1. Which metal is the most reactive? How do you know this?
2. Rank the metals in order of increasing reactivity.
3. Give the chemical equations for each single replacement reaction that took place.
4. Was Fe^3+ reduced? Of so what metal(s) acted as reducing agents?

A sunscreen made with Benzophenone-5 ([tex]C_1_4H_1_1NaO_6S[/tex]) would be expected to be more waterproof than benzophenone-3 ([tex]C_1_4H_1_2O_3[/tex]).

This is due to the presence of a sodium salt group (Na) and a sulfonic acid group ([tex]SO_3H[/tex] ) in benzophenone-5, which makes it more polar than benzophenone-3. Polar molecules interact more strongly with water molecules and are less likely to dissolve in nonpolar solvents such as oils.

Because sunscreen is designed to be water-resistant, the more polar benzophenone-5 should have stronger interactions with water and give more water resistance than benzophenone-3.

Moreover, the sulfonic acid group in benzophenone-5 may allow it to make stronger hydrogen bonds with water, increasing its water resistance even further.

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First, we need to write out the balanced chemical equation for the reaction: 4 KO2 + 2 CO2 → 2 K2CO3 + 3 O2

From the equation, we can see that 4 moles of KO2 react with 2 moles of CO2 to produce 3 moles of O2. Therefore, we need to convert the given masses of KO2 and CO2 into moles:

moles of KO2 = 2.61 g / molar mass of KO2 = 2.61 g / 71.10 g/mol = 0.0367 mol
moles of CO2 = 4.46 g / molar mass of CO2 = 4.46 g / 44.01 g/mol = 0.1013 mol

Next, we need to determine the limiting reagent (the reactant that will be completely consumed in the reaction) by comparing the mole ratios of KO2 and CO2 in the balanced equation. The ratio of moles of KO2 to moles of CO2 is:
0.0367 mol KO2 / 4 mol KO2 per 2 mol CO2 = 0.0184 mol CO2

Since this ratio is less than the actual number of moles of CO2 we have (0.1013 mol), CO2 is in excess and KO2 is the limiting reagent.

Using the mole ratio from the balanced equation, we can calculate the number of moles of O2 produced:

moles of O2 = 3 mol O2 per 4 mol KO2 × 0.0367 mol KO2 = 0.0275 mol O2

Finally, we can convert the moles of O2 to grams:

mass of O2 = moles of O2 × molar mass of O2 = 0.0275 mol × 32.00 g/mol = 0.88 g
Therefore, 2.61 g of KO2 and 4.46 g of CO2 would produce 0.88 g of O2.

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The molar equilibrium concentration of Cu² ⁺ is [tex]3.3 x 10^-26[/tex]M when 0.100 mol NH₃ is added to 1.00 L of 0.800 M with Kf = [tex]2.1 x 10^13[/tex].

The issue includes computing the molar balance convergence of Cu² ⁺ in an answer that has 0.100 mol NH3 added to 1.00 L of 0.800 M [Cu(NH₃)₄]²⁺ . To tackle the issue, we can involve the balance consistent articulation for the arrangement of[Cu(NH₃)₄]²⁺:

Kf =[Cu(NH₃)₄]²⁺/(Cu² ⁺)(NH₃)₄

Since the volume of the arrangement doesn't change when NH₃ is added, the underlying grouping of [Cu(NH₃)₄]²⁺ is as yet 0.800 M, while the underlying convergences of Cu² ⁺ and NH₃ are zero. Let x be the molar centralization of Cu² ⁺ at balance, and (0.100 - 4x) be the molar grouping of NH₃ at harmony. Then, we can compose the harmony consistent articulation as:

[tex]2.1 x 10^13 = (x)(0.800 - x)^4/(0.100 - 4x)^4[/tex]

Settling for x gives the molar balance convergence of Cu² ⁺ as 3.3 x [tex]10^-26[/tex] M. This tiny focus demonstrates that the majority of the copper in the arrangement is as [Cu(NH₃)₄]²⁺ and that the expansion of NH₃ has moved the harmony towards the development of this complex.

