The graph shows the reaction AB → A+B+ heat.
If the graph indicates how quickly the reaction is progressing,
then the concentration of which component of the equation is
shown in the graph?

Oreactant

O product A

O product B

O heat

Help asap 20pts

The ratio of aluminum to hydrogen in the reaction is 2:3. For every 2 moles of aluminum that reacts, 3 moles of hydrogen are produced.

The balanced chemical equation for the reaction 2Al + 3H₂SO₄ = 3H₂ + Al₂(SO₄)₃ shows that 2 moles of aluminum (2Al) reacts with 3 moles of sulfuric acid (3H₂SO₄) to produce 3 moles of hydrogen gas (3H₂) and 1 mole of aluminum sulfate (Al₂(SO₄)₃).

o express the ratio in terms of the number of atoms of each element involved in the reaction, we need to consider the coefficients of the balanced chemical equation. The coefficient in front of each element or compound indicates the number of moles of that substance involved in the reaction.

In the given equation, the coefficient for aluminum (Al) is 2 and the coefficient for hydrogen (H) is 6 (3 on each side). Therefore, the ratio of aluminum atoms to hydrogen atoms in the reaction is 2:6, which simplifies to 1:3.

So, for every one atom of aluminum that reacts, three atoms of hydrogen are produced. This can also be expressed as the molar ratio of aluminum to hydrogen, which is 2:3.

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The percentage of iron in ferric oxide is 70%.

Molecular formula of ferric oxide is [tex]Fe_{2} O_{3}[/tex].

First, we will calculate the total mass of ferric oxide.

Molecular weight of oxygen = 16

Molecular weight of iron = 56

Therefore, total mass of oxygen=3 × 16 =48 g

and total mass of iron=2 × 56 =112 g

Percentage of metal in the chemical = total mass of the metal/ total mass of the compound× 100

Now, total mass of ferric oxide = 48+ 112 =160 g

Percentage of iron in the chemical = total mass of the iron/ total mass of ferric oxide × 100= 112160 × 100=70 %

Therefore, the percentage of iron in ferric oxide is 70%.

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Answer:

Explanation:

need points :>

Answer:

Great question! Here are four body systems that are used when taking a test and how each helps: 1. Nervous system: The nervous system is responsible for processing information and responding to stimuli. It plays a crucial role in test-taking by allowing students to process and understand the questions being asked, recall the relevant information, and formulate responses. 2. Cardiovascular system: The cardiovascular system circulates blood throughout the body, providing oxygen and nutrients to the brain and other organs. During a test, the cardiovascular system helps to maintain focus and mental clarity by providing the brain with the energy it needs to function optimally. 3. Respiratory system: The respiratory system is responsible for taking in oxygen and expelling carbon dioxide. Proper breathing is essential during test-taking because it helps to reduce stress and anxiety, and provides oxygen to the brain, which is necessary for clear thinking. 4. Muscular system

Four key body systems that are used when taking a test are Nervous System, Circulatory System, Respiratory System, Musculoskeletal System

Nervous System: The nervous system is crucial for cognitive processes, including memory, attention, and problem-solving.

Circulatory System: The circulatory system, consisting of the heart, blood vessels, and blood, plays a vital role in delivering oxygen and nutrients to the brain.

Respiratory System: The respiratory system is responsible for supplying oxygen to the body and eliminating carbon dioxide.

Musculoskeletal System: The musculoskeletal system, consisting of bones, muscles, and joints, supports posture and physical stability during the test.

Hence, four body systems are explained above.

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Explanation:

We can use the ideal gas law to calculate the mass of the N2 gas sample:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant (0.08206 L·atm/mol·K), and T is the temperature.

First, we need to convert the temperature to Kelvin:

T = 50 °C + 273.15 = 323.15 K

Now we can rearrange the ideal gas law to solve for the number of moles:

n = PV/RT

n = (3 atm)(0.6 L)/(0.08206 L·atm/mol·K)(323.15 K)

n = 0.0705 mol

The molar mass of N2 is 28.02 g/mol, so we can calculate the mass of the N2 gas sample:

mass = n × molar mass

mass = 0.0705 mol × 28.02 g/mol

mass = 1.98 g

Therefore, the mass of the N2 gas sample is approximately 1.98 g.

The probability that two heterozygous individuals will have a child together with the short earlobes phenotype is 15%.

The likelihood of the genotype and phenotype of the progeny can be calculated using a Punnett square. Let's refer to the long earlobe gene as "L" and the short earlobe allele as "l."

