can use the formula above to calculate the volume of water needed:

Volume (in litres) = Moles of NaI / Molarity

Volume (in litres) = 0.60 moles / 0.19 M

Volume (in litres) = 3.16 litres

Therefore, it would take 3.16 litres of water to make a 0.19 M solution of NaI from 0.60 moles of NaI.
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[tex] \:\:\:\:\:\:\star [/tex]For the general solubility equilibrium [tex]\sf \underline{AB \longrightarrow A^+ + B^-} [/tex]the solubility product has the following expression-

[tex] \:\:\:\:\:\:\star\longrightarrow \sf\underline{K_{(sp)} = [A^+] \times [B^-]}\\[/tex]

As per question, we are given that-

[tex] \:\:\:\:\:\:\star [/tex] Now that we have all the required values, so we can substitute these values into the Ksp expression and solve for Ksp-

[tex] \:\:\:\:\:\:\star\longrightarrow \sf\underline{K_{(sp)} = [A^+] \times [B^-]}\\[/tex]

[tex] \:\:\:\:\:\:\longrightarrow \sf K_{(sp)} = 0.00343 \:M\times 0.00343\:M\\[/tex]

[tex] \:\:\:\:\:\:\longrightarrow \sf K_{(sp)} = 0.00343 \:molL^{-1}\times 0.00343\:molL^{-1}\\[/tex]

[tex] \:\:\:\:\:\:\longrightarrow \sf \underline{K_{(sp)} = 1.17649\times 10^{-5} \: mol^2L^{-2}}\\[/tex]

If Abby doubles the initial monomer concentration and quadruples the initiator concentration from the original settings, the outcome of the new polymer will likely have a higher number average molecular weight.

Abby's outcome of the new polymer will likely have a higher number average molecular weight because increasing the monomer concentration will lead to more monomer units being available for polymerization, while increasing the initiator concentration will lead to more initiation events, resulting in a higher degree of polymerization.

However, the exact molecular weight of the new polymer will depend on the efficiency of the polymerization reaction and any potential side reactions or termination events that may occur. It is possible that increasing the initiator concentration could also lead to more side reactions, such as chain transfer or termination, which could affect the final molecular weight distribution.

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The balanced chemical equation for the reaction between hydrochloric acid (HCl) and calcium hydroxide (Ca(OH)2) is:

2HCl + Ca(OH)2 → CaCl2 + 2H2O

First, we need to calculate the moles of calcium hydroxide (Ca(OH)2) present in 5.00 grams:

molar mass of Ca(OH)2 = 40.08 + 2(15.99) + 2(1.01) = 74.10 g/mol

moles of Ca(OH)2 = mass / molar mass = 5.00 g / 74.10 g/mol = 0.0674 mol

According to the balanced chemical equation, 2 moles of HCl react with 1 mole of Ca(OH)2. Therefore, the number of moles of HCl required to react completely with 0.0674 mol of Ca(OH)2 is:

moles of HCl = 2 x moles of Ca(OH)2 = 2 x 0.0674 mol = 0.1348 mol

Finally, we can use the molarity (0.100 M) and the number of moles of HCl to calculate the volume of the HCl solution required:

moles = molarity x volume (in liters)

volume (in liters) = moles / molarity = 0.1348 mol / 0.100 mol/L = 1.35 L

Therefore, 1.35 liters of 0.100 M HCl are required to react completely with 5.00 grams of calcium hydroxide.

1.35 liters of 0.100 M [tex]HCl[/tex] would be required to react completely with 5.00 grams of calcium hydroxide.

To determine how many liters of 0.100 M [tex]HCl[/tex]would be required to react completely with 5.00 grams of calcium hydroxide, follow these steps:

1. Write the balanced chemical equation for the reaction:
[tex]2 HCl(aq) + Ca(OH)₂(s) → CaCl₂(aq) + 2 H₂O(l)[/tex]
2. Calculate the moles of calcium hydroxide (Ca(OH)₂):
Molar mass of [tex]Ca(OH)₂ = 40.08 (Ca) + 2 * (16.00 + 1.01) (2 * OH) = 74.10 g/mol[/tex]
Moles of[tex]Ca(OH)₂[/tex] = mass / molar mass =[tex]5.00 g / 74.10 g/mol ≈ 0.0675 mol[/tex]

3. Determine the stoichiometry between[tex]HCl[/tex] and[tex]Ca(OH)₂[/tex] from the balanced equation:
2 moles of [tex]HCl[/tex] react with 1 mole of [tex]Ca(OH)₂[/tex].