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The mole fractions of each species at equilibrium are 0.25 for A and D, 0.5 for B, and 0.225 for C.

we can use the principles of chemical equilibrium and the mole fraction formula.

First, we need to write the balanced chemical equation for the reaction involving A, B, C, and D. Let's assume that the reaction is:

A + 2B <=> C + D

where A, B, C, and D are the chemical species, and the coefficients indicate their stoichiometric ratios.

Next, we need to write the expression for the equilibrium constant, Kc, for this reaction:

Kc = [C][D] / [A][B]²

where [X] denotes the molar concentration of species X at equilibrium.

Since we know the initial moles of A, B, and D, we can calculate their total moles in the mixture:

Total moles = 1 mol A + 2 mol B + 1 mol D = 4 mol

We also know that the final mixture contains 0.9 mol of C. Therefore, the molar concentration of C at equilibrium is:

[C] = 0.9 mol / 4 L = 0.225 M

Since we have only one unknown, we can use the equilibrium constant expression to calculate the molar concentration of D:

Kc = [C][D] / [A][B]²

0.9 = (0.225)(D) / (1)(2²)

D = 1.8

Therefore, the molar concentration of D at equilibrium is 1.8 M.

Using the law of conservation of mass, we can also calculate the molar concentration of A and B at equilibrium:

[A] = 1 mol / 4 L = 0.25 M

[B] = 2 mol / 4 L = 0.5 M

Mole fraction of X = moles of X / total moles

Mole fraction of A = 1 mol / 4 mol = 0.25

Mole fraction of B = 2 mol / 4 mol = 0.5

Mole fraction of C = 0.9 mol / 4 mol = 0.225

Mole fraction of D = 1 mol / 4 mol = 0.25

Therefore, the mole fractions of each species at equilibrium are 0.25 for A and D, 0.5 for B, and 0.225 for C.

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Answer:

true

Explanation:

Answer:

0.0104 moles of gas in the flask.

Explanation:

To calculate the number of moles of gas in the flask, you can use the ideal gas law equation: PV = nRT. Where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant and T is temperature.

First, you need to convert the pressure from mmHg to atm and the temperature from Celsius to Kelvin. The pressure in atm is 760.0 mmHg / 760 mmHg/atm = 1 atm. The temperature in Kelvin is 17.00°C + 273.15 = 290.15 K.

Next, you need to convert the volume from mL to L. The volume in L is 250.0 mL / 1000 mL/L = 0.2500 L.

Now you can plug all the values into the ideal gas law equation and solve for n: (1 atm)(0.2500 L) = n(0.08206 L·atm/mol·K)(290.15 K). Solving for n gives n = 0.0104 mol.

So there are approximately 0.0104 moles of gas in the flask.

Explanation:

Table H lists vapor pressure data for pure water at various temperatures. We can use this data to estimate the vapor pressure of the water in the given system at its final temperature of 80.0°C.

First, we need to calculate the heat absorbed by the water sample during the heating process. We can use the specific heat capacity of water to do this:

q = m * c * ΔT

where q is the heat absorbed, m is the mass of water (100 g), c is the specific heat capacity of water, and ΔT is the temperature change (80°C - 30°C = 50°C).

Plugging in the values, we get:

q = 100 g * 4.18 J/(g*C) * 50 C

q = 20900 J

This tells us that 20,900 joules of energy were absorbed by the water sample during heating.

Next, we need to consider the saturated solution of KCIO3 in the water sample. At 80.0°C, the water is already close to boiling, so it is likely that the vapor pressure of the water in the system is close to the vapor pressure of pure water at this temperature. From Table H, we can see that the vapor pressure of pure water is approximately 356 mmHg at 80.0°C.

Therefore, the vapor pressure of the water in the given system at its final temperature of 80.0°C is approximately 356 mmHg.

Answer:

Explanation:

In the given reaction, carbon has a greater oxidation number in carbon dioxide (CO₂) than in carbon monoxide (CO). In CO₂, the oxidation number of carbon is +4, while in CO it is +2.

The molarity of the solution that has 2.0 moles of solute in 3.0 L of solution is 0.67 mol/L

Molarity is  described as a measure of the concentration of a chemical species, in particular of a solute in a solution, in terms of amount of substance per unit volume of solution.