The probability of each genotype is:

LL = 1/4

Ll = 1/2

ll = 1/4

Now we need to take into account the 60% penetrance of the short earlobes genotype. This means that even if an individual has the genotype for short earlobes (ll), they may not actually exhibit the phenotype.

So the probability of having the short earlobes phenotype is:

P(short earlobes phenotype) = P(ll) x 0.6

P(ll) = 1/4

Substituting in:

P(short earlobes phenotype) = (1/4) x 0.6

P(short earlobes phenotype) = 0.15 or 15%

The probability that two heterozygous individuals will have a child together with the short earlobes phenotype is 15%.

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Answer:

(a) Electrode reactions:

Pt/H+/H2: 2H+(aq) + 2e- -> H2(g) (reduction)

Ag/AgCl/Cl-: AgCl(s) + e- -> Ag(s) + Cl-(aq) (reduction)

Overall cell equation: 2AgCl(s) + H2(g) -> 2Ag(s) + 2HCl(aq)

(b) Direction of motion of ions and electrons:

In the Pt/H+/H2 half-cell, hydrogen ions (H+) move towards the platinum electrode and accept electrons to form hydrogen gas (H2). In the Ag/AgCl/Cl- half-cell, silver ions (Ag+) move towards the silver chloride (AgCl) electrode and accept electrons to form silver (Ag) metal while chloride ions (Cl-) move away from the electrode. Electrons move from the hydrogen electrode to the silver electrode through the external circuit.

(c) Electrode labeling:

The Pt/H+/H2 electrode is the cathode (-) and the Ag/AgCl/Cl- electrode is the anode (+).

(d) Standard cell potential (Eo):

The standard cell potential can be calculated using the standard reduction potentials for each half-cell:

Eo(cell) = Eo(reduction, Ag/AgCl/Cl-) - Eo(reduction, Pt/H+/H2)

Eo(reduction, Ag/AgCl/Cl-) = +0.222 V (from standard reduction potential tables)

Eo(reduction, Pt/H+/H2) = 0 V (by definition)

Eo(cell) = +0.222 V - 0 V = +0.222 V

(e) Actual cell potential (E):

E(cell) = Eo(cell) - (0.0592 V / n) * log[H3O+]

where n is the number of electrons transferred in the balanced equation (2 in this case)

E(cell) = +0.222 V - (0.0592 V / 2) * log(1.0 x 10^-4 M)

E(cell) = +0.222 V - (0.0296 V) = +0.1924 V

(f) Values of constants A and B:

E(cell) = A + B.pH

At pH 7 (neutral), E(cell) = Eo(cell) = +0.222 V

Therefore, A = +0.222 V and B = -0.0592 V/pH

Answer:

the rate constant of the reaction is approximately 0.0021 s^-1.

Explanation:

To calculate the rate constant of a first-order reaction, we can use the following equation:

ln([A]t/[A]0) = -kt

Where [A]t is the concentration of reactant at time t, [A]0 is the initial concentration of reactant, k is the rate constant, and t is time.

Given that the reaction is 45% complete after 400 s, we can assume that [A]t/[A]0 = 0.55 (since 100% - 45% = 55%). Plugging this value into the equation above, we get:

ln(0.55) = -k(400)

Solving for k, we get:

k = -ln(0.55)/400

k ≈ 0.0021 s^-1

A first-order reaction is 45% complete after 400 s. Therefore, 0.0021 s⁻¹ is the rate constant of the reaction.

The chemical kinetics rate law, which connects the molecular concentration of reacting substances to reaction rate, uses the rate constant as a proportionality factor. The letter k in an equation designates it, which is also referred to as either the resultant rate constant and reaction rate coefficient.

The link among the molecular concentration of reactants with the rate for a chemical reaction is shown by the proportionality constant k. Utilising the molecular weights of each of the reactants with the sequence of the reaction, the rate constant can be calculated experimentally. As an alternative, the Arrhenius equation can be used to compute it.

ln([A]t/[A]0) = -kt

[A]t/[A]0 = 0.55

ln(0.55) = -k(400)

k = -ln(0.55)/400

k ≈ 0.0021 s⁻¹

Therefore, 0.0021 s⁻¹ is the rate constant.

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The molecular formula of the compound is [tex]C_6H_{12}O_6[/tex] whose molar mass is 180.16g/mol with mass percent composition: C 40.00%, H 6.72%, O 53.28%.

