For the equation P4 (s ) + 5 O2 (g ) → P4 O10 (s ) , if 3 mol of phosphorous react with 10 mol of oxygen, the theoretical yield of phosphorous (V) oxide will be

Answer:

1.7 L

Explanation:

1.5M = 1.5 mol/1L

1.5 M means that 1 L solution has 1.5 mol HCl

1.5 mol HCl ----- 1 L

2.5 mol HCl ---- xL

x=(2.5*1)/1.5 ≈ 1.7 L solution, so we need 1.7 L of water to make 1.7 L of solution.

Final answer:

To make a 1.5 M solution with 2.5 moles of HCl, you would need 1.67 liters of solution.

Explanation:

To calculate the volume needed to make a 1.5 M solution with 2.5 moles of HCl, we can use the formula for molarity (M), which is moles of solute divided by liters of solution. In this case:

M = moles of solute / liters of solution

Rearranging the formula to solve for the liters of solution, we get:

liters of solution = moles of solute / M

By plugging in 2.5 moles of HCl and a molarity of 1.5 M, the calculation becomes:

liters of solution = 2.5 moles HCl / 1.5 M

liters of solution = 1.67 L

Therefore, you would need 1.67 liters of solution to make a 1.5 M solution of HCl.

Answer: 5.039moles

Explanation:

No. of moles=mass/molar mass

= 362.7/72= 5.039moles

Molar mass of C5H12= 72

Final answer:

To find the number of moles of C5H12 in 362.8 grams, divide the mass by the molar mass of C5H12 (72.0 g/mol), resulting in 5.04 moles.

Explanation:

To calculate how many moles of C5H12 are in 362.8 grams of the compound, you first need to determine the molar mass of C5H12. The molar mass of a compound is calculated by summing the molar masses of all atoms in the molecule. For C5H12, the calculation is as follows:

Carbon (C) has a molar mass of 12.0 g/mol, and there are 5 carbon atoms, which contributes 5 * 12.0 = 60.0 g/mol.Hydrogen (H) has a molar mass of 1.0 g/mol, and there are 12 hydrogen atoms, which contributes 12 * 1.0 = 12.0 g/mol.

Therefore, the molar mass of C5H12 is 60.0 g/mol (carbon) + 12.0 g/mol (hydrogen) = 72.0 g/mol.

To find the number of moles, divide the mass of the compound by its molar mass:

Moles of C5H12 = Mass of C5H12 / Molar mass of C5H12 = 362.8 g / 72.0 g/mol = 5.04 moles.

So, there are 5.04 moles of C5H12 in 362.8 grams of the compound.

Answer:

4L

Explanation:

No of mole= concentrate × volume

Volume = n/C

V= 10/2.5 = 4L

Answer:

The answer to your question is 1795.5 grams of CO₂

Explanation:

Data

mass of carbon dioxide = ?

mass of Octane = 571.3 g

Process

1.- Write the balanced chemical reaction

         C₈H₁₆ + 12O₂   ⇒  8CO₂  +  8H₂O

2.- Calculate the molar mass of octane and carbon dioxide

Octane = (12 x 8) + (16 x 1) =96 + 16 = 112 g

Carbon dioxide = 8[ 12 + 2(16)] = 352 g

3.- Use proportions to find the mass of carbon dioxide

              112 g of Octane ---------------- 352 g of carbon dioxide

              571.3 g of Octane -------------  x

                    x = (571.3 x 352) / 112

                    x = 201097.6 / 112

                   x = 1795.5 grams of CO₂

Answer:

A & C im 99% sure

Explanation:

Answer: A and C is correct.

Explanation:

Mark brainliest please .

Answer:

James Watson

Explanation:

Answer:C

Explanation:

Answer:

Radioactive

Explanation:

Just did this on study island

ΔH° = -769.2 kJ is required.

Explanation:

Given equations are:

Pb(s) + PbO₂(s) + 2 H₂SO₄(l) → 2 PbSO₄(s) + 2H₂O(l);  ΔH° = –509.2 kJ ------1

SO₃(g) + H₂O(l) → H₂SO₄(l);  ΔH° = –130. kJ ----2

From the above 2 equations, by adding or subtracting or multiplying or dividing the required amount to get the final equation by means of Hess's law.