Molarity = moles of solute / liters of solution

we then substitute the given values, and have

Molarity = 2.0 moles / 3.0 L

Molarity = 0.67 mol/L

Molarity is  very important because the ration used to express the concentration of  any  solution.

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5.221 grams of Al are required to react with 352 mL of 1.65 M HCl solution.

Molarity (M) is defined as the moles of solute per liter of the solution.

Balanced chemical equation is : 2Al + 6HCl → 2AlCl₃ + 3H₂

From the equation, we can see that 2 moles of Al react with 6 moles of HCl to produce 2 moles of AlCl₃ and 3 moles of H₂.

As moles of HCl = Molarity × Volume

moles of HCl = 1.65 mol/L × 0.352 L

moles of HCl = 0.58128 mol

and moles of Al = (2/6) × moles of HCl

moles of Al = (1/3) × 0.58128 mol

moles of Al = 0.19376 mol

mass of Al = moles of Al × molar mass of Al

mass of Al = 0.19376 mol × 26.98 g/mol

mass of Al = 5.221 g

So, 5.221 grams of Al are required to react with 352 mL of 1.65 M HCl solution.

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The mass of the silver block, given that it was initially at 55.1 °C  and is submerged into 100.0 g of water at 25.0°C is 189.8 g

We'll begin our calculation by obtaining the heat absorbed by the water. Details below:

Q = MCΔT

Q = 100 × 4.184 × 2.9

Q = 1213.36 J

Finally, we shall determine the mass of the silver block. Details below:

Q = MCΔT

-1213.36 = M × 0.235 × -27.2

-1213.36 = M × -6.392

Divide both sides by -6.392

M = -1213.36 / -6.392

M = 189.8 g

Thus, we can conclude that the mass of the silver block is 189.8 g

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Complete question:

A silver block, initially at 55.1∘C, is submerged into 100.0 g of water at 25.0∘C in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.9∘C. The specific heat capacities for water and silver are Cs,water = 4.18J/(g⋅∘C) and Cs, silver = 0.235J/(g⋅∘C). What is the mass of the silver block?

The volume of O2 that can be released at STP from the given sample of silver oxide is 23.45 mL.

Creating the balanced chemical equation for the breakdown of silver oxide is the first step in tackling this issue:

2Ag2O(s) → 4Ag(s) + O2(g)

We can deduce from the equation that 2 moles of AgO will result in 1 mole of O2. Since Ag2O has a molar mass of 231.735 g/mol, 0.4856 g of Ag2O is equivalent to:

0.4856 g Ag2O x (1 mol Ag2O/231.735 g Ag2O) = 0.002095 mol Ag2O

Therefore, the number of moles of O2 that can be produced from 0.4856 g of Ag2O is:

0.002095 mol Ag2O x (1 mol O2/2 mol Ag2O) = 0.0010475 mol O2

1 mole of any gas takes up 22.4 L of space at STP As a result, 0.4856 g of Ag2O can generate the following amount of O2 at STP:

0.0010475 mol O2 x 22.4 L/mol = 0.02345 L or 23.45 mL

Therefore, the volume of O2 that can be released at STP from the given sample of silver oxide is 23.45 mL.

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Answer:

3.566 mol

Explanation:

Since 60.05 is grams divided by mol to cancel out the grams to get only mols it must be divided by 16.84 g

[tex]\frac{60.05 g}{mol} *\frac{1 }{16.84g} =3.566[/tex] mols acetic acid

The equation that shows that the total mass during a chemical reaction stays the same is 2) H₂ + O₂ → H₂O.

This is an example of a balanced chemical equation where the number of atoms of each element on both the reactant and product side is equal. In other words, the total number of atoms of each element is conserved, and therefore the total mass is conserved. In the other reactions, either the number of atoms on the product side is different from the reactant side or there is no reaction at all.

