Which solubility curve on the right best represents the data table on the left?

The concept Boyle's law is used here to determine the new pressure of air inside the balloon. For a gas the relationship between volume and pressure is expressed using Boyle's law. The new pressure is 400 kPa.

The Boyle's law states that at constant temperature, the volume of a given mass of gas is inversely proportional to its pressure. The product of pressure and volume of a given mass of gas is constant.

Mathematically PV = k

P₁V₁ = P₂V₂

P₂ = P₁V₁ / V₂

100 × 4 / 1 = 400 kPa

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Answer:

Molecular weight of CH4 is 16 CH4 has four hydrogen atoms 1 mole of a compound contain 6.023*1023 atoms 12 gm of CH4 = 0

Yes, two magnets can create magnetic force fields that allows them to interact without touching.

Magnetic forces are non contact forces; they pull or push on objects without touching them. Magnets are only attracted to a few 'magnetic' metals and not all matter. Yes, the investigation did answer the question about whether two magnets create magnetic force fields that allow them to interact without touching.

The investigation provided enough evidence to support the idea that invisible magnetic force fields exist:

The investigation involved observing how two magnets interact with each other without touching. The magnets were brought closer together until they interacted, and then they were moved further apart. This process was repeated several times, and the results were observed and recorded. During the investigation, it was observed that the magnets interacted with each other even when they were not touching. This interaction occurred because the magnets created magnetic force fields that allowed them to interact with each other even when they were not in direct contact. This is because the interaction between the magnets could not be explained by any other means except through the existence of magnetic force fields.

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The final pressure inside the tank is 88.9 kPa.

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

The combined gas law is given by:

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

where

P1 and T1 are the initial pressure and temperature of the gas,

V1 is the initial volume of the gas,

P2 is the final pressure of the gas,

V2 is the final volume of the gas, and

T2 is the final temperature of the gas.

We can assume that the volume of the gas in the tank remains constant, since it is a steel tank. Therefore, V1 = V2.

We can convert the temperatures to Kelvin by adding 273.15 to each temperature value. Therefore,

T1 = 173.15 K and

T2 = 308.15 K.

Substituting these values into the combined gas law, we get:

(50.0 kPa * V1) / (173.15 K) = (P2 * V1) / (308.15 K)

P2 = (50.0 kPa * 308.15 K) / 173.15 K

P2 = 88.98 kPa

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Answer:

88.98 kPa (2 d.p.)

Explanation:

To find the final pressure inside the steel tank, we can use Gay-Lussac's law since the volume is constant.

[tex]\boxed{\sf \dfrac{P_1}{T_1}=\dfrac{P_2}{T_2}}[/tex]

where:

As we are solving for the final pressure, rearrange the equation to isolate P₂:

[tex]\sf P_2=\dfrac{P_1T_2}{T_1}[/tex]

Convert the given temperatures from Celsius to Kelvin by adding 273.15:

[tex]\implies \sf T_1=-100+273.15=173.15\;K[/tex]

[tex]\implies \sf T_2=35+273.15=308.15\;K[/tex]

Therefore, the values to substitute into the equation are:

Substitute the values into the equation and solve for P₂:

[tex]\implies \sf P_2=\dfrac{50.0\cdot 308.15}{173.15}[/tex]

[tex]\implies \sf P_2=\dfrac{15407.5}{173.15}[/tex]

[tex]\implies \sf P_2=88.98354028...[/tex]

[tex]\implies \sf P_2=88.98\;kPa\;(2\;d.p.)[/tex]

Therefore, the final pressure inside the steel tank is 88.98 kPa when the temperature is increased from -100.0°C to 35.0°C.

Answer:

It off soudium and i know this from experments so the answear is b

Explanation:

To solve the financial dilemma, the chemical company can consider using the excess silver nitrate solution to synthesize silver nanoparticles, which have various applications in industries.

