Consider the reaction below.

2NH3(e) N218) + 3H218)

What is the most likely effect to the forward reaction if there is an increase in pressure on this reaction?


The reactant surface area increases

The reaction rate decreases.

The reaction is not affected at all.

The reaction stops completely

Answer:

n₁ = 1.0× 10⁻⁴ mol

Explanation:

Given data:

Initial volume of balloon = 230 mL

Initial number of moles of He =?

Final number of moles of He = 3.8 × 10⁻⁴ mol

Final volume of balloon = 860 mL

Solution:

The given problem will be solve through Avogadro law,

"Number of moles of gas and volume are directly proportional to each other at constant temperature and constant pressure"

Mathematical relationship:

V₁/n₁ = V₂/n₂

No we will put the values.

230 mL  /n₁   = 860 mL/ 3.8 × 10⁻⁴ mol

n₁ = 230 mL× 3.8 × 10⁻⁴ mol/ 860 mL

n₁ = 874 × 10⁻⁴ mol. mL / 860 mL

n₁ = 1.0× 10⁻⁴ mol

Answer: the answer is n1=n2v1/v2

Explanation:

hope this helped

Answer:

An Ionic Bond

Explanation:

Salt compounds are formed by the "donating" of electrons.

Answer:

NaCl, or Salt, is an ionic bond.

Explanation:

Ionic bonds are formed from one metal and one nonmetal, Sodium being the metal and Chlorine being the nonmetal.

Explanation:

Because molarity is classified as moles of solute per liter of water, dilution of the water may result in a reduction of its concentration.

Therefore, because the amount of moles of solute has to be constant for dilution, you will use the molarity and volume of that same target solution to calculate how many moles of solute will be present in the sample of the stock solution that you dilute.

c  =   [tex]\frac{n}{v}[/tex]

⇒  n = c ⋅  V

[tex]n_{HCL}[/tex] =  0.250 M  ⋅  6.00 L  = 1.5 moles HCl

Now all you have to do is figure out what volume of   6.0 M  stock solution will contain  1.5  moles of hydrochloric acid

c = [tex]\frac{n}{v}[/tex]

V = [tex]\frac{n}{c}[/tex]

[tex]V_{Stock}[/tex] = [tex]\frac{1.5 moles}{6.0 \frac{moles}{L} }[/tex]   = 0.25 L

Expressed in milliliters, the answer will be

[tex]V_{Stock} = 250ML[/tex] →  rounded to two sig figs

The Aztec political system most closely resembles a theocracy where religious leaders influence political decisions, making Option B the correct answer as it aligns with the role of priests in Aztec governance.

The Aztec political system was most similar to a theocratic form of government where religious leaders held significant power in the state's political structure. Comparing the options provided to the Aztec system:

Option A suggests an attempt to keep religion out of politics, which is not characteristic of the Aztec system.

Option B reflects a scenario where religious leaders create policies, aligning closely with the Aztec theocracy where priests and the emperor, who was also seen as a divine figure, had substantial influence.

Option C implies an autocratic rule by a king without advice, which is not similar to the Aztec system that had a ruling elite and a structure of nobility.

Option D discusses a gender-based voting system, which is unrelated to the theocratic nature of the Aztec political system.

Therefore, the correct answer is B, a group of priests create all policies related to religion in a country. This reflects the Aztec civilization where political decisions were often intertwined with religious beliefs and practices, and religious leaders played a central role in governance.

Answer: Strong acids disassociate more compared to weak acids. Since there are more ions, due to more disassociation, there are more ions for electrons to flow through.

Explanation:

Images would show an increase in both the dissociated ions (H+ ions and anions) and the undissociated weak acid molecules in a concentrated solution of weak acid. However, the proportion between them remains unchanged, indicating the properties of a weak acid.

In a solution of a weak acid, the acid does not fully dissociate, meaning not all of its molecules separate into hydrogen ions (H+) and anions. Instead, there is an equilibrium between the undissociated acid molecules and the ions. If the concentration of the weak acid solution was increased, the number of acid molecules, both dissociated and undissociated, would increase proportionally.

The images or visual representation of this would show an increase in both the dissociated ions (H+ ions and anions) and the undissociated weak acid molecules. However, the proportion between them would remain the same if no other factors are changed, showing the characteristics of a weak acid.

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Answer:

Gas

Explanation:

Answer:

Parallel Circuit

Explanation:

In a parallel circuit, there are multiple paths through which the current can flow, so the resistance of the overall circuit is lower than it would be if only one path was available.