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We can use the combined gas law to determine the volume of the balloon at a higher altitude. The combined gas law relates the pressure, volume, and temperature of a gas:

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

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

We are given the initial pressure (P1 = 761 mmHg), volume (V1 = 56.0 L), and temperature (T1 = 23.1 °C = 296.25 K) of the gas, and the final pressure (P2 = 0.0772 atm), and temperature (T2 = -6.97 °C = 266.18 K) of the gas. We can solve for V2, the final volume of the gas:

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

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

V2 = (761 mmHg x 56.0 L x 266.18 K) / (0.0772 atm x 296.25 K)

V2 = 2,040 L (rounded to three significant figures)

Therefore, the volume of the weather balloon at the higher altitude is approximately 2,040 L.

The pressure of a gas that occupies 50.5L at 69.0°C is 6.95 atm.

The pressure of an ideal gas can be calculated using Avogadro's equation as follows;

PV = nRT

Where;

According to this question, 12.5 mol of an ideal gas occupies 50.5 L at 69.00°C. The pressure can be calculated as follows:

P × 50.5 = 12.5 × 0.0821 × 342

50.5P = 350.9775

P = 6.95 atm

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Answer:

Explanation:

[tex]\frac{918.7 g}{1} *\frac{1}{216.59m } = 4.241 mol[/tex] To start off the mol of HgO must be found.

After that the molar ratio between HgO and O must be found but in this case its 1:1

[tex]4.241 mol HgO*\frac{1 molO}{1molHgO} = 4.241 mol O[/tex] the mols of HgO is put on the bottom to cancel out  with the other one leaving just mols of oxygen. Finally to find g of oxygen it must be multiplied by its molar mass.

[tex]\frac{4.241 molO}{1} * \frac{15.999 g}{mol} = 67.85 g[/tex] Oxygen

Answer: 0.24 Moles. WARNING: "mm" in the original question seems to be a typo and was assumed to be "M" (moles per liter) for concentration.

Explanation:

To calculate the number of moles of solute needed to prepare a solution, we can use the formula:

moles of solute = concentration (in moles per liter) * volume of solution (in liters)

Given:

Concentration of NaCl solution = 0.8 M (moles per liter)

Volume of solution to be prepared = 300 mL = 300/1000 L (converted to liters)

Plugging in the given values:

Concentration = 0.8 M

Volume of solution = 300/1000 L

moles of NaCl = 0.8 M * 300/1000 L

Calculating:

moles of NaCl = 0.24 moles

So, 0.24 moles of NaCl are needed to prepare 300 mL of a 0.8 M NaCl solution.

The equation that represents a balanced reaction involving 14 atoms of oxygen is:

2C2H6 + 7O2 --> 4CO2 + 6H2O

a. The relationship between variables in this equation is that 2 moles of C2H6 (ethane) react with 7 moles of O2 (oxygen) to produce 4 moles of CO2 (carbon dioxide) and 6 moles of H2O (water). This equation follows the law of conservation of mass, where the total number of atoms on both sides of the equation is the same, indicating a balanced reaction.

b. The graph is linear, as the coefficients of the reactants and products in the equation are whole numbers and form a consistent ratio. The coefficients of 2, 7, 4, and 6 represent the stoichiometry of the reaction, indicating a fixed relationship between the reactants and products.

c. An example of a situation where this balanced equation could be applicable is the combustion of ethane (C2H6) in the presence of excess oxygen (O2) to produce carbon dioxide (CO2) and water (H2O), which is a common reaction in the combustion of hydrocarbon fuels. The equation represents the balanced stoichiometry of this reaction, where 2 moles of ethane react with 7 moles of oxygen to produce 4 moles of carbon dioxide and 6 moles of water, involving a total of 14 atoms of oxygen in the reaction.

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A 6.50-g sample of copper metal at 25.0 °C is heated by the addition of 145 J of energy. The final temperature of the copper is 83.7 °C. The specific heat capacity of copper is 0.38 J/g-K.

The correct answer choice is "83.7"

To solve this problem, we can use the equation:

q = mcΔT

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

Rearranging this equation to solve for ΔT, we get:

ΔT = q / (mc)

Substituting the given values, we get:

ΔT = 145 J / (6.50 g x 0.38 J/g-K)

ΔT = 58.7 K

Therefore, the final temperature of the copper is:

25.0 °C + 58.7 °C = 83.7 °C

So the correct option is 83.7.