Given the mass percent compositions as:

the mass percent composition of carbon (C) = 40.00%

the mass percent composition of hydrogen (H) = 6.72%

the mass percent composition of oxygen (O) = 53.28%

The molar mass of the compound is  = 180.16 g/mol.

Let us assume we have 100g of compound then,

we have 40g of carbon, 6.72g of hydrogen and 53.28g of oxygen.

The atomic masses of carbon, hydrogen, and oxygen, respectively, are 12.01 g/mol, 1.01 g/mol, and 16.00 g/mol.

We need to calculate the number of moles of each element present in the compound.

Number of moles of carbon = 40.00/12.01 g/mol = 3.33 moles

Number of moles of hydrogen = 6.72/1.01 g/mol = 6.65 moles

Number of moles of oxygen = 53.28/16.00 g/mol = 3.33 moles

Total number of moles = 3.33 + 6.65 + 3.33 = 13.31 moles

Mole ratio of carbon, hydrogen and carbon = 3.33 : 6.65 : 3.33

Mole ratio of carbon, hydrogen and carbon = 1 : 2 : 1

The empirical formula is = [tex]CH_2O[/tex]

The empirical formula mass of [tex]CH_2O[/tex] is = 30.03

n = 180.18/30.03 = 6

The molecular formula is = [tex]C_6H_{12}O_6[/tex]

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Answer:

the pressure of the gas is 1.67 atm when the volume increased to 4.5 L.

Explanation:

Assuming the temperature and the amount of gas remain constant (i.e., the process is isobaric):

Using Boyle's law, we can relate the initial pressure (P1) and volume (V1) to the final pressure (P2) and volume (V2):

P1V1 = P2V2

Plugging in the given values:

P1 = 1.50 atm

V1 = 5.00 L

V2 = 4.5 L

Solving for P2:

P2 = (P1V1)/V2 = (1.50 atm x 5.00 L)/4.5 L = 1.67 atm

Fe²⁺ is the reducing agent since in the given redox reaction it loses electrons which are transferred to another species.

A reducing agent, also known as a reductant, is a substance that causes a reduction in another substance by donating electrons or by removing oxygen from the substance being reduced. In other words, it is a substance that facilitates a chemical reaction by undergoing oxidation itself.

A reducing agent is typically an electron donor and is oxidized during the reaction. Examples of reducing agents include metals like zinc, hydrogen gas, and organic compounds like alcohols and sugars.

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Answer: 0.10

I'm bad at explaining but trust, I had the same question.

CH2, N2O3 are covalent

NH4ClO, Fe3(PO4)2 and CrBr2 are ionic

Ionic compounds are formed when a metal atom donates one or more electrons to a nonmetal atom. This transfer of electrons creates ions, which are charged particles that attract each other due to their opposite charges.

Covalent compounds, on the other hand, are formed when two or more nonmetal atoms share electrons. In this type of bonding, each atom contributes one or more electrons to a shared pair, creating a covalent bond.

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Answer:

9mol N

Explanation:

The balanced chemical equation is:

N₂ + 3H₂ → 2NH₃

According to the stoichiometry of this reaction, 1 mole of N₂ reacts with 3 moles of H₂ to produce 2 moles of NH₃.

So, to produce 2 moles of NH₃, we need 1 mole of N₂.

Therefore, to produce 18 moles of NH₃, we would need:

18 mol NH₃ × (1 mol N₂ / 2 mol NH₃) = 9 mol N₂

Thus, 9 moles of nitrogen are required to produce 18 mol of NH₃.

Answer:

the molarity of the HCl is 1.17 M.

Explanation:

The balanced chemical equation for the reaction between HCl and NaOH is:

HCl + NaOH -> NaCl + H2O

From the equation, we can see that one mole of HCl reacts with one mole of NaOH to produce one mole of NaCl and one mole of water.

First, let's calculate the number of moles of NaOH used:

moles of NaOH = Molarity x Volume in liters

moles of NaOH = 0.650 M x 0.0900 L

moles of NaOH = 0.0585 mol

Since the reaction between HCl and NaOH is a 1:1 stoichiometry, the number of moles of HCl is also equal to 0.0585 mol.

Now, we can use the number of moles of HCl and the volume of HCl to calculate the molarity:

Molarity of HCl = moles of HCl / Volume in liters

Molarity of HCl = 0.0585 mol / 0.0500 L

Molarity of HCl = 1.17 M

Therefore, the molarity of the HCl is 1.17 M.

For a 1-gram piece of magnesium, the amount of MgO produced by Mg is less than the amount produced by O2. Therefore, Mg is the limiting reactant and O2 is in excess.

