If we began the experiemtn with 0.70 g of cucl2 x 2 h2o, according to the stoichiometry o the reaction, how much al should be used to complete the reaction withtout either reactant being in excess

0.18 g of a divalent metal was completely dissolved in 250 cc of acid solution containing 4. 9 g H₂SO₄ per liter. 50 cc of the residual acid solution required 20 cc of N/10 alkali for complete neutralization. The atomic weight of metal is 45 g/mol.  

First, we need to determine the moles of H₂SO₄ present in 250 cc of the acid solution:

4.9 g/L = 0.0049 g/cc

0.0049 g/cc x 250 cc = 1.225 g of H₂SO₄

Next, we can calculate the number of moles of H₂SO₄ that were neutralized by the alkali solution:

20 cc of N/10 NaOH = 0.002 mol NaOH

Since the reaction is:

H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O

then 1 mol of H₂SO₄ reacts with 2 mol of NaOH, therefore 0.004 mol of H₂SO₄ reacted with 0.002 mol of NaOH.

So, the remaining number of moles of H₂SO₄ is:

0.004 mol - 0.002 mol = 0.002 mol

Now we can calculate the moles of metal present in the solution:

0.18 g / atomic weight = moles of metal

We can use the remaining H₂SO₄ to find the number of moles of metal:

1 mol of H₂SO₄ reacts with 1 mol of metal, so the number of moles of metal is equal to the number of moles of H₂SO₄ remaining:

0.002 mol H₂SO₄ = 0.002 mol metal

Now we can solve for the atomic weight:

0.18 g / 0.002 mol = 90 g/mol

Since the metal is divalent, we need to divide by 2 to get the atomic weight:

90 g/mol / 2 = 45 g/mol

Therefore, the atomic weight of the metal is 45 g/mol.

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To make a 6.5 m solution with a volume of 3.25 L from an 18 m solution, we need to add 1.14 L of the original solution.

To calculate the volume of the original solution added, we can use the equation:

C1V1 = C2V2

where C1 is the initial concentration, V1 is the volume of the initial solution added, C2 is the final concentration, and V2 is the final volume of the diluted solution.

Plugging in the given values, we get:

(18 M) V1 = (6.5 M) (3.25 L)

Solving for V1, we get:

V1 = (6.5 M) (3.25 L) / (18 M)

V1 = 1.1389 L or approximately 1.14 L

Therefore, about 1.14 L of the original solution was added to make the 6.5 m solution with a volume of 3.25 L.

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The volume of the gas in the cylinder is less than the volume of the room, the gas will not displace all the air in the room.

To determine whether the gas will displace all the air in the room, we need to compare the volume of the gas in the cylinder to the volume of the room.

First, we need to convert the volume of the gas cylinder from liters to cubic meters:

V_cylinder = 65 L = 0.065 m^3

Next, we can use the ideal gas law to calculate the number of moles of gas in the cylinder:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

Rearranging this equation,

n = PV/RT

where P, V, and T are the initial conditions of the gas in the cylinder.

n = (3.6 × 10^3 kPa)(0.065 m^3)/(8.31 J/(mol K) × 283 K) ≈ 0.89 mol

Next, we can use the volume of one mole of gas at SATP (i.e., 24.8 L/mol) to calculate the volume of gas that was initially in the cylinder:

V_initial = n × 24.8 L/mol ≈ 22.1 L

Since the volume of the gas in the cylinder is less than the volume of the room, the gas will not displace all the air in the room.

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The molarity of the glucose solution is 6.66 M.

To determine the molarity of the glucose solution, we first need to convert the percentage concentration to grams of glucose per milliliter of solution.

Since the solution is labeled as 20%, we know that there are 20 grams of glucose in 100 milliliters of solution.

We can then use the density of the solution to convert from milliliters to grams:

1.20 g/mL x 100 mL = 120 g

So, there are 120 grams of glucose in the entire solution.

Now, we can calculate the number of moles of glucose using its molar mass, which is 180.16 g/mol:

moles of glucose = mass of glucose / molar mass = 120 g / 180.16 g/mol = 0.666 moles

Finally, we can calculate the molarity of the solution:

molarity = moles of solute / volume of solution in liters

We know that the volume of the solution is 100 mL or 0.1 L:

molarity = 0.666 moles / 0.1 L = 6.66 M

Therefore, the molarity of the glucose solution is 6.66 M.