Multiplying eq. 2 by 2 we will get,

2 SO₃(g) + 2 H₂O(l) → 2 H₂SO₄(l) ;  ΔH° = -260 kJ ----3

Adding it to eq. 1 we will get,

Pb(s) + PbO₂(s) + 2 H₂SO₄(l) → 2 PbSO₄(s) + 2H₂O(l);  ΔH° = –509.2 kJ ------1

2 H₂SO₄ and 2 H₂O gets cancelled since they are on opposite sides, and the ΔH° values are added to get the ΔH° value of the required equation as,

Pb(s) + PbO₂(s) + 2 SO₃(g) → 2 PbSO₄(s)

ΔH° = -509.2 - 260 = -769.2 kJ

Answer:

[tex]\large \boxed{\text{121 L}}[/tex]

Explanation:

We can use the Ideal Gas Law.

pV = nRT

Data:

p = 0.700 atm

n = 3.80 mol

T = -1  °C

Calculations:

1. Convert the temperature to kelvins

T = (-1 + 273.15) K= 272.15 K

2. Calculate the volume

[tex]\begin{array}{rcl}pV &=& nRT\\\text{0.700 atm} \times V & = & \text{3.80 mol} \times \text{0.082 06 L}\cdot\text{atm}\cdot\text{K}^{-1}\text{mol}^{-1} \times \text{272.15 K}\\0.700V & = & \text{84.86 L}\\V & = & \textbf{121 L} \\\end{array}\\\text{The volume of the balloon is $\large \boxed{\textbf{121 L}}$}[/tex]

Answer:

90.9% is the percent yield of the reaction.

Explanation:

Mass of hydrogen gas = 24.2 g

Moles of hydrogen = [tex]\frac{24.2 g}{2g/mol}=12.1 mol[/tex]

[tex]2H_2+O_2\rightarrow 2H_2O[/tex]

According to reaction, 2 moles of hydrogen gas gives 2 moles of water , then 12.1  moles of hydrogen will give:

[tex]\frac{2}{2}\times 12.1mol=12.1mol[/tex]  water

Mass of 12.1 moles of water

= 12.1 mol × 18 g/mol = 217.8 g

Theoretical yield of water = 217.8 g

Experimental yield of water = 198 g

The percentage yield of reaction:

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

[tex]=\frac{198 g}{217.8 g}\times 100=90.9\%[/tex]

90.9% is the percent yield of the reaction.

The pH of the solution after the addition of 75.0 mL of 0.10 M KOH to a 100.0 mL sample of a 0.20 M HF solution is approximately 2.57. This is calculated using the molar concentrations of HF and KOH, the equilibrium expression for HF, and the pH formula.

To calculate the pH of a solution after adding KOH to the HF solution, we first need to calculate the produced moles of HF and KOH. The molar concentration of HF is 0.20 M in 100.0 mL which is equal to 0.02 moles. Furthermore, the molar concentration of KOH is 0.10 M in 75.0 mL which is equal to 0.0075 moles.

Since KOH is a strong base and fully ionizes, all the moles of KOH will react with HF to form F- and H2O. This will result in 0.02 - 0.0075 = 0.0125 moles of HF remaining and 0.0075 moles of F- formed.

Next, we use the Ka expression of HF, which is Ka = [H+][F-]/[HF]. Since HF is a weak acid and partially ionizes, we can assume that the concentration of H+ equals that of F- at equilibrium. Substituting the values, we get 3.5 × 10-4 = x^2/0.0125, solving for x which represents [H+], it's about 0.0027 M

Finally, we can use the definition of pH = -log[H+] to find the pH of the solution, which gives a pH of around 2.57 after adding 75.0 mL of KOH to the HF solution.

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Answer:

The answer to your question is    V = 0.32 L

Explanation:

Data

Volume of NH₃ = ?