For a 1000-gram piece of magnesium, the amount of MgO produced by Mg is still less than the amount produced by O2, even though there is a lot more Mg present. Therefore, Mg is still the limiting reactant and O2 is in excess.

To determine which reactant is limiting and which is in excess, we need to calculate the amount of product that each reactant can produce and compare them.

For a 1-gram piece of magnesium:

Moles of Mg = mass/Molar mass = 1 g/24.31 g/mol = 0.041 moles

Moles of O2 = volume x pressure/RT = (22.4 L at STP x 1 atm)/(0.0821 L·atm/mol·K x 273 K) = 1.0 moles

According to the balanced equation, 2 moles of Mg reacts with 1 mole of O2 to produce 2 moles of MgO

Therefore, the amount of MgO produced by 0.041 moles of Mg would be (2/2) x 0.041 moles = 0.041 moles

The amount of MgO produced by 1 mole of O2 would be (2/1) x 0.041 moles = 0.082 moles

We can see that the amount of MgO produced by Mg is less than the amount produced by O2. Therefore, Mg is the limiting reactant and O2 is in excess.

For a 1000-gram piece of magnesium:

Moles of Mg = mass/Molar mass = 1000 g/24.31 g/mol = 41.1 moles

Moles of O2 = volume x pressure/RT = (22.4 L at STP x 1 atm)/(0.0821 L·atm/mol·K x 273 K) = 1.0 moles

According to the balanced equation, 2 moles of Mg reacts with 1 mole of O2 to produce 2 moles of MgO

Therefore, the amount of MgO produced by 41.1 moles of Mg would be (2/2) x 41.1 moles = 41.1 moles

The amount of MgO produced by 1 mole of O2 would be (2/1) x 41.1 moles = 82.2 moles

We can see that the amount of MgO produced by Mg is still less than the amount produced by O2, even though there is a lot more Mg present. Therefore, Mg is still the limiting reactant and O2 is in excess.

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Assuming the acid used for titration is a strong acid (such as HCl), the balanced chemical equation for the reaction would be:

HCl + NaOH → NaCl + H2O

From the equation, we can see that 1 mole of HCl reacts with 1 mole of NaOH. Therefore, the number of moles of HCl used for titration can be calculated as:

moles of HCl = moles of NaOH = M x V x n

where M is the molarity of NaOH, V is the volume of NaOH used (100 mL or 0.1 L), and n is the number of moles of NaOH per liter of solution (1 mole/L).

moles of HCl = 0.15 M x 0.1 L x 1 mol/L = 0.015 mol

Since the volume of acid used for titration is 150 mL or 0.15 L, we can calculate the molarity of the acid as:

Molarity of acid = moles of acid / volume of acid used

Molarity of acid = 0.015 mol / 0.15 L = 0.1 M

Therefore, the molarity of the acid solution is 0.1 M.

Based on public policy, the most recent scientific findings, and efficient management, we give leadership on matters relating to food, agriculture, energy wealth, rural development, nutrition, & related topics.

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The demand for biotechnology is growing in industries including pharmaceutical, animal husbandry, agricultural, healthcare, medicine, genetic engineering, etc. In addition, biotechnologists are well compensated for their work. Thus, it is undoubtedly a smart professional choice.

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The heat for the reaction per gram of ZnS used is -4.51 kJ/g.

To calculate the heat for the reaction per gram of ZnS used, we need to first calculate the amount of heat released per mole of ZnS used and then convert that to per gram.

The given balanced chemical equation shows that 2 moles of ZnS react with 3 moles of O2 to produce 2 moles of ZnO and 2 moles of SO2, and the amount of heat released during the reaction is -879 kJ/mol.

So, the amount of heat released per mole of ZnS used is:

(-879 kJ/mol) / 2 = -439.5 kJ/mol

Now, to calculate the amount of heat released per gram of ZnS used, we need to divide the amount of heat released per mole by the molar mass of ZnS:

-439.5 kJ/mol / 97.46 g/mol = -4.51 kJ/g.

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The amount of potassium permanganate (KMnO4) in the volumetric pipette and the 100 ml solution is the same.

When a volumetric pipette is used to take 10 ml of the stock solution, it is designed to deliver an accurate volume of liquid, ensuring that the amount of solute (KMnO4) is accurately transferred to the flask. By adding water to the volumetric flask to make a more dilute solution, the total amount of solute (KMnO4) remains the same, but it is now distributed throughout the larger volume of the flask.