0.11 moles of the gas are present in the sample of dry gas.

Explanation:

Data given:

mass of the gas  = 2.1025 grams

volume of the gas = 2.850 litres

temperature =  22 degrees (273.15+22) = 295.15 K

Pressure = 740 mm Hg or 0.973 atm

moles of the gas =?

R = 0.08206 atmL/Mole K

From the ideal gas law the number of moles can be calculated in the sample of dry gas. Number of moles will be determined by the pressure exerted, volume and temperature of the gas.

The formula:

PV = nRT

n = [tex]\frac{PV}{RT}[/tex]

putting the values in the above equation:

n = [tex]\frac{2.850 x 0.973}{0.08206 X 295.15}[/tex]

  = 0.11 moles

0.11 moles of the dry gas is present in the sample given.

When, a sample of dry gas weighing 2.1025 g is found to occupy 2.850 L at 22.0oC and 740.0 mm Hg. Then, total 0.0994 moles of gas are present.

First, we convert the temperature to Kelvin (T(K) = T(C) + 273.15) which is 22.0 + 273.15 = 295.15 K. Next, we convert pressure from mm Hg to atm by dividing by 760, as 1 atm = 760 mm Hg:

Pressure in atm = 740.0 mm Hg / 760 mm Hg/atm = 0.9737 atm.

Now we must solve for n, the number of moles of gas:

The number of moles of gas present is therefore 0.0994 moles.

Answer:

PN₂ = 191.3 Kpa

Explanation:

Given data:

Total pressure of tire = 245.0 Kpa

Partial pressure of PO₂ = 51.3 Kpa

Partial pressure of PCO₂  = 0.10 Kpa

Partial pressure of others =  2.3 Kpa

Partial pressure of PN₂ = ?

Solution:

According to Dalton law of partial pressure,

The total pressure inside container is equal to the sum of partial pressures of individual gases present in container.

Mathematical expression:

P(total) = P₁ + P₂ + P₃+ ............+Pₙ

Now we will solve this  problem by using this law.

P(total) = PO₂ + PCO₂ + P(others)+ PN₂

245 Kpa = 51.3 Kpa + 0.10 Kpa + 2.3 Kpa + PN₂

245 Kpa = 53.7 Kpa+ PN₂

PN₂ = 245 Kpa -  53.7 Kpa

PN₂ = 191.3 Kpa

The partial pressure of nitrogen is determined to be 191.3 kPa.

The total pressure in the automobile tire is given as 245.0 kPa. To find the partial pressure of nitrogen (PN₂), we can use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of all gases present.

Here's the step-by-step calculation:

Using Dalton's Law:

Ptotal = PO₂ + PCO₂ + P-others + PN₂

Substituting the given values: 245.0 kPa = 51.3 kPa + 0.10 kPa + 2.3 kPa + PN₂

Rearranging to solve for PN₂:

PN₂ = 245.0 kPa - (51.3 kPa + 0.10 kPa + 2.3 kPa)

PN₂ = 245.0 kPa - 53.7 kPa

PN₂ = 191.3 kPa

Therefore, the partial pressure of nitrogen in the car tire is 191.3 kPa.

The new volume of [tex]H_2[/tex] gas is required.

The new volume of the required gas is 1.49 L.

[tex]P_1[/tex] = Initial pressure = 1 atm

[tex]P_2[/tex] = Final pressure = 2.50 atm

[tex]T_1[/tex] = Initial temperature = 273.15 K

[tex]T_2[/tex] = Final temperature = [tex]10.00^{\circ}\text{C}=10+273.15=283.15\ \text{K}[/tex]

[tex]V_1[/tex] = Initial volume = 3.60 L

[tex]V_2[/tex] = Final volume

From the ideal gas laws we have

[tex]\dfrac{P_1V_1}{T_1}=\dfrac{P_2V_2}{T_2}\\\Rightarrow V_2=\dfrac{P_1V_1T_2}{T_1P_2}\\\Rightarrow V_2=\dfrac{1\times 3.6\times 283.15}{273.15\times 2.5}\\\Rightarrow V_2=1.49\ \text{L}[/tex]

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The new volume of H₂ gas in the balloon, taken to the sea where the pressure is 2.50 atm and the temperature is 10.00°C, is approximately 3.63 liters. This calculation is based on the ideal gas law using the initial conditions at STP.