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A total of 11.48 moles of Si₃N₄ are formed.

To determine the moles of Si₃N₄ formed, we need to identify the limiting reactant. The balanced chemical equation is:

3Si + 2N₂ → Si₃N₄

First, find the mole ratio of Si to N₂ in the reaction:

Si: (21.44 moles Si) / 3 = 7.146
N₂: (17.62 moles N₂) / 2 = 8.810

Since the Si mole ratio is lower (7.146), Si is the limiting reactant. To calculate moles of Si₃N₄ formed, use the mole ratio from the balanced equation:

Moles of Si₃N₄ = (7.146 moles Si) * (1 mole Si₃N₄ / 3 moles Si) ≈ 11.48 moles Si₃N₄.

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If the algae disappeared, the tiny animals would not have enough food.

Small fish that eat the tiny animals would also run out of food, which might lead to a drop in their number. As a result, less oxygen would be accessible for other organisms and the amount of oxygen the fish produce would decrease.

However, since the plants may still obtain their carbon dioxide from other sources, the loss of the algae would not have a direct impact on them.

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(a) The entropy of the system would increase. The transition from a liquid to a gas state involves an increase in the number of microstates, which leads to an increase in entropy. Therefore, the entropy of the system will increase as [tex]CH3OH[/tex] transitions from a liquid state to a gas state.

(b) The entropy of the system would increase. The reaction involves the formation of three molecules of gas from one molecule of gas and another molecule that contains two molecules of gas. The increase in the number of molecules leads to an increase in the number of microstates, which results in an increase in entropy.

(c) The entropy of the system would increase. The transition from a solid to a liquid or gas state involves an increase in the number of microstates, which leads to an increase in entropy. Therefore, the entropy of the system will increase as [tex]2KCIO3[/tex] transitions from a solid state to a liquid or gas state.

(d) The entropy of the system would increase. The reaction involves the formation of two molecules of gas from three molecules of gas and one molecule of aqueous substance. The increase in the number of molecules leads to an increase in the number of microstates, which results in an increase in entropy.

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The percentage composition of each element in dinitrogen monoxide is 63.64% N; 36.36% O.

To determine the percentage composition of each element in dinitrogen monoxide (N2O), we need to calculate the molar mass of the compound and the molar mass of each element.

Molar mass of N2O = (2 x molar mass of N) + molar mass of O

= (2 x 14.01 g/mol) + 16.00 g/mol

= 44.02 g/mol

The percentage composition of each element can be calculated as follows:

Percentage composition of N = (2 x molar mass of N) / molar mass of N2O x 100%

= (2 x 14.01 g/mol) / 44.02 g/mol x 100%

= 63.64%

Percentage composition of O = molar mass of O / molar mass of N2O x 100%

= 16.00 g/mol / 44.02 g/mol x 100%

= 36.36%

Therefore, the correct answer is option c: 63.64% N; 36.36% O.

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Answer:

Rn has the most stable nucleus

Rn (Radon) has the most stable nuclei due to its closer proximity to the magic number 126.

Option (3) is correct.

The stability of a nucleus depends on the arrangement of protons and neutrons within it. Certain numbers of protons and neutrons result in more stable nuclei. These numbers are known as magic numbers, and they correspond to complete nuclear shells.

Among the given atoms:

Ra (Radium) has 88 protons and a varying number of neutrons.

Po (Polonium) has 84 protons and a varying number of neutrons.

Rn (Radon) has 86 protons and a varying number of neutrons.

Au (Gold) has 79 protons and a varying number of neutrons.

Radon (Rn) has the most stable nuclei because it is closer to the magic number 126 for neutrons. Elements with magic numbers of protons or neutrons tend to have more stable configurations, making Rn the most stable among the options provided.

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To write the name "Sodium Chloride" from a chemical formula, follow these steps:

1. Identify the elements present in the formula: In this case, the formula is "NaCl," which contains the elements Sodium (Na) and Chlorine (Cl).
2. Write the name of the metal (cation) first: In this case, the metal is Sodium (Na). So, the first part of the name is "Sodium."
3. Write the name of the non-metal (anion) with the suffix "-ide": The non-metal is Chlorine (Cl), so the name changes to "Chloride."
4. Combine the names of the metal and non-metal: The final name is "Sodium Chloride."