Therefore, there is no more or less KMnO4 in the volumetric pipette or the 100 ml solution. Both contain the same amount of KMnO4, which was accurately transferred using the volumetric pipette. It is important to note that accuracy in transferring the correct volume is critical in ensuring that the concentration of the diluted solution is correct.

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Answer:

Disproportionation reactions involve a molecule being both oxidized and reduced simultaneously, while comproportionation reactions involve two different species reacting to form a single product with an intermediate oxidation state.

For example, the reaction of hydrogen peroxide (H2O2) with potassium permanganate (KMnO4) is a disproportionation reaction, which can be represented as:

For example, the reaction of sodium thiosulfate (Na2S2O3) with iodine (I2) is a comproportionation reaction, which can be represented as:

One mole of carbon dioxide would require 84.01 grams of NaHCO₃.

It is discovered that the ratio of moles of CO₂ generated to moles of NaHCO₃ reacted is 1:2.

We can observe from this equation that 1 mole of NaHCO₃ results in 1 mole of CO₂. As a result, NaHCO₃ and CO₂ have a molar ratio of 1:1.

Na2CO₃(s) + H₂O(g) + CO₂ = 2 NaHCO₃(s)(g)

CO₂ has a molar mass of about 44.01 g/mol. As a result, we must determine how much NaHCO₃ weighs in relation to one mole of CO₂. Using the molar mass of NaHCO₃, the following can be calculated:

Molar mass of NaHCO₃ is 84.01 g/mol.

The mass of NaHCO₃ needed to create one mole of CO₂ is as follows:

(84.01 g NaHCO₃/1 mole NaHCO₃) = 84.01 g CO₂/mol for 1 mole of NaHCO₃.

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There are approximately [tex]1.2*10^17[/tex] molecules of food dye in the last solution.

Assuming that one drop of 100% solution is approximately 0.1 mL, then 10 drops of the 100% solution would be equivalent to 1 mL. If this 1 mL of the 100% solution was diluted to a final volume of 50 mL, then the dilution factor is 50.

Using the given approximation of 1 gram of food dye having approximately [tex]1.2*10^22[/tex] molecules, we can calculate the number of molecules in the original 1 mL of the 100% solution to be:

1 g * ([tex]1.210^22[/tex]molecules/g) = [tex]1.210^22[/tex]molecules

For the first dilution, the number of molecules would be 1/10th of this value, or:

(1/10) * [tex]1.210^221.210^22[/tex] = [tex]1.210^21[/tex]molecule

For the second dilution, the number of molecules would be 1/10th of this value, or:

[tex](1/10) * 1.210^21 = 1.210^20[/tex] molecules

If this process was repeated for a total of 5 dilutions, the number of molecules in the final solution would be:

[tex](1/10)^5 * 1.210^22 = 1.210^17[/tex]molecules

Therefore, there are approximately [tex]1.2*10^17[/tex] molecules of food dye in the last solution.

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Approximately 5.43 x [tex]10^{13}[/tex] moles of NaCl are extracted each year from the largest salt mine in the world.

What is NaCl?

NaCl is the chemical formula for table salt, which is a compound made up of sodium and chlorine ions. It is a white, crystalline solid that is commonly used as a seasoning and preservative in food, as well as in many industrial processes. NaCl is highly soluble in water and is an important electrolyte in the human body, helping to regulate many physiological processes.

First, we need to convert 7.00 million tons to kilograms:

7.00 million tons x 2,000 lb/ton x 1 kg/2.205 lb = 3.17 x [tex]10^{9}[/tex]kg

Next, we need to calculate the number of moles of NaCl present in this amount of halite:

Molar mass of NaCl = 58.44 g/mol

3.17 x [tex]10^{9}[/tex] kg x 1000 g/kg / 58.44 g/mol = 5.43 x [tex]10^{13}[/tex] moles of NaCl

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Answer:

To solve the problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas:

(P1V1) / T1 = (P2V2) / 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 = 750 mmHg, V1 = 1.27 L, T1 = 298 K, V2 = 0.75 L, T2 = 448 K, and the amount of gas does not change.

First, we can solve for P2 by rearranging the equation as:

P2 = (P1V1T2) / (V2T1)

Substituting the values we get:

P2 = (750 mmHg x 1.27 L x 448 K) / (0.75 L x 298 K)

P2 = 1504 mmHg

Therefore, the final pressure at a volume of 0.75 L and a temperature of 448 K is 1504 mmHg.