P = 3.2 atm

T = 23°C

mass of CaH₂ = 2.65 g

Balanced chemical reaction

               6Ca  +  2NH₃   ⇒   3CaH₂  +  Ca₃N₂

Process

1.- Convert the mass of CaH₂ to moles

-Calculate the molar mass of CaH₂

 CaH₂ = 40 + 2 = 42 g

                             42 g ------------------ 1 mol

                              2.65 g --------------  x

                              x = (2.65 x 1)/42

                              x = 0.063 moles

2.- Calculate the moles of NH₃

                     2 moles of NH₃ --------------- 3 moles of CaH₂

                      x                        --------------- 0.063 moles

                                x = (0.063 x 2) / 3

                                x = 0.042 moles of NH₃

3.- Convert the °C to °K

Temperature = 23°C + 273

                      = 296°K

4.- Calculate the volume of NH₃

-Use the ideal gas law

              PV = nRT

-Solve for V

                V = nRT / P

-Substitution

                V = (0.042)(0.082)(296) / 3.2

-Simplification

               V = 1.019 / 3.2

-Result

               V = 0.32 L

Polar solute dissolve in polar solvent and non polar solute dissolve in non polar solvent. Solubility is directly proportional o temperature. The solubility increases with temperature.

Solubility shows the extent of solubility of a solute in solvent to make a solution. Solute is substances that is present in small amount. solvent is a substance that is present in large amount. Its SI unit is gram per litre or g/L.

Bond strength affect the solubility of a solute in solvent. weaker the bond strength is, more the solubility is. The weaker bond can be easily broken by water molecule.

The solubility increases with temperature. The increase in kinetic energy that comes with higher temperatures allows the solvent molecules to more effectively break apart the solute molecules that are held together by intermolecular attractions.

Therefore, solubility increases with temperature.

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The solubility of gases in water decreases as the temperature increases, a phenomenon explained by the disruption of attractive forces between gas molecules and water due to added thermal energy. This inverse relationship has significant implications, including the effects of thermal pollution on dissolved oxygen levels in natural water bodies and the principles underlying decompression sickness in divers.

The relationship between water temperature and the amount of dissolved gases follows an inverse pattern. As the temperature of water increases, the solubility of gases decreases. This phenomenon can be explained by examining the nature of molecular interactions and the process of dissolution. When gases dissolve in water, they form attractive interactions with water molecules. Dissolving is generally an exothermic process for gases, meaning it releases heat. However, with the addition of heat to the system—which is what happens when water temperature rises—this thermal energy disrupts the attractive forces between gas molecules and water, leading to a decrease in the gas's solubility.

Temperature, solubility, and dissolved gases are intricately linked. For instance, in natural water bodies, an increase in temperature due to thermal pollution can lead to lower dissolved oxygen levels, impacting aquatic life. Moreover, the principles governing this relationship also explain phenomena such as the release of gases from a carbonated beverage upon opening. This scenario is a direct application of Henry's Law, which states that the solubility of a gas in a liquid at a specific temperature decreases as the partial pressure of that gas above the liquid decreases.

The practical implications of this phenomenon extend to various scenarios, including environmental impacts like thermal pollution and human activities such as diving, where understanding the solubility of gases is crucial to avoiding decompression sickness.

Answer:

The energy released as heat when 9.94 g Cu 2 O ( s ) undergo oxidation at constant pressure is -10.142 kJ

Explanation:

Here we have

2Cu₂O ( s ) + O₂ ( g ) ⟶ 4 CuO ( s ) Δ H ∘ rxn = − 292.0 kJ mol

In the above reaction, 2 Moles of Cu₂O (copper (I) oxide) react with one mole of O₂ to produce 4 moles of CuO, with the release of − 292.0 kJ/mol of energy

Therefore,

1 Moles of Cu₂O (copper (I) oxide) react with 0.5 mole of O₂ to produce 2 moles of CuO, with the release of − 146.0 kJ  of energy

We have 9.94 g of Cu₂O with molar mass given as 143.09 g/mol

Hence the number of moles in 9.94 g of Cu₂O is given as

9.94/143.09 = 6.95 × 10⁻² moles of Cu₂O

6.95 × 10⁻² moles of Cu₂O will therefore produce 6.95 × 10⁻² ×  − 146.0 kJ mol  or -10.142 kJ.

Final answer:

The energy released as heat when 9.94 g of copper(I) oxide undergoes oxidation is calculated by determining the moles of Cu2O from its mass and using the stoichiometry of the reaction along with its enthalpy change to find the energy change. The result is approximately -10.14 kJ.