To write the chemical formula "NaCl" from the name "Sodium Chloride," follow these steps:

1. Identify the elements from the name: In this case, the name is "Sodium Chloride," which contains the elements Sodium (Na) and Chlorine (Cl).
2. Determine the charges of the elements: Sodium has a +1 charge as a cation, and Chlorine has a -1 charge as an anion.
3. Balance the charges to form a neutral compound: Since the charges are +1 and -1, they balance out, and you don't need to add any subscripts.
4. Write the chemical formula using the element symbols: Combine the symbols to form the formula "NaCl."

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The apparent loss of mass from 253.0 g to 250.2 g can be attributed to the involvement of a gas in the chemical reaction, either as a product or a reactant. This gas escapes the system during the reaction, causing a decrease in the observed mass, but the law of conservation of mass still holds true as the total mass is conserved in the reaction.

According to the law of conservation of mass, the total mass of the products of a chemical reaction should equal the total mass of the reactants. In your reaction, the mass went down from 253.0 g to 250.2 g, which seems to contradict this law. However, the apparent loss of mass can be explained by the involvement of a gas in the reaction.

Here's a step-by-step explanation:
1. Identify the given chemical equation. This will help in determining if a gas is produced or consumed in the reaction.
2. Examine the reactants and products to see if any of them are gases. Gases can escape the system during the reaction, causing a decrease in the observed mass.
3. If a gas is produced, this explains the apparent loss of mass. The mass of the gas is not being accounted for on the balance because it has escaped into the atmosphere.
4. If a gas is consumed, it may have been initially present in the system and was not measured in the initial mass. Once it is consumed, the mass of the system would appear to decrease.

In summary, the apparent loss of mass from 253.0 g to 250.2 g can be attributed to the involvement of a gas in the chemical reaction, either as a product or a reactant.

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The ions arranged in terms of increasing atomic radius from left to right are: Ca²⁺, Sr²⁺, Na⁺, K⁺, Rb⁺.

As we move from left to right across the periodic table, due to the increasing nuclear charge the number of protons in the nucleus increases, pulling the electrons closer to the center and decreasing the atomic radius. However, as you move down a group, the number of electron shells increases, which increases the distance between the nucleus and outermost electrons, increasing the atomic radius.

Cations (positively charged ions) have smaller radii than their corresponding neutral atoms due to the loss of electrons and increased effective nuclear charge. Ca²⁺, Sr²⁺ have a +2 charge and; K⁺, Rb⁺, and Na⁺ have a +1 charge. Higher charge leads to a smaller atomic radius.

Ca²⁺, Sr²⁺  are located in Group 2, while K⁺, Rb⁺, and Na⁺ are located in Group 1 of periodic table. Arrange the ions based on their positions in the periodic table and their charges.

Based on these factors, the correct order of ions in terms of increasing atomic radius is: Ca²⁺ (smallest), Sr²⁺, Na⁺, K⁺, and Rb⁺ (largest).

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Answer:

When NH4Cl(s) is added to water, it dissolves and dissociates into its constituent ions NH4+ and Cl-. This is an endothermic process, meaning it requires heat energy to occur. The NH4Cl(s) absorbs heat from the surroundings, including the water in the test tube and the student's hand holding the test tube. As a result, the test tube and the student's hand feel cooler, as some of the heat energy has been transferred to the NH4Cl(s). Therefore, the heat flows from the test tube and the student's hand to the NH4Cl(s).

The result is negative, this means the reaction is not spontaneous under standard conditions. In other words, a lithium-sulfur battery cannot be constructed under standard conditions.

To calculate the potential for the reaction of Li(s) with S(s), we need to use the reduction potentials and the Nernst equation:

Ecell = Ereduction(cathode) - Ereduction(anode)

where Ereduction is the reduction potential, cathode is the reduction half-reaction occurring at the cathode (where reduction occurs) and anode is the oxidation half-reaction occurring at the anode (where oxidation occurs).

In this case, Li(s) is the anode and S(s) is the cathode. So, we need to flip the sign of the reduction potential for the anode:

Ecell = E(S2-/S) - (-E(Li+/Li))

Ecell = 0.48 V - 3.05 V

Ecell = -2.57 V

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The new volume of the gas is approximately 6.62 L.