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273.8 grams of zinc (Zn) are needed to produce 8.45 grams of hydrogen gas [tex](H_2).[/tex]

In this chemical reaction, zinc (Zn) reacts with sulfuric acid [tex](H_2SO_4)[/tex] to produce zinc sulfate  [tex](ZnSO_4)[/tex] and hydrogen gas [tex](H_2).[/tex]

From the balanced chemical equation, we can see that 1 mole of zinc (Zn) reacts with 1 mole of sulfuric acid [tex](H_2SO_4)[/tex] to produce 1 mole of hydrogen gas [tex](H_2).[/tex]

Hydrogen gas  has a molar mass of 2.016 g/mol.

Therefore, 8.45 grams of hydrogen gas is equal to 8.45 g / 2.016 g/mol = 4.19 moles of [tex]H_2[/tex].

Since 1 mole of Zn reacts with 1 mole of [tex]H_2[/tex] , we need 4.19 moles of Zn to produce 4.19 moles of [tex]H_2[/tex].

molar mass of Zinc = 65.38 g/mol.

Therefore, 4.19 moles of Zn has a mass of 4.19 moles x 65.38 g/mol = 273.8 grams.

Therefore, you would need 273.8 grams of zinc (Zn) to produce 8.45 grams of hydrogen gas [tex](H_2).[/tex]

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Answer:its b

Explanation:

jusut bcss

The product that is formed first is product B and the product that will be the major product if given enough time would also be product B.

In an energy diagram, the vertical axis represents the overall energy of the reactants, while the horizontal axis is the ‘reaction coordinate’, tracing from left to right the progress of the reaction from starting compounds to final products.

The activation energy of the reaction can be shown on a diagram as the energy between the reactants that the transition state.

The product with lesser activation energy is the product that is formed first and the major product is decided by the stability of the product which depends on the energy. Lesser is the energy of the product, greater is its stability.

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The rate constant, k = 5.27 E-2 s⁻¹, determines the rate law for the reaction P → E + Z.

The rate of the reaction P → E + Z can be expressed as:

Rate = - d[P]/dt = d[E]/dt = d[Z]/dt

where d[P], d[E], and d[Z] = changes in the concentrations of P, E, and Z, respectively, over a small time interval dt.

Use the experimental data to determine the rate constant and the order of the reaction.

Calculate the initial rate of the reaction in each trial by dividing the change in concentration of P by the time interval:

rate1 = (d[P]/dt)1 = (0.30 M - 0 M)/(20 s) = 0.015 M/s

rate2 = (d[P]/dt)2 = (0.60 M - 0.30 M)/(20 s) = 0.015 M/s

rate3 = (d[P]/dt)3 = (0.90 M - 0.60 M)/(20 s) = 0.015 M/s

The initial rates are the same in all three trials, which suggests that the reaction is first-order with respect to P.

Now using any of the three trials to determine the value of the rate constant k, trial 1:

Rate1 = k[P]1

k = Rate1/[P]1 = (1.58 E-2 M/s)/(0.30 M) = 5.27 E-2 s⁻¹

Therefore, the rate law for the reaction P → E + Z is:

Rate = k[P]

where k = 5.27 E-2 s⁻¹ is the rate constant.

Use the rate law to calculate the expected rates of the reaction at different concentrations of P. For example:

Rate2 = k[P]2 = (5.27 E-2 s⁻¹)(0.60 M) = 3.16 E-2 M/s

Rate3 = k[P]3 = (5.27 E-2 s⁻¹)(0.90 M) = 4.74 E-2 M/s

These expected rates are close to the experimental rates, which suggests that the rate law is a good approximation for the reaction under these conditions.

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The oxidation number of the unknown chlorine in the compound is + 5

The oxidation number of an element in a compound is determined by a set of rules based on its position in the periodic table, as well as the charges of other atoms in the compound

We know that the oxidation number of the chlorine which we want to obtain would be designated as x and the total of the oxidation numbers of the elements in the compound is zero.