Silver nanoparticles can be synthesized by reducing silver ions with a reducing agent, and silver nitrate can serve as a source of silver ions.

One possible reaction for the synthesis of silver nanoparticles using silver nitrate is the reduction of silver ions with sodium borohydride (NaBH4). The reaction can be represented as:

AgNO3 + NaBH4 → Ag nanoparticles + NaNO3 + B2H6

In this reaction, silver nitrate is the oxidizing agent, which accepts electrons, while sodium borohydride is the reducing agent, which donates electrons to reduce the silver ions. The reaction also produces sodium nitrate and borane gas as byproducts.

The synthesized silver nanoparticles can be sold to various industries, generating revenue for the company and potentially reducing their debt. The company can also consider optimizing the synthesis process to increase the yield and purity of the silver nanoparticles, which can increase their market value.

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When 250.0 g of lead is cooled from 15.0°C to 12.0°C, approximately 29.36 calories of energy (heat) are released.

To calculate the amount of energy (heat) released when 250.0 g of lead is cooled from 15.0°C to 12.0°C, we need to use the specific heat capacity and the change in temperature of lead. The specific heat capacity of lead is 0.128 J/g°C.

The equation to calculate the energy released (Q) is:

Q = m × c × ΔT

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

Substituting the given values, we get:

Q = 250.0 g × 0.128 J/g°C × (12.0°C - 15.0°C)

Q = - 122.88 J

The negative sign indicates that energy is being released, as the lead is losing heat. To convert this to calories, we need to divide by the conversion factor of 4.184 J/cal:

Q = - 122.88 J ÷ 4.184 J/cal

Q ≈ - 29.36 cal

Therefore, when 250.0 g of lead is cooled from 15.0°C to 12.0°C, approximately 29.36 calories of energy (heat) are released.

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The process of carbon dioxide getting into the atmosphere primarily occurs through natural processes like respiration, volcanic eruptions, and decay of organic matter.

However, human activities like burning of fossil fuels and deforestation have significantly increased the levels of carbon dioxide in the atmosphere. When these fuels are burned, they release carbon dioxide into the air, which contributes to the greenhouse effect, trapping heat in the atmosphere and leading to global warming. Additionally, deforestation reduces the number of trees that absorb carbon dioxide through photosynthesis, further exacerbating the problem.

Overall, the process of carbon dioxide getting into the atmosphere is a complex interaction between natural and human-induced factors that have significant impacts on our planet.

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The new volume of the gas at STP is 163.8 mL. The pressure in the aerosol can at a temperature of 60 C is 8.4 atm. The volume of nitrogen at STP is 558.8 mL.

1. To solve for the new volume of the gas at STP, we can use the combined gas law equation:

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

where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2 and T2 are the new pressure and temperature, respectively, at STP. We know that STP is defined as 1 atm and 273 K.

Plugging in the given values, we get:

(6 atm x 10 mL)/100 K = (1 atm x V2)/273 K

Simplifying and solving for V2, we get:

V2 = (6 atm x 10 mL x 273 K)/(100 K x 1 atm) = 163.8 mL

Therefore, the new volume of the gas at STP is 163.8 mL.

2.To solve for the pressure in the aerosol can at a temperature of 60 C, we can use the combined gas law equation again:

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

where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2 and T2 are the new pressure and temperature, respectively, at 60 C. We know that V1 is constant since the can is sealed.

Plugging in the given values, we get:

(8 atm x V1)/318 K = (P2 x V1)/333 K

Simplifying and solving for P2, we get:

P2 = (8 atm x 333 K)/(318 K) = 8.4 atm

Therefore, the pressure in the aerosol can at a temperature of 60 C is 8.4 atm.

3. To solve for the volume of nitrogen at STP, we can use the combined gas law equation again:

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

where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2 and T2 are the new pressure and temperature, respectively, at STP. We know that P1 is constant since it is given that the pressure is constant.