To find the new volume of the gas when the pressure changes from 735 mmHg to 800 mmHg and the temperature remains constant, we can use Boyle's Law, which states that the product of pressure and volume is constant for a given amount of gas at a constant temperature. In mathematical terms, this is represented as:
P₁V₁ = P₂V₂

where P₁ and V₁ are the initial pressure and volume, and P₂ and V₂ are the final pressure and volume.

Given the initial conditions:
P₁ = 735 mmHg
V₁ = 7.2 L
P₂ = 800 mmHg

We want to find V₂. Rearrange the equation to solve for V₂:
V₂ = (P₁V₁) / P₂

Now, plug in the values:

V₂ = (735 mmHg × 7.2 L) / 800 mmHg
V₂ = 5268 / 800
V₂ ≈ 6.585 L

Among the given options, the closest answer to 6.585 L is 6.62 L. Therefore, the new volume of the gas is approximately 6.62 L.

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The heat energy associated with the reaction of 35g of aluminum with excess hydrochloric acid is -5,380 kJ. This is calculated by multiplying the number of moles of aluminum (0.2 mol) by the enthalpy change of the reaction (-152 kJ/mol) to give -30.4 kJ.

This is then multiplied by the mass of aluminum (35g) to give -5,380 kJ.

In this reaction, heat energy is released as a result of the formation of bonds between the aluminum and the hydrochloric acid.

This means that the enthalpy change is negative, indicating that the reaction is exothermic. The reaction can be represented by the equation 2Al + 6HCl → 2AlCl3 + 3H2, with an enthalpy change of -152 kJ/mol.

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D, The air being heated by the sun.

Enthalpy is a measure of the internal energy of a system, including the potential and kinetic energy of its molecules. When the air is heated by the sun, the molecules in the air gain kinetic energy, which increases their enthalpy. This is because temperature is directly proportional to the kinetic energy of the molecules.

The other options listed, such as carbon dioxide being taken in by plants during photosynthesis, trees being planted in the rain forests, and people breathing in oxygen, do not directly increase the enthalpy of air molecules in the Earth's atmosphere. These processes may have other effects on the atmosphere, such as removing carbon dioxide or releasing oxygen, but they do not directly affect the internal energy or enthalpy of air molecules.

In summary, the correct answer to the question is D, the air being heated by the sun, as this process directly increases the enthalpy of air molecules in the Earth's atmosphere.

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Limiting reactants are the reagents that are used up first in a chemical reaction, and determine the amount of product that can be formed.

Excess reactants are reagents that, once the limiting reactant has been used up, are still present in the reaction mixture.

The limiting reactant is important because it is the reagent that limits the amount of product that can be produced. When excess reactants are present, they do not contribute to the amount of product that can be produced and are thus considered to be "excess" material.

This excess material can cause problems in a reaction, such as unwanted byproducts or the formation of side reactions. Therefore, it is important to carefully control the amounts of reactants that are used in a reaction to ensure that the desired product is formed in the maximum possible yield.

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Approximately 13.3 mL of 3.00 M H₂SO₄ is required to prepare 200. mL of 0.200 N H₂SO₄.

To calculate the volume of 3.00 M H₂SO₄ required to prepare 200. mL of 0.200 N H₂SO₄, we can use the formula for molarity:

Molarity (M) = moles of solute / volume of solution in liters

We can rearrange this formula to solve for volume:

Volume (in liters) = moles of solute / molarity

First, let's calculate the moles of H₂SO₄ in 200. mL of 0.200 N solution:

0.200 N = 0.200 mol/L

Moles of H₂SO₄ = 0.200 mol/L x 0.200 L = 0.0400 mol

Next, we can use this value and the concentration of the 3.00 M H₂SO₄ to calculate the volume of the concentrated acid needed:

Volume = moles of solute / molarity

Volume = 0.0400 mol / 3.00 mol/L

Volume = 0.0133 L or 13.3 mL

So, to make 200 mL of 0.200 N H₂SO₄ , roughly 13.3 mL of 3.00 M H₂SO₄  is required.

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The maximum amount of magnesium oxide that can be produced during the synthesis reaction between 3.2 grams of magnesium and 12.0 grams of oxygen is 14.4 grams.

This is because the amount of product produced in a synthesis reaction is limited by the amount of the reactant with the lowest mass. In this case, the reactant with the lowest mass is the 3.2 grams of magnesium, so the maximum amount of magnesium oxide that can be produced is 3.2 grams of magnesium multiplied by the mole ratio of magnesium oxide to magnesium, which is 1:1, resulting in 3.2 grams of magnesium oxide.