Answer:

2) 110 g P2O3

Explanation:

If the green box is in the denominator of a fraction and represents the molar mass of P2O3, then the correct answer choice would be 2) 110 g P2O3. Here’s how you can use this value to solve the problem:

The balanced chemical equation for the reaction between P2O3 and H2O to produce H3PO3 is: P2O3 + 3H2O → 2H3PO3.

From this equation, we can see that 1 mole of P2O3 reacts with 3 moles of H2O to produce 2 moles of H3PO3. So the number of moles of H3PO3 produced is twice the number of moles of P2O3 that reacted.

The molar mass of P2O3 is approximately 110 g/mol. So 93.2 g of P2O3 is equivalent to (93.2 g) / (110 g/mol) = 0.848 mol of P2O3.

Since the number of moles of H3PO3 produced is twice the number of moles of P2O3 that reacted, the number of moles of H3PO3 produced is 0.848 mol × 2 = 1.696 mol.

The molar mass of H3PO3 is (3 × 1.01 g/mol) + (1 × 30.97 g/mol) + (3 × 16.00 g/mol) = 81.99 g/mol. So 1.696 mol of H3PO3 is equivalent to (1.696 mol) × (81.99 g/mol) = 139 g of H3PO3.

So the complete reaction of 93.2 g P2O3 would produce approximately 139 g of H3PO3.

In both fusion and fission, stability decreases as a result of the reaction. In fusion, two smaller nuclei combine to form a larger nucleus, releasing energy in the process.

The resulting nucleus may be unstable and undergo radioactive decay, which can further release energy. In fission, a larger nucleus is split into smaller nuclei, also releasing energy. The resulting nuclei may also be unstable and undergo radioactive decay. In both cases, the process of splitting or combining nuclei releases energy, but it also reduces the overall stability of the resulting nuclei.

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Answer:

the sodium hydroxide solution was 0.4 M.

Explanation:

To solve this problem, we can use the dilution formula:

M1V1 = M2V2

where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume.

We are given that 45.0 mL of a sodium hydroxide solution was diluted and the resulting volume is 180 mL with a concentration of 0.100 M. Let's use M1 for the initial concentration, V1 for the initial volume, M2 for the final concentration, and V2 for the final volume.

M2 = 0.100 M

V1 = 45.0 mL

V2 = 180 mL

We can rearrange the dilution formula to solve for M1:

M1 = (M2V2) / V1

Substituting the given values, we get:

M1 = (0.100 M x 180 mL) / 45.0 mL

M1 = 0.400 M

Therefore, the initial molarity of the sodium hydroxide solution was 0.4 M.

The final balanced chemical equation is:

C₉H₂₀(l) + 14O₂(g) → 9CO₂(g) + 10H₂O(l)

A balanced chemical equation is a representation of a chemical reaction using chemical formulas and coefficients to show the reactants and products involved in the reaction.

To balance a chemical equation, coefficients are placed in front of the chemical formulas to ensure that the number of atoms of each element is equal on both sides of the equation. This results in a balanced equation that accurately represents the reactants and products involved in the reaction, and their relative amounts.

To balance the chemical equation, we need to make sure that the number of atoms of each element is the same on both sides of the equation.

Let's start by counting the number of atoms of each element in the reactants and products:

Reactants:

C₉H₂₀(l) → 9 carbon atoms (C), 20 hydrogen atoms (H)

O₂(g) → 2 oxygen atoms (O) per molecule, so 14 O₂ molecules give 28 oxygen atoms (O)

Products:

9CO₂(g) → 9 carbon atoms (C), 18 oxygen atoms (O)

10H₂O(l) → 20 hydrogen atoms (H), 10 oxygen atoms (O)

Now, we can see that the number of carbon and hydrogen atoms are already balanced, but we need to balance the oxygen atoms.

To do so, we can see that 14 O₂ molecules give us 28 oxygen atoms, which means we need 28/2 = 14 molecules of CO₂ and 14 molecules of H₂O to balance the equation.

The final balanced equation is:

C₉H₂₀(l) + 14O₂(g) → 9CO₂(g) + 10H₂O(l)

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Explanation:

a)Take percentages and divide by mole wt ( from periodic table) of the corresponding element

          C     14.25 / 12            = 1.1875

          O     56.93 / 15.99     = 3.56

          Mg   28.83/24.3        = 1.186        Divide by the smallest number

                        C 1.1875/1.186      = 1

                         O 3.56 / 1.186     = 3

                         Mg  1.186 / 1.186 =  1

C O3  Mg         commonly written as Mg CO3   ( magnesium carbonate)