4. Calculate the moles of[tex]HCl[/tex] required to react completely with[tex]Ca(OH)₂[/tex]:
Moles of [tex]HCl = 0.0675 mol Ca(OH)₂ * (2 mol HCl / 1 mol Ca(OH)₂) = 0.135 mol HCl[/tex]

5. Determine the volume of 0.100 M[tex]HCl[/tex]needed to provide the required moles of[tex]HCl[/tex]:
Volume = moles of[tex]HCl[/tex] / molarity = 0.135 mol / 0.100 M = 1.35 L

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To fix the issue, the student should carefully reapply the sample in a smaller amount, allow it to dry completely, and adjust the solvent system if necessary to achieve proper separation of the components on the TLC plate.

The student might have made the following technical mistake while running the TLC plate:

1. Overloading the sample: When spotting the TLC plate, the student may have applied too much sample, causing the components to streak rather than separate into individual spots. To resolve this, the student should apply a smaller amount of sample and ensure that it is evenly distributed.

2. Insufficient drying: If the student did not allow the spotted sample to dry properly before placing it in the solvent, it can cause the components to streak. To prevent this, the student should ensure the sample is completely dry before running the TLC plate.

3. Inappropriate solvent system: Although the student used a 10% ethyl acetate/hexane mixture, it is possible that this solvent system was not suitable for the specific sample. Adjusting the solvent ratio or trying different solvent systems could help achieve better separation.

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Performing a reaction in a vacuum chamber to control the experiment is a valid approach to prevent external variables from impacting the reaction.

However, it may not be sufficient to determine if the reaction is endothermic or exothermic and measure the amount of energy absorbed or given off. This is because the vacuum chamber only isolates the reaction from the environment, but it does not provide a way to measure the energy changes that occur during the reaction. To measure the energy changes, the scientist should use techniques such as calorimetry, which directly measures the heat absorbed or released by the reaction.

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While considering a good solvent alternative for diethyl ether, the best one will be ethyl acetate. It can be used for extraction due to its polarity and less toxicity.

Diethyl ether is one of the commonly used solvent in extraction process of non-polar or slightly polar organic compounds. This is because it does not have hydrogen bonding. So here methanol cannot be used as it has extensive hydrogen bonding and non-polar compounds might not dissolve.

Water also cannot be used because of its polar nature. So organic compounds does not dissolve. Tetrahydrofuran can be used as a solvent, but toxicity levels are higher compared to diethyl ether.

So the alternative that can be used is ethyl acetate, which is also widely used solvent in extraction of non-polar compounds. Also it has less toxicity compared to THF.

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1. The mass (in grams) of FeBr₃ produced from 65 g of Br₂ is 80.13 g

2. The mole of CO₂ formed from 10 moles of C₅H₁₂ is 50 moles

3. The moles of MnCl₂ prepared from 52.1 grams of MnO₂ is 0.6 mole

The mass of FeBr₃ produced can be obtained as illustrated below:

2Fe + 3Br₂ -> 2FeBr₃

From the balanced equation above,

480 g of Br₂ reacted to produce 591.7 g of FeBr₃

Therefore,

65 g of Br₂ will react to produce = (65 × 591.7) / 480 = 80.13 g of FeBr₃

Thus, the mass of FeBr₃ produced is 80.13 g

The mole of CO₂ formed can be obtained as follow:

C₅H₁₂ + 8O₂ -> 5CO₂ + 6H₂O

From the balanced equation above,

1 mole of C₅H₁₂ reacted to produce 5 moles of CO₂

Therefore,

10 moles of C₅H₁₂ will react to produce = 10 × 5 = 50 moles of CO₂

Thus, the mole of CO₂ formed is 50 moles

First, we shall obtain the mole of 52.1 g of MnO₂, Details below:

Mole = mass / molar mass

Mole of MnO₂ = 52.1 / 86.94

Mole of MnO₂ = 0.6 mole

Finally, we shall determine the mole of MnCl₂ prepared can be obtained as follow:

MnO₂ + 4HCl -> MnCl₂ + Cl₂ + 2H₂O

From the balanced equation above,

1 mole of MnO₂ reacted to produce 1 mole of MnCl₂

Therefore,

0.6 mole of MnO₂ will also react to produce 0.6 mole of MnCl₂

Thus, the mole of MnCl₂ prepared is 0.6 mole

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The ionic equations are as follows:
[tex]H^{+} (aq) + CN^{-} (aq) < -- > HCN(aq)[/tex]
[tex]CN^{-} (aq) + H2O (l) < = > HCN (aq) + OH^{-} (aq)[/tex]

The buffer solution containing a mixture of aqueous HCN and KCN can be represented as:

[tex]HCN(aq) + CN^{-} (aq) + K^{+} (aq) < --- > HCN(aq) + KCN(aq)[/tex]

a. When a few drops of HCl are added to the buffer solution, the H+ ions from the HCl react with the CN- ions in the buffer solution to form HCN. The net ionic equation for the reaction is:

[tex]H^{+} (aq) + CN^{-} (aq) < -- > HCN(aq)[/tex]

b. When a few drops of NaOH are added to the buffer solution, the OH- ions from the NaOH react with the HCN molecules in the buffer solution to form CN- ions. The net ionic equation for the reaction is:

[tex]CN^{-} (aq) + H2O (l) < = > HCN (aq) + OH^{-} (aq)[/tex]

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When a strong acid and a strong base are mixed in equal amounts, they undergo a neutralization reaction, resulting in the formation of water and a salt.

Therefore, the mixture of 1 M NaOH and 1 M HCl will not result in a neutral solution but instead will form sodium chloride and water. On the other hand, the mixture of 1 M NH3 and 1 M HCl, and the mixture of 1 M KOH and 1 M HBr, will also undergo neutralization reactions but will result in the formation of ammonium chloride and potassium bromide, respectively. The mixture of 1 M NaOH and 1 M HI will also not result in a neutral solution but will form sodium iodide and water due to the reaction between the strong base NaOH and the weak acid HI.

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To calculate the molar mass of the unknown substance, we need to use the formula:

Molar mass = (mass of solute) / (number of moles of solute)

First, let's calculate the number of moles of solute in the solution:

Number of moles = (concentration) x (volume in liters)

We know that the concentration of the solution is 0.45 M, and the volume of the solution is 425 mL, which is equivalent to 0.425 L. Substituting these values into the formula, we get:

Number of moles = 0.45 M x 0.425 L

Number of moles = 0.19125 moles

Next, we can calculate the mass of the solute (the unknown substance) by using the formula:

mass = number of moles x molar mass

Rearranging the formula, we get:

molar mass = mass / number of moles

We know that the mass of the solute is 12 grams, and we have already calculated the number of moles as 0.19125 moles. Substituting these values into the formula, we get:

molar mass = 12 g / 0.19125 moles

molar mass = 62.8 g/mol

Therefore, the molar mass of the unknown substance is 62.8 g/mol.

The new temperature of the neon gas is 151.45°C when the pressure changes to 145 kPa and the volume remains constant.

Assuming that the amount of neon gas remains constant, we can use the combined gas law to find the new temperature. The combined gas law states that:

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

where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature, respectively. We are given P1 = 123 kPa, T1 = 89°C = 362 K, V1 = V2 (since the volume remains constant), and P2 = 145 kPa. Substituting these values into the combined gas law equation gives:

(123 kPa x V) / 362 K = (145 kPa x V) / T2

Simplifying this equation by cross-multiplying and rearranging gives:

T2 = (145 kPa x 362 K) / 123 kPa

T2 = 424.6 K

Finally, we can convert the temperature from Kelvin to Celsius by subtracting 273.15:

T2 = 424.6 K - 273.15

T2 = 151.45°C

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The net ionic equation for the acid-base hydrolysis equilibrium that is established when ammonium nitrate is dissolved in water is given below:Answer: NH4+(aq) + H2O(l) ⇌ H3O+(aq) + NH3(aq) + NO3-(aq).