Plugging in the given values and using the values for STP, we get:

(1 atm x 600 mL)/(293 K) = (P2 x V2)/(273 K)

Simplifying and solving for V2, we get:

V2 = (1 atm x 600 mL x 273 K)/(293 K) = 558.8 mL

Therefore, the volume of nitrogen at STP is 558.8 mL.

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In your gas sample, there are approximately 1.21 moles of gas.

To determine the number of moles of gas in the sample, you can use the ideal gas law formula: PV = nRT. In this formula, P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L atm/mol K), and T is the temperature in Kelvin.

1. Convert the pressure to atm: (1663 mmHg) * (1 atm/760 mmHg) = 2.19 atm.

2. Convert the temperature to Kelvin: (83°C) + 273.15 = 356.15 K.

3. Rearrange the formula to solve for n: n = PV/RT.

4. Plug in the values: n = (2.19 atm) * (22.4 L) / (0.0821 L atm/mol K) * (356.15 K).

5. Calculate the number of moles: n = 1.21 moles (rounded to two decimal places).

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In this case, the error is 0%, indicating that your experimental value is identical to the known value.

To calculate the error between your calculated specific heat of each metal and the known values in Table C, you can use the following formula:

Error = [(Calculated specific heat of metal - Known specific heat of metal) / Known specific heat of metal] x 100

Here are the steps to follow:

Look up the known specific heat of each metal in Table C.

Calculate the specific heat of each metal using your experimental data.

Substitute the known and calculated specific heats of each metal into the formula above.

Calculate the error for each metal by performing the subtraction and division operations.

Multiply the result by 100 to express the error as a percentage.

For example, let's say you conducted an experiment to measure the specific heat of copper and obtained a value of 0.39 J/g°C. The known specific heat of copper from Table C is 0.39 J/g°C.

To calculate the error:

Error = [(0.39 J/g°C - 0.39 J/g°C) / 0.39 J/g°C] x 100

Error = 0 / 0.39 J/g°C x 100

Error = 0%

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Part A: 0.568 L, Part B: 0.071 L, Part C: 0.140 L

Part A: To find the volume of the 0.211 M KCl solution that contains 0.12 mol of KCl, use the formula:

M = mol / L
0.211 M = 0.12 mol / volume

Rearranging the formula and solving for the volume:

Volume = 0.12 mol / 0.211 M = 0.568 L

Part B: To find the volume of the 1.7 M KCl solution that contains 0.12 mol of KCl:

1.7 M = 0.12 mol / volume

Volume = 0.12 mol / 1.7 M = 0.071 L

Part C: To find the volume of the 0.855 M KCl solution that contains 0.12 mol of KCl:

0.855 M = 0.12 mol / volume

Volume = 0.12 mol / 0.855 M = 0.140 L

So, the volumes containing 0.12 mol of KCl are as follows:
Part A: 0.568 L
Part B: 0.071 L
Part C: 0.140 L

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We can distinguish 4-hydroxy-4-methyl-2-pentanone (side product) from the major product.

To distinguish 4-hydroxy-4-methyl-2-pentanone (side product) from the major product using physical properties, you should consider the following factors:

1. Molecular weight: Calculate the molecular weight of both the side product and the major product. Different molecular weights result in different physical properties.

2. Boiling point: The boiling point of each compound may vary, so compare their boiling points to distinguish between them.

3. Melting point: Like the boiling point, the melting point of each compound may be different, allowing you to differentiate them.

4. Solubility: Check the solubility of both compounds in different solvents. Their solubility may differ in various solvents, helping you identify each compound.

5. Polarity: Determine the polarity of each compound by looking at their molecular structures. Different polarities can affect various physical properties, such as solubility and boiling points.

6. Spectroscopy: Analyze the compounds using spectroscopic techniques like infrared (IR), nuclear magnetic resonance (NMR), or mass spectrometry (MS). Each compound will have unique spectroscopic properties, which can be used for identification.