To find the new volume of H₂ gas in the balloon when taken to the sea, we can use the ideal gas law, which relates the pressure (P), volume (V), temperature (T), and the number of moles (n) of a gas. The ideal gas law is represented as:

PV = nRT

Where:

P = Pressure (in atm)

V = Volume (in liters)

n = Number of moles

R = Universal gas constant (0.0821 L·atm/mol·K)

T = Temperature (in Kelvin)

First, let's calculate the number of moles of H₂ gas in the balloon at STP (Standard Temperature and Pressure):

Pressure at STP (P₁) = 1 atm

Temperature at STP (T₁) = 273.15 K (0°C + 273.15)

Using the ideal gas law:

P₁V₁ = nRT₁

1 atm × 3.60 L = n × 0.0821 L·atm/mol·K × 273.15 K

n ≈ 0.150 moles

Now, we can use the new conditions at the sea:

Pressure at the sea (P₂) = 2.50 atm

Temperature at the sea (T₂) = 10.00°C + 273.15 = 283.15 K

We want to find the new volume (V₂) of H₂ gas

P₂V₂ = nRT₂

Substituting the values:

(2.50 atm) × V₂ = (0.150 moles) × (0.0821 L·atm/mol·K) × (283.15 K)

Now, solve for V₂:

V₂ ≈ (0.150 moles × 0.0821 L·atm/mol·K × 283.15 K) / 2.50 atm

V₂ ≈ 3.63 L

So, the new volume of H₂ gas in the balloon when taken to the sea is approximately 3.63 liters.

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Answer:

2

Explanation:

S2x3=S6

Al2S3

S6/S3=2

Answer :

(a) The mass of [tex]Al_2O_3[/tex] produced is, 15.2 grams.

(b) The percent yield of the reaction is, 72.5 %

Explanation :

Part (a) :

Given,

Mass of [tex]Al[/tex] = 85.1 g

Molar mass of [tex]Al[/tex] = 27 g/mol

First we have to calculate the moles of [tex]Al[/tex]

[tex]\text{Moles of }Al=\frac{\text{Given mass }Al}{\text{Molar mass }Al}=\frac{85.1g}{27g/mol}=3.15mol[/tex]

Now we have to calculate the moles of [tex]Al_2O_3[/tex]

The balanced chemical equation is:

[tex]4Al+3O_2\rightarrow 2Al_2O_3[/tex]

From the reaction, we conclude that

As, 4 moles of [tex]Al[/tex] react to give 2 moles of [tex]Al_2O_3[/tex]

So, 3.15 moles of [tex]Al[/tex] react to give [tex]\frac{2}{4}\times 3.15=1.58[/tex] mole of [tex]Al_2O_3[/tex]

Now we have to calculate the mass of [tex]Al_2O_3[/tex]

[tex]\text{ Mass of }Al_2O_3=\text{ Moles of }Al_2O_3\times \text{ Molar mass of }Al_2O_3[/tex]

Molar mass of [tex]Al_2O_3[/tex] = 102 g/mole

[tex]\text{ Mass of }Al_2O_3=(1.58moles)\times (102g/mole)=161.2g[/tex]

Therefore, the mass of [tex]Al_2O_3[/tex] produced is, 161.2 grams.

Part (b) :

Now we have to calculate the percent yield of the reaction.

[tex]\text{Percent yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100[/tex]

Experimental yield = 116.9 g

Theoretical yield = 161.2 g

Now put all the given values in this formula, we get:

[tex]\text{Percent yield}=\frac{116.9g}{161.2g}\times 100=72.5\%[/tex]

Therefore, the percent yield of the reaction is, 72.5 %

Answer:

Explanation:

Fossil fuel is nonrenewable, whereas hydro, wind, solar, and wave power are generally ... depletes its fuel stock but at a relatively slow rate, and geothermal energy (Williamson, ... Future primary energy sources (e.g. nuclear, coal and solar) are primarily ... b. Distributed peak electrical generation, •. c. Distributed electricity ...

Answer: is C fossil fuel

The statement that should be rightly mentioned with respect to the   equation of thermochemical is 4 Fe (s) + 3O2(g) -------> 2Fe2O3(s)        ΔH = -3926 KJ

It is a balanced of stoichiometric chemical equation that involved the change with respect to enthalpy, ΔH. Here the reactants and the product state should be considered as the liquid, solid, or in gaseous state.