Explanation:

The problem involves calculating the energy released as heat during the oxidation of copper(I) oxide (Cu2O) to copper(II) oxide (CuO), given the mass of copper(I) oxide and the enthalpy change of the reaction. The reaction is 2 Cu2O(s) + O2(g) → 4 CuO(s) with an enthalpy change (ΔH°rxn) of -292.0 kJ/mol.

To find the energy released, we first need to find the number of moles of Cu2O. The molar mass of Cu2O is 143.09 g/mol (2*63.55 + 15.99). Using the given mass of Cu2O (9.94 g), we have:

moles of Cu2O = mass (g) / molar mass (g/mol) = 9.94 g / 143.09 g/mol = 0.0694 mol

The reaction stoichiometry shows that 2 moles of Cu2O yield -292.0 kJ, so we need to calculate the energy for 0.0694 moles:

Energy released = 0.0694 mol * (-292.0 kJ/mol) / 2 = -10.14 kJ

Therefore, the energy released as heat when 9.94 g of Cu2O undergoes oxidation at constant pressure is approximately -10.14 kJ.

Answer:

D. Atmospheres

Explanation:

Answer:

The concentration of the solution is 6 [tex]10^{-4}[/tex] mol/dm3.

Explanation:

We have the relationship between concentration and volume to be:

[tex]c_{1} v_{1} = c_{2} v_{2}[/tex]   where c1v1 and c2v2 are initial and final concentrations and volumes respectively.

NOTE: (volume should be in litres if concentration is in Molar, M. But seeing as you have 2 × 10-3, I assume you have converted from mL to L already.)

15mL × 0.002mol/dm3 = 50mL × [tex]x[/tex] mol/dm3

∴ [tex]x[/tex] = [tex]\frac{0.03}{50}[/tex]

= 0.0006 ≅ 6 ×[tex]10^{-4}[/tex]mol/dm3

Based on the data provided, the final concentration of the solution is  6 * 10⁻⁴ mol/dm3

Concentration of a solution is the amount of solute dissolved in a given volume of solution in litres.

The formula: C1V1 = C2V2 is used to calculate the concentration of solutions after dilution where

Using C1V1 = C2V2:

15 × 0.002= 50 × C2

C2 = 6 * 10⁻⁴ mol/dm3

Therefore, the final concentration of the solution is  6 * 10⁻⁴ mol/dm3.

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Answer:

Finches after drought had stronger and larger beaks to demolish the harder and larger seeds that the drought brought, a difference from those that lived in wet times that had smaller, pointy beaks to eat smaller seeds.

Explanation:

This is called the theory of animal evolution, where animals adapt according to the environment, this theory was just analyzed by this species of animals and many more on the island of Galapagos by Darwin.

What I also approve of as that animal that survives a certain environment is the one that is considered most suitable to live in that place.

The AH for the reaction is 1043 kJ/mol and the reaction is endothermic.

The reaction you provided:

2NaHCO3(s) → Na2CO3(s) + H2O(l) + CO2(g)

AH = -948 kJ/mol - (-1311 kJ/mol + -286 kJ/mol + -394 kJ/mol)

AH = -948 kJ/mol + 1311 kJ/mol + 286 kJ/mol + 394 kJ/mol

AH = 1043 kJ/mol

The value of AH is 1043 kJ/mol, which means the reaction is endothermic. This is because the AH value is positive, indicating that energy is absorbed from the surroundings during the reaction.

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To find the ΔH for the decomposition of sodium bicarbonate, we subtract the sum of the enthalpies of formation of the reactants from those of the products, which results in -95 kJ. This indicates the reaction is exothermic.

To determine the enthalpy change (ΔH) for the decomposition of sodium bicarbonate (baking soda), we use the given enthalpies of formation for the reactants and products in the reaction:

2 NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(l)

The enthalpy (ΔH) for the reaction is calculated as follows:

ΔH = { ΔHf(products) - ΔHf(reactants) }

For this reaction, the enthalpy change is:

ΔH = [(-1311 kJ/mol for Na2CO3) + (-394 kJ/mol for CO2) + (-286 kJ/mol for H2O)] - [2 x (-948 kJ/mol for NaHCO3)]

ΔH = (-1311 - 394 - 286) - (2 x -948)

ΔH = -1991 + 1896

ΔH = -95 kJ

Since the enthalpy change is negative, we can classify this reaction as exothermic. An exothermic reaction is one that releases heat to the surroundings, as evidenced by the negative sign of ΔH.