Thus we have that;

1 + x + 3(-2) = 0

1 + x - 6 = 0

-5 + x = 0

x = 5

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The reaction rates for trial 1 is 8.22 x 10⁻² M⁻² s⁻¹ and 1.10 M⁻² s⁻¹ for trail 2 and 3

Keep the concentration of W constant while varying the concentrations of U and S while measuring the reaction rate in order to determine the reaction rate with regard to U and S.

Select trial 1 as the reference trial and calculate the reaction's rate constant (k) with respect to U and S, assuming that the concentration of W is constant throughout all three trials.

For trial 1:

[W] = 0.13 M

Rate = 4.72 x 10⁻⁴ M/s

For trial 2:

[W] = 0.13 M

Rate = 1.18 x 10⁻² M/s

From the equation rate = k[U][S], set up the following ratio of rates:

Rate2/Rate1 = (k[U]2[S]2)/(k[U]1[S]1)

Simplifying:

k = (Rate2/Rate1) x (1/[U]2) x (1/[S]2) x ([U]1) x ([S]1)

Substituting the values from trials 1 and 2:

k = (1.18 x 10⁻² M/s) / (4.72 x 10⁻⁴ M/s) x (1/0.65 M) x (1/1 M) x (0.13 M) x (1 M)

k = 8.22 x 10⁻²M⁻² s⁻¹

Similarly, for trial 3:

[W] = 0.13 M

Rate = 2.95 x 10⁻¹ M/s

Again, using trial 1 as the reference trial, figure out the reaction's rate constant (k) in relation to U and S:

k = (Rate3/Rate1) x (1/[U]3) x (1/[S]3) x ([U]1) x ([S]1)

k = (2.95 x 10⁻¹ M/s) / (4.72 x 10⁻⁴ M/s) x (1/3.25 M) x (1/1 M) x (0.13 M) x (1 M)

k = 1.10 M⁻² s⁻¹

Therefore, the equation states the reaction rate in relation to U and S is k = 8.22 x 10⁻² M⁻² s⁻¹ and 1.10 M⁻² s⁻¹ for trials 2 and 3, respectively.

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A silver bar with the mass of the 300 grams is heated from the 30 °C to 55 °C. The amount heat does the silver bar absorb in the joules is 1762.5 J.

The mass of the silver bar = 300 g

The initial temperature = 30 °C

The final temperature = 55 °C

The heat energy is expressed as :

Q = mc ΔT

Where,

The m is mass of the silver bar = 300 g

The c is the specific heat capacity = 0.235 J/g °C

The ΔT is the change in the temperature = final temperature - initial temperature

The ΔT is the change in the temperature = 55 °C - 30 °C

The ΔT is the change in the temperature = 25 °C

The heat energy, Q = 300 × 0.235 × 25

The heat energy, Q = 1762.5 J

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If a skimmer and a gull eat the same fish and the skimmer is more successful at catching the fish over time, it is likely that the skimmer population would increase, while the gull population may decrease.

The skimmer's success in catching the fish would give it an advantage in obtaining the necessary nutrients for survival and reproduction. As a result, the skimmer population would likely grow over time as more individuals are able to survive and reproduce due to the abundance of food.

On the other hand, the gull population may decrease due to the competition with the skimmer for the same food source. If the skimmer population grows significantly, it may lead to a reduction in the availability of fish for the gulls to feed on. Over time, this could result in a decline in the gull population due to reduced food availability.

However, it is important to note that the impact on the bird populations may depend on various factors such as the size of the populations, availability of other food sources, and environmental factors. Therefore, the outcome of this scenario cannot be predicted with certainty and would require further analysis and investigation.

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The mass (in grams) of aluminum, Al that must react with iodine to form AlI₃, given that -836.0 KJ of heat is relaesd is 149.0 g

The mass of aluminum required to react with iodine to produce AlI₃ can be obtain as shown below:

2Al(s) + 3I₂(s) → 2AlI₃(s) ∆H = -302.9 KJ

From the balanced equation above,

When -302.9 KJ of heat energy is released, 54 g of aluminum, Al reacted.

Therefore,

When -836.0 KJ of heat energy will be release = (-836.0KJ × 54 g) / -302.9 KJ = 149.0 g of aluminum, Al will react.

Thus, from the above calculation, we can conclude that the mass of aluminum, Al required is 149.0 g

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