Also, the value of the heat should be absorbed since  ΔH < 0 so the reaction should be considered as the exothermic and ΔH > 0 then the reaction is endothermic.

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The correct thermochemical equation is '4Fe (s) + 3O2 (g) → 2Fe2O3 (s), ΔH = −3,926 kJ', which includes the balanced chemical equation and the enthalpy change for the whole reaction.

The question asks which statement is a correctly written thermochemical equation. A proper thermochemical equation includes the balanced chemical equation alongside the enthalpy change (ΔH) for the reaction. The enthalpy change represents the heat absorbed or released during the reaction when it occurs at constant pressure. There is only one correct thermochemical equation provided:

4Fe (s) + 3O2 (g) → 2Fe2O3 (s), ΔH = −3,926 kJ

This equation is balanced and represents the reaction of iron (Fe) with oxygen (O2) to form iron(III) oxide (Fe2O3). The enthalpy change is given for the entire reaction, not per mole, which is the correct way to represent it in a thermochemical equation. The other equations either do not include the enthalpy change in the correct units or are missing it entirely.

Answer:

601.8 mL

Explanation:

For an ideal gas kept at constant temperature and pressure, the number of moles of the gas is directly proportional to the volume of the gas:

[tex]n\propto V[/tex]

where

n is the number of moles

V is the volume of the gas

Therefore, for a gas undergoing a transformation at constant temperature and pressure, we can write:

[tex]\frac{V_1}{n_1}=\frac{V_2}{n_2}[/tex]

where here we have:

[tex]V_1=343.4 mL[/tex] is the initial volume of the gas

[tex]n_1=0.214 mol[/tex] is the initial number of moles

[tex]n_2=0.375 mol[/tex] is the final number of moles

Solving for V2, we find the final volume of the gas:

[tex]V_2=\frac{n_2 V_1}{n_1}=\frac{(0.375)(343.4)}{0.214}=601.8 mL[/tex]

The volume would 0.375 mol of argon gas occupy under the same conditions will be "601.8 mL".

According to the question,

Gas initial volume, V₁ = 343.4 mL

Initial no. of moles, n₁ = 0.214 mol

Final no. of moles, n₂ = 0.375 mol

We know that,

Moles of gas ∝ Volume of gas

or,

                   n ∝ V

and, the relation will be:

→ [tex]\frac{V_1}{n_1} = \frac{V_2}{n_2}[/tex]

then,

The final volume be:

→ V₂ = [tex]\frac{n_2 V_1}{n_1}[/tex]

By substituting the values, we get

       = [tex]\frac{0.375\times 343.4}{0.214}[/tex]

       = [tex]\frac{128.775}{0.214}[/tex]

       = 601.8 mL  

Thus the above answer is correct.

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The lens below is an example of a convex lens. Once light enters the lens, the light converges or comes together.

Convex Lens: A convex lens is thicker in the middle and thinner at the edges. It bulges outward. When light passes through a convex lens, it refracts (bends) inward toward the center of the lens.

Converges: When light converges, it means that the rays of light come together at a single point after passing through the lens. This point is called the focal point.

So, when light enters a convex lens, it bends inward and focuses at a point, which is known as convergence. This convergence is a characteristic feature of convex lenses and is utilized in various optical instruments like cameras, microscopes, and telescopes to form clear and magnified images.

Answer:

135g

Explanation:

The equation for the reaction is given below:

2H2 + O2 —> 2H2O

Next, let us calculate the mass of H2 that reacted and the mass of H2O produced from the balanced equation. This is illustrated below:

Molar Mass of H2 = 2x1 = 2g/mol

Mass of H2 from the balanced equation = 2 x 2 = 4g

Molar Mass of H2O = (2x1) + 16 = 2 + 16 = 18g/mol

Mass of H2O from the balanced equation = 2 x 18 = 36g

From the balanced equation,

4g of H2 produced 36g of H2O.

Therefore, 15g of H2 will produce = (15x36)/4 = 135g of H2O

From the calculations made above, 15g of H2 produced 135g of water (H2O)

Final answer:

15 grams of hydrogen can produce 133.80 grams of water when reacted with sufficient oxygen, following the stoichiometry of the balanced chemical equation 2H₂ + O₂ → 2H₂O.

Explanation:

The question asks how many grams of water can be produced from 15 grams of hydrogen according to the balanced chemical reaction: 2H₂(g) + O₂(g) → 2H₂O(l).