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Answer:

4 moles

Explanation:

The balanced equation for the reaction is given below:

N2 + 3H2 → 2NH3

From the balanced equation above,

1 mole of N2 produced 2 moles of NH3.

Therefore, 2 moles of N2 will produce = 2x2 = 4 moles of NH3.

Therefore, if we start with 2 moles of N2, then, we will produce 4 moles of NH3

Based on the balanced chemical equation, 2 moles of nitrogen can produce 4 moles of ammonia when reacted with sufficient hydrogen. The stoichiometric relationship is used to fill out the T-chart, demonstrating how the initial amounts of reactants lead to the production of the product.

The question at hand is regarding the stoichiometry of a chemical reaction in which nitrogen (N₂) and hydrogen (H₂) react to form ammonia (NH₃). Based on the balanced chemical equation N₂ + 2 H₂ → 2 NH₃, we can determine the stoichiometric relationship between nitrogen and ammonia. Each mole of nitrogen can produce two moles of ammonia. Therefore, starting with 2 moles of N₂, you can make 4 moles of NH₃.

Here is the T-chart filled out based on the balanced chemical equation:

Reaction
2 N₂ + 4 H₂ → 4 NH₃

Initial quantity (mol)
N₂: 2
H₂: -
NH₃: 0

Change (mol)
N₂: -2
H₂: -
NH₃: +4

Final quantity (mol)
N₂: 0
H₂: -
NH₃: 4

Answer:

A cell grows to its full size, The cell copies its DNA

Explanation:

I just did that question

During interphase, a cell grows to its full size and it copies its DNA. Division of the cytoplasm, nuclear division, and formation of two identical cells occur later in the cell cycle, not during interphase.

The events that occur during interphase, which is a phase in the cell cycle, include the following:

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Answer: The maximum amount of C that can be produced is 2.0 mol.

Explanation:

The balanced equation will be as follows.

        [tex]4A + 3B \rightarrow 4C[/tex]

As we are given that,

   moles of C = moles of A = [tex]\frac{4}{3}[/tex] moles of B

When we react 2.0 mol A with 3.0 mol B then the limiting reagent is A as specie A has less number of moles. Therefore, the maximum amount of C which can be produced is as follows.

          [tex]\frac{2.0}{4} \times 4[/tex]

              = 2.0 mol

Therefore, we can conclude that the maximum amount of C that can be produced is 2.0 mol.

The maximum amount of product C that can be produced when reacting 2.0 mol A with 3.0 mol B is 2.0 mol C.

This is because the stoichiometry of the reaction indicates that 2.0 mol A can produce a maximum of 2.0 mol C, and this is the limiting reactant in the reaction. The information that 3.0 mol B can produce 4.0 mol C is irrelevant in this case since B is in excess and the amount of product C formed is limited by the amount of reactant A.

To understand this, let's consider the stoichiometry of the reaction:

[tex]\[ aA + bB \rightarrow cC \][/tex]

 From the given information, we can deduce the following stoichiometric coefficients for the reactants:

[tex]\[ 2.0 \text{ mol A} \rightarrow 2.0 \text{ mol C} \] \[ 3.0 \text{ mol B} \rightarrow 4.0 \text{ mol C} \][/tex]

However, since A is the limiting reactant, we use its stoichiometry to determine the maximum amount of C that can be produced:

[tex]\[ 2.0 \text{ mol A} \rightarrow 2.0 \text{ mol C} \][/tex]

Thus, even though there is excess B that could theoretically produce more C, the actual amount of C produced is constrained by the amount of A present. Therefore, the reaction of 2.0 mol A with 3.0 mol B will yield 2.0 mol C, as A is the limiting reactant.

Answer:

The mass of cryolite will be produced = 71247 g or, 71.247 kg

Explanation:

The balanced chemical equation for the synthesis of cryolite

        Al₂O₃(s) + 6 NaOH(l) + 12 HF(g) → 2 Na₃AlF₆ + 9 H₂O(g)

The rise time of moon is from the evening about 3 PM. The visibility of moon in earth depends on the clouds and climate.