The ionic equation is a chemical equation in which the electrolytes in aqueous solution are represented by their actual ions rather than their complete formulas. It indicates that ions undergo a chemical reaction to produce a new compound.

The net ionic equation displays the actual chemical reaction taking place in an aqueous solution. It is derived by eliminating spectator ions, which do not play any active role in the chemical reaction.The acid-base hydrolysis equilibrium is as follows:NH4+(aq) + H2O(l) ⇌ NH3(aq) + H3O+(aq).

The ammonium ion hydrolyzes to form ammonium ion and hydronium ions. The nitrate ion is a spectator ion that does not participate in the reaction. Therefore, the net ionic equation is given by:NH4+(aq) + H2O(l) ⇌ H3O+(aq) + NH3(aq).

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Ion-dipole attraction is the electrostatic attraction between an ion and a polar molecule. The correct answer is d.

Ion-dipole attraction is an intermolecular force that arises from the electrostatic attraction between an ion and a polar molecule. The ion is attracted to the partial charges on the polar molecule due to the separation of positive and negative charges within the molecule. This attraction is important in a variety of chemical processes, including dissolution of ionic compounds in solvents, such as water, where the solvent molecules surround and solvate the ions.

Ion-dipole interactions also play a significant role in many biological processes, such as protein folding and enzyme catalysis, as well as in industrial processes, such as separating ions in solution through methods like ion-exchange chromatography. Hence, the correct answer is d.

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565 mL of this solution must be diluted with water in order to make 1.000 L of 0.100 M [tex](Ba(OH) _{2} )[/tex].

Mass of [tex](Ba(OH) _{2} )[/tex] = 72.28 g

Volume of solution = 2.450 L

Molarity of water = 0.1 mole/L

Volume of water = 1000 L

To begin with, we must count the moles of Ba (OH)2 in the original solution:

[tex]n(Ba(OH) _{2} )[/tex] = 171.34g/mol/74.28g

​ =0.4335mol

0.100 moles of [tex](Ba(OH) _{2} )[/tex] are needed to make 1.000 L of a 0.100M [tex](Ba(OH) _{2} )[/tex] solution.

As a result, the starting solution's volume that has to be diluted is equal to:

V=2.450L× 0.4335mol/0.100mol

​=0.565L

0.565*1000ml

=565mL

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Complete question:

A 74.28-g sample of Ba (OH)2 is dissolved in enough water to make 2.450 liters of solution. How many mL of this solution must be diluted with water in order to make 1.000 L of 0.100 M Ba(OH)2?

The statement that does not describe radon-222 is  It binds with hemoglobin in the blood and can lead to death.

Radon-222 is a radioactive gas that occurs from the natural decay of uranium. It exists in igneous rock granite all around the world and can seep into homes through cracks in the foundation or soil. Its effects can be reduced by increasing ventilation in the affected areas.

This statement is inaccurate because radon does not bind with hemoglobin in the blood. Instead, radon gas decays into radioactive particles that can be inhaled and damage lung tissue, increasing the risk of lung cancer.

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Answer: 1.57g and 70.5%

Explanation:

Theoretical Yield

The theoretical yield of a reaction is the absolute maximum amount of product that could be created with the amounts of reactants.

This problem gives us the amount of hydrochloric acid, which is 6.37 grams. The molar mass of HCl is the molar mass of hydrogen plus the molar mass of chlorine, which is 36.46 g/mol.

To find the moles of HCl, we just divide the mass by the molar mass.

6.37/36.46 = 0.175 moles HCl

Since oxygen is in excess, the amount used in the reaction will be dictated by the amount of HCl used in the reaction. It does not need to be taken into consideration when determining the amount of reactant since it is in excess.

To find the theoretical yield of water, we will do stoichiometry.

Balancing the equation

Written out with the chemical symbols, this equation is

HCl + O2 ⇒H2O + Cl

This is not balanced, since there is 1 hydrogen on the left side and 2 on the right, and 2 oxygens on the left and 1 on the right.

To balance this, we can put coefficients in front of some reactants and products to make sure there are equal amounts of everything on each side.

The balanced equation will be 4HCl + O2 ⇒ 2H2O + Cl

Now, there are 4 hydrogens on the left and 4 on the right, as well as 2 oxygens on the left and 2 on the right. It is balanced.