Using stoichiometry, we first determine the molar mass of hydrogen (H₂). Since there are 2 moles of hydrogen in the reaction and the molar mass of hydrogen (H) is approximately 1.01 g/mol, the molar mass of H₂ is 2.02 g/mol. This means 2 moles of H₂ weigh 4.04 g.

Therefore, 15 grams of hydrogen is equivalent to 15 g H₂ × (1 mol H₂ / 2.02 g H₂) = 7.426 moles of H₂.

According to the balanced equation, 2 moles of H₂ produce 2 moles of H₂O. So, 7.426 moles of H₂ would produce 7.426 moles of H₂O.

As the molar mass of H₂O is 18.02 g/mol, 7.426 moles of H₂O would weigh:

7.426 moles × 18.02 g/mol = 133.80 g of H₂O.

Thus, 15 grams of hydrogen can produce 133.80 grams of water, assuming there's sufficient oxygen available to react completely with the hydrogen.

Answer:

When a rock gets hot it expands a little, and when it gets cold the rock contracts a little. If a rock is heated and cooled many times, cracks form and pieces of rock fall away. This type of physical weathering happens a lot in deserts, because it is very hot during the day but very cold at night.

Explanation:

Answer:

The particles of rock are rearranged.

The sizes and shapes of the rocks are changed.

The identities and total mass of the rocks remain the same.

A physical change is a change in some of the physical properties of matter, but not its identity.

Explanation:2020

WFH 8th Gr PhySci_20-21

Answer:

all answers in image:

Explanation:

happy searching

The correct options are B, A, A, C and D.

The rate of reaction or reaction rate is the speed at which reactants are converted into products. When we talk about chemical reactions, it is a given fact that rate at which they occur varies by a great deal.

Some chemical reactions are nearly instantaneous, while others usually take some time to reach the final equilibrium.

Increasing the surface area of one or more reactants affect the reaction rate of a system will speed up the reaction.

increase the concentration of a reactant  will usually speed the reaction rate of a chemical system

Some metals found in a car’s exhaust system speed up a chemical reaction but are not used up and they act as catalysts.

A catalyst decreases the activation energy needed for a reaction.

The theory explains the increase in reaction rate caused by raising the temperature or raising the pressure of a system is collision theory.

Therefore, The correct options are B, A, A, C and D.

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Answer:

The current model of the atom and the characteristics of each of the 3 subatomic particles are the electron cloud which contains 1 subatomic particle the electron which has negative charge and weights 1/2000 AMU the electron cloud surrounds the nucleus, the nucleus contains two subatomic particles the proton which has positive charge and weights one AMU and the neutron which has neutral/no charge and weights one AMU.

The concentration of the HCl solution is 0.047 M.

Explanation:

Data given about acid and base:

volume of acid Vacid = 46.9 ml

molarity of acid =?

volume of the base (NaOH) = 16.4 ml

molarity of the base = 0.135 M

To know the concentration of the acid in this reaction, the formula used in titration  is used. It is

Macid X Vacid = Mbase X Vbase

the formula is rewritten as:

Macid = [tex]\frac{Mbase X Vbase}{Vacid}[/tex]

putting the values in the equation:

Macid = [tex]\frac{0.135 X 16.4}{46.9}[/tex]

          = 0.047 M

the concentration of the acid i.e HCl in the solution is of 0.047 M.

The number of total molecules on both sides of a balanced equation may differ. It is the number of each type of atom that must be equal, not the molecule count, to comply with the law of conservation of matter.

The number of total molecules on the left side of a balanced equation does not necessarily have to equal the number of total molecules on the right side. What must be equal are the numbers of each type of atom because chemical reactions follow the law of conservation of matter, meaning that matter is not created or destroyed in a chemical reaction. The balancing of equations ensures that there is the same number of each kind of atom on both sides of the equation, thereby obeying this fundamental law.

However, the actual molecule numbers can vary, as it's the ratio of molecules that must reflect the coefficients in the balanced equation. For instance, if we have 2 H2O (2 molecules of water) as reactants, this could lead to 2 H2 and 1 O2 (3 molecules in total) as products, with 4 hydrogen atoms and 2 oxygen atoms balanced on both sides.

Answer: 4m/s2 (B)

Explanation:

Force = mass × acceleration

Force given is 8N

Mass=2kg

Acceleration =?