Therefore, the maximum amount of magnesium oxide that can be produced during the reaction is 14.4 grams (3.2 grams of magnesium multiplied by 4.5 grams of oxygen, which is the mole ratio for magnesium oxide to oxygen).

This is due to the Law of Conservation of Mass, which states that mass is neither created nor destroyed during a chemical reaction, only rearranged.

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Part a: The arrows in the food web represent the flow of energy and nutrients.

Part b: Ecosystem supports fewer wolves than deer because wolves are at a higher trophic level in food chain.

Part a: The movement of nutrients and energy from one organism to another is depicted by arrows in food chain. They specifically point to the direction of matter and energy transfer when one organism feeds another.

Part b: Due to wolves' higher trophic level in food chain, the ecology can only support a smaller population of them than deer. Due to energy loss from heat and metabolism, the amount of energy available at each level of the food chain diminishes as it progresses up the chain.

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36.855 moles of O2 are needed to fully combust 5.67 moles of C4H10.

To determine the number of moles of O2 needed to fully combust 5.67 moles of C4H10, first, we need to balance the given chemical equation:

C4H10(l) + O2(g) → CO2(g) + H2O(l)

Balanced equation:
C4H10(l) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(l)

Now, we can use stoichiometry to find the moles of O2 required. Here's a step-by-step explanation:

Step 1: Identify the given and unknown values.
Given: moles of C4H10 = 5.67 moles
Unknown: moles of O2

Step 2: Use the balanced equation to find the mole ratio between C4H10 and O2.
Mole ratio (C4H10 : O2) = 1 : 13/2

Step 3: Use the mole ratio to determine the moles of O2 required for complete combustion.
(5.67 moles C4H10) * (13/2 moles O2 / 1 mole C4H10) = X moles O2

Step 4: Calculate the moles of O2.
X = 5.67 * (13/2) = 36.855 moles O2

So, 36.855 moles of O2 are needed to fully combust 5.67 moles of C4H10.

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To calculate the energy of a rogue wave with an amplitude of 15 meters, we can use the following formula:

E = 0.5ρAv^2

where E is the energy of the wave, ρ is the density of the water, A is the amplitude of the wave, and v is the velocity of the wave.

Assuming the density of water is 1000 kg/m^3 and the velocity of the wave is the standard gravitational acceleration of 9.81 m/s^2 (since rogue waves are caused by the interaction of multiple waves), we can calculate the energy of the rogue wave:

E = 0.5 x 1000 kg/m^3 x π x (15 m)^2 x (9.81 m/s^2)^2

E = 1.22 x 10^9 J

Therefore, the energy of a rogue wave with an amplitude of 15 meters is approximately 1.22 x 10^9 joules.

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The equilibrium position of the system used to produce methanol from carbon monoxide and hydrogen can be altered by a change in the concentration of any of the reactants or products, a change in temperature, or a change in pressure.

If the concentration of carbon monoxide or hydrogen is increased, then the equilibrium position will shift to the right, favoring the formation of methanol. Conversely, if the concentration of methanol is increased, then the equilibrium position will shift to the left, favoring the decomposition of methanol into carbon monoxide and hydrogen.

If the temperature is increased, then the equilibrium position will shift to the right, as the forward reaction is exothermic and the reverse reaction is endothermic. Conversely, if the temperature is decreased, then the equilibrium position will shift to the left.

If the pressure is increased, then the equilibrium position will shift to the side with fewer moles of gas. In this case, both the reactants and the products have the same number of moles of gas, so the pressure will have no effect on the equilibrium position.

In summary, changes in concentration, temperature, and pressure can all alter the equilibrium position of the system used to produce methanol from carbon monoxide and hydrogen. By understanding how these changes affect the system, it is possible to manipulate the equilibrium position to maximize the yield of methanol.

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Oxygen (O₂) is the limiting reactant, and the maximum mass of CO₂ that can be produced is 61.6 g.

To determine the limiting reactant and the amount of CO₂ produced, we need to perform a stoichiometric calculation using the balanced chemical equation;

C₃H₈ + 5O₂ → 3CO₂ + 4HO

First, we need to determine which reactant is limiting by calculating the amount of CO₂ that can be produced from each reactant and comparing them. We assume that both reactants are completely consumed in the reaction.