By comparing and analyzing these physical properties, you can distinguish 4-hydroxy-4-methyl-2-pentanone (side product) from the major product.

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0.06 moles of glucose can be broken down with 0.36 moles of oxygen.

To determine how many moles of glucose can be broken down with 0.36 moles of oxygen, we can use the stoichiometry of the reaction: C₆H₁₂O₆ + 6O₂ --> 6CO₂ + 6H₂O.

Step 1: Write the balanced equation.
C₆H₁₂O₆ + 6O₂ --> 6CO₂ + 6H₂O

Step 2: Identify the given amount and the substance you need to find.
Given: 0.36 moles of O₂
Find: moles of glucose (C₆H₁₂O₆)

Step 3: Use the stoichiometry from the balanced equation to find the moles of glucose.
According to the balanced equation, 6 moles of O₂ are required to break down 1 mole of glucose.

Step 4: Calculate the moles of glucose.
(0.36 moles O₂) x (1 mole glucose / 6 moles O₂) = 0.06 moles of glucose

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A chemist interested in the efficiency of a chemical reaction would calculate the percent yield. To do this, follow these steps:

1. Determine the balanced chemical equation for the reaction, which shows the stoichiometric relationship between reactants and products.

2. Identify the limiting reactant by comparing the initial amounts of reactants to their stoichiometric ratios in the balanced equation.

3. Calculate the theoretical yield by using the stoichiometric relationship between the limiting reactant and the desired product, based on their balanced chemical equation.

4. Measure the actual yield of the product obtained from the experiment.

5. Calculate the percent yield using the formula: (Actual yield / Theoretical yield) × 100%.

This process will provide the chemist with a measure of the efficiency of the chemical reaction.

Complete question : A chemist interested in the efficiency of a chemical reaction would calculate the percent yield ?

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We can use the formula for calculating heat:

Q = m × c × ΔT

where Q is the amount of heat transferred, m is the mass of the substance, c is its specific heat, and ΔT is the change in temperature.

Plugging in the given values, we get:

8250 J = m × 0.9025 J/g ·°C × 40.0 °C

Simplifying, we get:

8250 J = m × 36.1 J/g

Solving for m, we get:

m = 8250 J ÷ 36.1 J/g

m ≈ 228.26 g

Therefore, the mass of the aluminum is approximately 228.26 g.

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During the discharge of a lead-acid battery, the oxidation reaction occurs at the anode where lead (Pb) is converted into lead sulfate (PbSO4) and electrons are released:
Pb(s) → PbSO4(s) + 2e-

Meanwhile, reduction occurs at the cathode where lead dioxide (PbO2) is reduced to lead sulfate (PbSO4) by gaining those electrons released at the anode:
PbO2(s) + 4H+(aq) + 2e- → PbSO4(s) + 2H2O(l)
The balanced chemical equation shows that for every two electrons transferred at the anode, one molecule of PbSO4 is formed. Therefore, the 378 grams of Pb from the anode would produce 378/207 = 1.82 moles of PbSO4.
Since the reaction at the cathode involves the reduction of PbO2 to PbSO4, the same number of moles of PbSO4 should be formed at the cathode. The molar mass of PbO2 is 239.2 g/mol, so the mass of PbO2 that is reduced at the cathode would be:
1.82 moles x 239.2 g/mol = 435.8 g
Therefore, during the same period of discharge, 435.8 grams of PbO2 would be reduced at the cathode.

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To manipulate seven additional data sets and place these values in your Ocean Interactions, follow these steps:
Step 1: Obtain the data sets
First, acquire the seven additional data sets that you want to include in your Ocean Interactions analysis. These data sets could be related to variables such as temperature, salinity, ocean currents, or marine life distributions.

Step 2: Organize the data
Next, organize the data sets by sorting, filtering, or aggregating them as needed to make them more manageable for analysis. This process may involve cleaning the data to remove any inconsistencies or errors, as well as converting the data into a compatible format for further manipulation.