Moon is the only natural satellite for earth and it revolves around earth about in equal time as it takes to rotate in its own axis. Moon experience a gravitational pull from earth and moon in turn have the same force towards earth.

The time at which moon touches the upper edge of the horizon is called moon rise. The time we see moon in the sky will change with each seasons and with the rotation speed of earth.

When the whether is cloudy or rainy, moon will be invisible between the clouds. Usually moon rises at evening time about 3 PM and starts to brighten tonite. The position of moon changes as it is revolving around earth .

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Answer:C

Explanation:

Final answer:

A brightly glowing light bulb in a conductivity apparatus indicates the presence of an electrolyte in the solution, meaning it contains enough ions to conduct electricity.

Explanation:

When a conductivity apparatus is placed in a solution and the light bulb glows brightly, this indicates that the solution contains an electrolyte. An electrolyte is a substance that dissociates into ions when dissolved in water, which allows the solution to conduct electricity.

The brightness of the light bulb in the conductivity apparatus depends on the concentration of ions in the solution. A bright light suggests a high concentration of ions, corresponding to a strong electrolyte, while a dim light would indicate a lower concentration of ions, which would be a weak electrolyte.

The conductance of an aqueous solution containing the substance can be measured to identify if a substance is a strong, weak, or nonelectrolyte. To conduct electricity, the solution must contain freely mobile, charged species. Therefore, when the power supply is turned on and the light bulb in the conductivity apparatus glows brightly, the solution provides a path for the current to flow due to the presence of these charged ions.

Answer:

3.1 *10^22 atoms Cu

Explanation:

M(Cu) = 63.5 g/mol

3.3 g Cu * 1mol Cu/63.5 g Cu = 0.0520 mol Cu

0.0520 mol Cu * 6.02*10^23 atoms Cu/1 mol Cu = 3.1 *10^22 atoms Cu

Answer:

0.225M of Fecl3

Explanation:

No of mole=mass/molar mass

Molar mass of fecl3= 162g/Mol

No of mole= 10/162= 0.062mol

No of Mol = concentrate × volume

Concentration= n/V = 0.062/0.275

C= 0.225M of FeCl3

Answer:

9.09cm3

Explanation:

The following data were obtained from the question:

Mass of dimethyl sulfoxide = 10g

Density of dimethyl sulfoxide = 1.10gcm−3

Volume of dimethyl sulfoxide =?

The density of a substance is simply the mass substance per unit volume of the substance. It is represented mathematically as:

Density = Mass/volume.

With the above formula, we can obtain the volume of dimethyl sulfoxide as follow:

Density = Mass/volume

1.10gcm−3 = 10g/ volume

Cross multiply to express in linear form

1.10gcm−3 x Volume = 10g

Divide both side by 1.10gcm−3

Volume = 10g / 1.10gcm−3

Volume = 9.09cm3

Therefore, the volume of dimethyl sulfoxide the student should pour out is 9.09cm3

Answer:

9L

Explanation:

Given parameters:

Initial volume V₁ = 3.6L

Initial pressure P₁  = 2.5atm

Final pressure P₂  = 1atm

Unknown:

Final volume V₂  = ?

Condition: constant temperature  = 25°C

Solution:

This problem compares the volume and pressure of a gas at constant temperature.

This is highly synonymous to the postulate of Boyle's law. It states that "the volume of a fixed mass of gas is inversely proportional to the pressure provided that temperature is constant".

Mathematically;

              P₁V₁  = P₂V₂

where P and V are pressure and volume

          1 and 2 are initial and final states

Input the parameters and solve for V₂;

          2.5 x 3.6  = 1 x V₂

                  V₂  = 9L

Answer: 24.6kpa

Explanation:

This is a classic case where Boyle's Law can be applied.

The equation for Boyle's Law is given as: P1V1 = P2V2

Where P1 = initial pressure

P2 = final pressure

V1 = initial volume

V2 = final volume

From the question, P1 = ?, P2 = 98.2kpa , V1 =4L , V2 =1L

P1V1 = P2V2

P1 x 4L = 98.2 kpa x 1L

Make P1 subject of formula we then have:

P1 = 98.2kpa X 1L / 4L

= 24.6kpa

Answer:

24.6kpa

Explanation:

Answer:

false, false, true