Substitute into the formula

F=ma

8=2a

A=8/2

A=4m/s2

Acceleration used is 4m/s2 (B)

Answer:

b

Explanation:

Reaction of

Ca + HCl => CaCl + H2

Is a single displacement reaction.

The reaction between calcium (Ca) and hydrochloric acid (HCl) to form calcium chloride (CaCl2) and hydrogen gas (H2) is a single displacement reaction. It exemplifies a metal element reacting with an acidic compound to displace hydrogen and form a salt and hydrogen gas.

When calcium (Ca) reacts with hydrochloric acid (HCl), a single displacement reaction occurs where calcium replaces hydrogen in hydrochloric acid to form calcium chloride (CaCl2) and hydrogen gas (H2). This type of chemical reaction where an element reacts with a compound and displaces another element from it is known as a single displacement reaction or substitution reaction. In this case, the balanced reaction would be Ca + 2HCl → CaCl2 + H2.

Related Information:

The reaction of calcium carbonate (CaCO3) with hydrochloric acid to produce calcium chloride, carbon dioxide (CO2), and water (H2O) is an example of a double displacement reaction, also known as a metathesis reaction. Here, two compounds exchange ions to form two new compounds. This reaction is represented by 2 HCl(aq) + CaCO3(aq) → CaCl2(aq) + CO2(g) + H2O(l).

Answer:

4362.4 mmHg

Explanation:

Step 1:

Determination of the number of mole of H2 and the number of mole of Ar.

Molar Mass of H2 = 2x1 = 2g/mol

Mass of H2 = 1g

Number of mole of H2 =?

Number of mole = Mass/Molar Mass

Number of mole of H2 = 1/2 = 0.5 mole

Molar Mass of Ar = 40g/mol

Mass of Ar = 8g

Number of mole of Ar =?

Number of mole = Mass/Molar Mass

Number of mole of Ar = 8/40 = 0.2 mole

Step 2:

Data obtained from the question.

Volume (V) of the mixture = 3L

Temperature (T) = 27°C = 27°C + 273 = 300K

Number of mole (n) of the mixture = 0.5 + 0.2 = 0.7 mole

Gas constant (R) = 0.082atm.L/Kmol

Pressure (P) of the mixture =?

Step 3:

Determination of the pressure of the mixture.

The pressure of the mixture can be obtained as follow:

PV = nRT

P x 3 = 0.7 x 0.082 x 300

Divide both side by 3

P = (0.7 x 0.082 x 300) /3

P = 5.74 atm

Step 4:

Conversion of the pressure obtained from atm to mmHg.

1 atm = 760mmHg

Therefore, 5.74 atm = 5.74 x 760 = 4362.4 mmHg

Answer:

1) Solvent

2) Solute

3) Solute

Explanation:

According to the concept of solubility, benzene is a solvent and toulene and octylphenol ethoxylate are solutes.

Solubility is defined as the ability of a substance which is basically solute to form a solution with another substance. There is an extent to which a substance is soluble in a particular solvent. This is generally measured as the concentration of a solute present in a saturated solution.

The solubility mainly depends on the composition of solute and solvent ,its pH and presence of other dissolved substance. It is also dependent on temperature and pressure which is maintained.Concept of solubility is not valid for chemical reactions which are irreversible. The dependency of solubility on various factors is due to interactions between the particles, molecule or ions.

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To determine the mass of silver produced in the reaction, we need to calculate the moles of magnesium that react and use the mole ratio from the balanced equation. Given that 6.50x10^23 atoms of Mg react, the mass of silver produced is 232.87 grams.

To determine the mass of silver (Ag) produced, we need to calculate the number of moles of magnesium (Mg) that react and use the mole ratio from the balanced equation. First, convert the given number of atoms of Mg to moles by dividing by Avogadro's number. Then, use the balanced equation to relate the moles of Mg to the moles of Ag. Finally, convert the moles of Ag to grams by multiplying by the molar mass of Ag.

In this case, the mole ratio between Mg and Ag is 1:2. So, for every mole of Mg that reacts, 2 moles of Ag are produced. Given that 6.50x10^23 atoms of Mg react, we can calculate:

Moles of Mg = (6.50x1023 atoms / 6.022x10^23 atoms/mol) = 1.08 moles of Mg

Moles of Ag = 2 moles of Ag / 1 mole of Mg * 1.08 moles of Mg = 2.16 moles of Ag

Grams of Ag = Moles of Ag * Molar mass of Ag = (2.16 moles) * (107.87 g/mol) = 232.87 grams of Ag

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