Step 3: Manipulate the data
Using various data manipulation techniques, transform the additional data sets to create new variables or features that can help provide a deeper understanding of the Ocean Interactions. This manipulation could include calculations, statistical analysis, or creating visual representations to identify patterns or trends within the data.

Step 4: Integrate the data
Combine the manipulated additional data sets with the existing Ocean Interactions data to create a comprehensive analysis. This integration process may involve merging or joining data sets based on common variables or geographical locations, ensuring that the resulting data accurately reflects the interactions between various ocean-related factors.

Step 5: Analyze the data
With the additional data sets now integrated into your Ocean Interactions analysis, examine the relationships between the different variables to gain insights into the complex dynamics at play. This analysis could involve statistical tests, correlations, or predictive modeling techniques to better understand the underlying patterns and trends in the data.

Step 6: Interpret the results
Based on the analysis, draw conclusions about the role of the additional data sets in the overall Ocean Interactions. This interpretation should consider the potential implications of these findings for the broader understanding of ocean processes and the management of marine ecosystems.

By following these steps, you will successfully manipulate seven additional data sets and place these values in your Ocean Interactions analysis, enhancing your understanding of the complex dynamics involved in the marine environment.

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Manganese(IV) permanganate is a chemical compound with the formula [tex]MnO4[/tex]. It is an ionic compound that consists of one manganese atom and four oxygen atoms.

The oxidation state of manganese in the compound is +7, which means that it has lost seven electrons and has seven fewer electrons than the neutral atom. The oxidation state of oxygen in the compound is -2, which means that each oxygen atom has gained two electrons.

To calculate the number of moles of oxygen in one mole of manganese(IV) permanganate, we can use the molecular formula of the compound, which tells us that there are four oxygen atoms per one manganese atom. Therefore, the molar ratio of oxygen to manganese is 4:1.

So, one mole of manganese(IV) permanganate contains four moles of oxygen. This can be written as:

1 mole [tex]MnO4[/tex] = 4 moles O2

This means that if we have one mole of manganese(IV) permanganate, we would have four moles of oxygen atoms.

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The pyramid shape is a good way to model the relative amount of energy in different groups of organisms in a food chain because it reflects the energy transfer from one trophic level to another.

In a food chain, energy is transferred from one organism to another through the consumption of food. As each organism consumes the one below it, a large proportion of the energy that was stored in the previous organism is lost as heat or used for metabolic processes such as respiration. This means that there is less energy available for the next organism in the chain.

The pyramid shape reflects this decrease in available energy at each trophic level. The base of the pyramid represents the primary producers, which have the largest amount of energy available to them through photosynthesis. As we move up the pyramid to the next trophic level, the available energy decreases, representing the loss of energy as we move up the food chain.

By using a pyramid shape to model the relative amount of energy in different groups of organisms in a food chain, we can see the significant decrease in available energy at each successive trophic level. This shape helps to illustrate the importance of primary producers in supporting life on Earth and the delicate balance of energy transfer that exists in ecosystems.

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It is False to state that an Absolute brightness scale is called apparent magnitude.

The brightness of a star as seen from Earth is described by apparent magnitude.  It is determined by the size of the star and its distance from Earth.  On a scale of (-26.8 to +29), Negative values are low in bright stars. The Sun (apparent magnitude -26.8) is the brightest star in the sky.

The absolute magnitude scale is the same as the apparent magnitude scale, with a difference in brightness of 1 magnitude = 2.512 times. This logarithmic scale is likewise unitless and open-ended. Again, the brighter the star, the lower or more negative the value of M.

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Full Question:

An Absolute brightness scale is called apparent magnitude.
True or False?

The correct answer is therefore A, -1.66 V.