We can see by looking at the coefficients of the balanced equation that every 4 moles of HCl consumed will produce 2 mole of H2O, so the ratio is 1:2.

To do stoichiometry, we will multiply the moles of HCl by the ratio of H2O to HCl, which is just dividing by 2.

The theoretical yield of water is then 0.175 moles HCl * [tex]\frac{1moleH2O}{2moleHCl}[/tex] = 0.1874 moles H2O.

Our theoretical yield is 0.0874 moles H2O. But the question and the actual yield are in grams, so we will convert this to grams. To convert moles to grams, just multiply the moles by the molar mass. The molar mass of water is 18.0 g/mol, so

0.0874*18.0 = 1.57 g

The theoretical yield is 1.57 g H2O

Percent Yield

Percent yield is much easier. Percent yield is

((actual yield)/(theoretical yield))*100

In this case, our actual yield is 1.11 grams and our theoretical yield is 3.15 grams, so

[tex]\frac{1.11}{1.57} =[/tex] 70.5%

70.5% is the percent yield.

The percentage of plants showing phototropism is the dependent variable, and the color of the light is the independent variable. Therefore, the correct answer is: "the percentage of plants showing phototropism is the dependent variable, and the color of the light is the independent variable."

The dependent variable is the variable that is being measured or observed, and its value depends on the independent variable, which is the variable that is being manipulated or changed in the experiment. In this experiment, the percentage of plants showing phototropism is being measured, which means that it is the dependent variable. The color of the light is being manipulated, which means that it is the independent variable.

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Answer:

G, A, A, T, C, C, G, A, A, T, G, G, T

Explanation:

The LD50 concentration of CuSO₄ for brine shrimp is reported to be around 2.75 ppm (parts per million), which means that if 50% of the brine shrimp population were exposed to this concentration of CuSO₄, they would die as a result of the exposure

The LD50 and ED50 are both terms commonly used in toxicology to express the effectiveness or toxicity of a substance.

The LD50, which stands for "lethal dose 50," is the amount of a substance required to cause death in 50% of the test population. It is typically expressed in units of milligrams or micrograms of the substance per kilogram of body weight of the test animal.

On the other hand, the ED50 stands for "effective dose 50," which is the amount of a substance required to produce a desired effect in 50% of the test population. It is commonly used in pharmacology to measure the potency of a drug.

In the case of the brine shrimp, the LD50 concentration of CuSO4 (copper sulfate) would be the amount of CuSO4 that would cause the death of 50% of the shrimp population in a given test. It is important to note that the LD50 can vary depending on various factors such as the species being tested, the method of exposure, and the duration of exposure.

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When the coefficients in the redox reaction are doubled, the given quantities will be affected for a voltaic cell under nonstandard conditions in the following ways.

Explanation:

An increase in the coefficients of a balanced redox reaction increases the number of moles of the reacting species. Thus, an increase in the coefficients of a redox reaction would result in an increase in the cell potential.

Furthermore, the reaction quotient Q would become smaller due to an increase in the concentrations of products and a decrease in the concentrations of reactants. This shift toward the products would make the reaction more spontaneous.The increase in coefficients would result in an increase in the molar quantities of each species, resulting in a change in the Q value. The standard EMF of the cell is unaffected since it is based solely on standard conditions. The value of ΔG, which is directly related to the potential difference in a galvanic cell, changes as the value of Q changes.

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Tech A is correct who says that overheated catalysts cannot be restored and must be replaced.

In chemistry, a catalyst is any substance that speeds up a reaction without consuming itself. Many crucial biochemical reactions are catalysed by enzymes, which are substances that occur naturally.

The majority of solid catalysts are made of metals, or the oxides, sulphides, and halides of metals, as well as of the semimetallic elements silicon, aluminium, and boron. Solid catalysts are frequently dispersed in materials known as catalyst supports, while gaseous and liquid catalysts are typically used in their pure form or in combination with appropriate carriers or solvents.

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The part 2 in the attached image will undergo reduction with sodium borohydride.