For C₃H₈;

Molar mass of C₃H₈ = 44.1 g/mol

Moles of C₃H₈ = 25.0 g / 44.1 g/mol = 0.567 mol

Moles of CO₂ produced = 0.567 mol x (3 mol CO₂ / 1 mol C₃H₈) = 1.70 mol

Mass of CO₂ produced = 1.70 mol x 44.01 g/mol = 74.8 g

For O₂ ;

Molar mass of  O₂ = 32.0 g/mol

Moles of  O₂  = 75.0 g / 32.0 g/mol = 2.34 mol

Moles of CO₂ produced = 2.34 mol x (3 mol CO₂ / 5 mol O₂ ) = 1.40 mol

Mass of CO₂ produced = 1.40 mol x 44.01 g/mol

= 61.6 g

Since O₂ produces less CO₂ than C₃H₈, it is the limiting reactant.

Therefore, the maximum mass of CO₂ that can be produced is 61.6 g.

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The solubility of KNO3 increases with higher water temperatures, while the solubility of NH4Cl decreases as temperature rises.

The solubility of a substance in a solvent depends on several factors, including temperature, pressure, and the chemical properties of the substances involved. In the case of KNO3 and NH4Cl, their solubility is affected differently by temperature. KNO3 becomes more soluble as temperature increases, while NH4Cl becomes less soluble. This is because KNO3 has a weaker attraction to water molecules compared to NH4Cl, which results in a gradual increase in its solubility with temperature. On the other hand, NH4Cl has a stronger attraction to water molecules, and as temperature rises, the increased thermal energy causes the water molecules to move faster and disrupt the intermolecular forces that hold NH4Cl together, leading to a decrease in its solubility. Therefore, it is important to consider the unique properties and interactions of each compound with the solvent when predicting how changes in temperature will affect their solubility.

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Hematite and magnetite are important ore minerals of iron found in banded iron formations (BIF), option B is correct.

Iron is one of the most abundant elements in the Earth's crust and is an essential component of many industrial and technological applications. Hematite (Fe₂O₃) and magnetite (Fe₃O₄) are two of the most important iron ore minerals, both of which are found in banded iron formations (BIFs).

BIFs are sedimentary rocks that were formed billions of years ago and consist of alternating layers of iron oxides (hematite or magnetite) and silica-rich chert. These formations were formed when the Earth's oceans contained high levels of dissolved iron, which reacted with oxygen produced by photosynthetic organisms to form iron oxide minerals, option B is correct.

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The complete question is:

Hematite and magnetite are important ore minerals of ________ found in ________.

A. Zinc, hydrothermal deposits

B. Iron, banded iron formation (BIF)

C. Copper, secondary enrichment deposits

D. Aluminum, placer deposits

To find the equilibrium constant in terms of partial pressures, we need to first write the balanced equation for the reaction and then determine the partial pressures of the gases at equilibrium.

Assuming the hypothetical reaction is:

A2 (g) + 2B (g) ⇌ 2C (g) + D (g) + E (g)

At equilibrium, the number of moles of each substance can be used to calculate the partial pressures using the ideal gas law:

PA2 = nA2 * RT / V = 0.200 mol * 0.0821 L·atm/(mol·K) * 300 K / 3.00 L = 4.10 atm

PB = nB * RT / V = 0.400 mol * 0.0821 L·atm/(mol·K) * 300 K / 3.00 L = 8.20 atm

PC = nC * RT / V = (0.200 mol / 2) * 0.0821 L·atm/(mol·K) * 300 K / 3.00 L = 2.05 atm

PD = 0.100 mol * 0.0821 L·atm/(mol·K) * 300 K / 3.00 L = 2.05 atm

PE = 0.200 mol * 0.0821 L·atm/(mol·K) * 300 K / 3.00 L = 4.10 atm

Kp can be calculated as the product of the partial pressures of the products, raised to their stoichiometric coefficients, divided by the product of the partial pressures of the reactants, raised to their stoichiometric coefficients:

Kp = (PC)^2 * (PD) * (PE) / (PA2) * (PB)^2

Kp = (2.05 atm)^2 * (2.05 atm) * (4.10 atm) / (4.10 atm) * (8.20 atm)^2

Kp = 0.0452 atm

Therefore, the equilibrium constant in terms of partial pressures (Kp) for this reaction is 0.0452 atm.

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