The given information includes the standard reduction potential of the half-reaction:

Ag(aq) + e- → Ag(s) E° = +0.80 V

We can use this information along with the standard cell potential equation to find the standard reduction potential of the half-reaction:

E°cell = E°reduction + E°oxidation

where E°cell is the standard cell potential, E°reduction is the reduction potential for the half-reaction being reduced, and E°oxidation is the oxidation potential for the half-reaction being oxidized.

In this case, the two half-reactions involved are:

M3+(aq) + 3e- → M(s) (reduction)

3Ag(aq) → 3Ag+(aq) + 3e- (oxidation)

The reduction half-reaction needs to be flipped and its potential sign changed to obtain the oxidation potential:

M(s) → M3+(aq) + 3e- (oxidation)

The standard cell potential is the difference between the reduction and oxidation potentials:

E°cell = E°reduction + E°oxidation

E°cell = E°(M3+(aq) + 3e- → M(s)) + E°(M(s) → M3+(aq) + 3e-)

E°cell = E°(M(s) → M3+(aq) + 3e-) + (-E°(3Ag(aq) → 3Ag+(aq) + 3e-))

E°cell = E°(M(s) → M3+(aq) + 3e-) - E°(Ag(aq) → Ag(s))

E°cell = E°(M3+(aq) + 3e- → M(s)) - E°(Ag(aq) → Ag(s))

E°cell = -2.46 V - 0.80 V = -3.26 V

Therefore, the standard reduction potential for the half-reaction M3+(aq) + 3e- → M(s) is:

E°(M3+(aq) + 3e- → M(s)) = E°cell + E°(Ag(aq) → Ag(s))

E°(M3+(aq) + 3e- → M(s)) = -3.26 V + 0.80 V = -2.46 V

The correct answer is therefore A, -1.66 V.

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Here, each of the elements below with the class to which it belongs.  

Lithium → Alkali metals

Uranium → Transition metals

What is an Alkali metals?

Alkali metals are a group of highly reactive chemical elements in the periodic table. These elements include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). Alkali metals have a single electron in their outermost shell, which makes them highly reactive and able to easily lose that electron to form a positive ion. They are typically soft, silvery-white metals that have low melting and boiling points, and are highly reactive with water and other substances. Alkali metals are important in various industrial applications, such as batteries, alloys, and chemical synthesis.

Krypton → Noble gases

Manganese → Transition metals

Fluorine → Halogens

Barium → Alkaline Earth

Most reactive metal → Alkali metals

Silicon → Metalloids

Groups 3-12 → Transition metals

Most reactive nonmetals → Halogens

Inert and unreactive → Noble gases

Has characteristics of metals and nonmetals → Metalloids

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To determine the empirical formula of the compound, we need to first find the moles of each element present in the compound:

moles of Al = 94.5 g / 26.98 g/mol = 3.50 mol

moles of F = 199.5 g / 18.99 g/mol = 10.50 mol

Next, we need to find the ratio of the moles of each element in the compound by dividing by the smallest number of moles. In this case, the smallest number of moles is 3.50 mol:

moles of Al = 3.50 mol / 3.50 mol = 1

moles of F = 10.50 mol / 3.50 mol = 3

The empirical formula of the compound is therefore AlF3.

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To solve this problem, we can use the formula:

q = m*c*ΔT, where q is the amount of heat energy absorbed by the gold, m is the mass of the gold, c is the specific heat capacity of gold, and ΔT is the change in temperature of the gold.

We are given the mass of gold (m = 4.1 g), the specific heat capacity of gold (c = 0.130 J/g °C), and the amount of energy used to heat the gold (q = 52.2 J). We are asked to find the final temperature of the gold (ΔT).

Rearranging the formula, we get:
ΔT = q/(m*c)
Substituting the values we know, we get:
ΔT = 52.2 J / (4.1 g * 0.130 J/g °C)
ΔT = 98.92 °C
This is the change in temperature of the gold. To find the final temperature, we add this to the original temperature of 25.0°C:
Final temperature = 25.0°C + 98.92°C
Final temperature = 123.92°C
Therefore, the final temperature of the gold is 123.1°C.