Sodium borohydride (NaBH₄) is a commonly used reducing agent in organic chemistry. It is primarily used to reduce carbonyl groups (aldehydes and ketones) to their corresponding alcohols. Sodium borohydride can also reduce some other functional groups, such as imines and acid chlorides, but its reactivity towards these groups is much lower compared to carbonyls.

In general, the carbonyl groups in a molecule are the most likely functional groups to undergo reduction with sodium borohydride. Other functional groups such as alkenes, alkynes, aromatic rings, and alcohols are generally unreactive towards sodium borohydride.

Therefore, if your compound contains any carbonyl groups (such as aldehydes or ketones), those groups would be the most likely candidates for reduction with sodium borohydride. Part 2 is a carbonyl group, hence it will react.

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When a stock solution is diluted, the number of moles of solute (NaNO3 in this case) remains constant. Therefore, we can use the following equation to find the final molarity of the diluted solution:

M1V1 = M2V2

where M1 is the initial molarity (0.275 M), V1 is the initial volume (15.00 mL), M2 is the final molarity (what we want to find), and V2 is the final volume (100.0 mL).

First, we need to convert the initial volume from milliliters to liters:

V1 = 15.00 mL = 0.01500 L

Next, we can substitute the given values into the equation:

(0.275 M) × (0.01500 L) = M2 × (0.1000 L)

Solving for M2, we get:

M2 = (0.275 M × 0.01500 L) ÷ 0.1000 L

M2 = 0.04125 M

Therefore, the final molarity of the NaNO3 solution is 0.04125 M.

The acid dissociation constant of hexanoic acid is 4.93 × 10^-10 mol/L.

When measuring the pH of a solution of hexanoic acid to be 4.96, the acid dissociation constant of hexanoic acid can be calculated. This can be done through the following equation:

Ka = [H3O+][A-] / [HA]whereKa

= acid dissociation constantH3O+

= hydronium ionA-

= conjugate baseHA

= acidThe pH of the solution of hexanoic acid is measured to be 4.96.

Thus, [H3O+] is equal to 10^-4.96 or 7.02 × 10^-5 M.

The initial concentration of the hexanoic acid is equal to the concentration of the undissociated acid or [HA].The acid dissociation constant of hexanoic acid can be calculated by plugging the known values into the equation:

Ka = [7.02 × 10^-5][A-] / [HA]The concentration of the conjugate base, A-, is equal to the concentration of the dissociated acid, which is equal to [H3O+].

Thus,Ka = [7.02 × 10^-5]^2 / [HA]Ka = 4.93 × 10^-10 mol/L

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The enthalpy change or AH for the reaction is -1560.9 kJ/mol. This negative value indicates that the reaction is exothermic, meaning it releases energy in the form of heat to the surroundings.

C2H4 (g) + 3O2 (g) → 2H2O (g) + 2CO2 (g)

We can use the standard enthalpies of formation (∆Hf°) of the products and reactants to determine the overall enthalpy change. The ∆Hf° values can be found in a reference table or online database.

The balanced equation tells us that 1 mole of C2H4 reacts with 3 moles of O2 to form 2 moles of H2O and 2 moles of CO2. So, we can write:

ΔH° = [2∆Hf°(H2O) + 2∆Hf°(CO2)] - [∆Hf°(C2H4) + 3∆Hf°(O2)]

Substituting the ∆Hf° values for each substance, we get:

ΔH° = [2(-241.8 kJ/mol) + 2(-393.5 kJ/mol)] - [(52.3 kJ/mol) + 3(0 kJ/mol)] ΔH° = -1560.9 kJ/mol

Therefore, the enthalpy change or AH for the reaction is -1560.9 kJ/mol. This negative value indicates that the reaction is exothermic, meaning it releases energy in the form of heat to the surroundings.

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The presence of hydrogen would be indicated by a pale blue flame that is nearly invisible in broad daylight, but the presence of carbon dioxide would be indicated by the flame going out.

A flame ignited by hydrogen gas emits a barely perceptible pale blue flame under normal lighting conditions. This is due to the flame that hydrogen gas produces mostly emitting light in the ultraviolet spectrum, which is invisible to the human eye.

On the other side, a flame is put out when carbon dioxide gas is added to it. This is because carbon dioxide is a gas that does not support burning and is not flammable.

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