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The percent composition of the sample containing 1.29 grams of carbon and 1.71 grams of oxygen is 43% carbon and 57% oxygen.

The percent composition of a sample can be calculated by dividing the mass of each element in the sample by the total mass of the sample and then multiplying by 100%.

To find the percent composition of a sample containing 1.29 grams of carbon and 1.71 grams of oxygen, we need to calculate the total mass of the sample first.

Total mass of the sample = mass of carbon + mass of oxygen
= 1.29 grams + 1.71 grams
= 3 grams

Now, we can calculate the percent composition of carbon and oxygen in the sample:

Percent composition of oxygen = (mass of oxygen / total mass of the sample) x 100%
= (1.71 grams / 3 grams) x 100%
= 57%

Percent composition of carbon =  (mass of carbon / total mass of the sample) x 100%

=(1.29 grams / 3 grams) x 100%

= 43%

Therefore, the sample contains 43% carbon and 57% oxygen by mass.

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When hydrogen and steam are both present in a gas at the same pressure and temperature, this is the ideal gas condition. This is so because according to the ideal gas law, an ideal gas's pressure, volume, and temperature are all precisely proportional to one another.

This indicates that when the two gases have the same temperature and pressure, the two gases will also have the same volume. As a result, the gases are in their ideal state, having the same volume and pressure but retaining their distinct chemical compositions.

This is perfect because it enables the two gases to interact with one another in a predictable way, allowing for the measurement and prediction of the gases' behaviour.

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A 35. 3 g of element M is reacted with nitrogen to produce 43. 5 g of compo und M₃N₂ (i) The molar mass of element M is 24.0 g/mol. (ii) The name of the element is magnesium (Mg).

(i) To find the molar mass of element M, we need to use stoichiometry to relate the mass of M to the mass of M₃N₂. We can start by calculating the moles of M3N2 produced:

43.5 g M₃N₂ × 1 mol M₃N₂/100.9 g M₃N₂ = 0.43 mol M₃N₂

Since the molar ratio between M and M₃N₂ is 1:3, we can calculate the moles of M:

0.43 mol M₃N₂ × 1 mol M/3 mol M₃N₂ = 0.14 mol M

Finally, we can calculate the molar mass of M by dividing its mass (35.3 g) by the number of moles (0.14 mol):

molar mass of M = 35.3 g/0.14 mol = 253 g/mol

However, this value is much higher than the molar mass of any known element. We can recognize that the formula M₃N₂ implies that element M is a metal with a +2 charge, since each M atom forms 3 bonds with N atoms, and each N atom forms 2 bonds with M atoms.

(ii) Based on this information, we can identify element M as magnesium (Mg), which has a molar mass of 24.0 g/mol.

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Starting with 29.25 g of NaOH and 107 g of FeCl₃, the limiting reactant is NaOH with yeild percentage of 60%.

To find the reaction yield and the limiting reactant, starting with 29.25 g of NaOH and 107 g of FeCl₃, you need to perform the following steps:

1. Write the balanced chemical equation:
FeCl₃ + 3NaOH → Fe(OH)₃ + 3NaCl

2. Calculate moles of each reactant:
NaOH: 29.25 g / (23.0 g/mol Na + 15.99 g/mol O + 1.01 g/mol H) ≈ 0.729 moles
FeCl₃: 107 g / (55.85 g/mol Fe + 3 * 35.45 g/mol Cl) ≈ 0.397 moles

3. Identify the limiting reactant:
For every mole of FeCl₃, you need 3 moles of NaOH. Divide moles of each reactant by their coefficients in the balanced equation:
NaOH: 0.729 moles / 3 ≈ 0.243
FeCl₃: 0.397 moles / 1 ≈ 0.397

The smaller value is for NaOH, so it is the limiting reactant.

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