How many calories are needed to raise the temperature of 25 grams of water form 50°C to 70°C? The specific heat of water is 1cal/g°C

Answer: 68.6 kPa

Explanation:

To calculate the new pressure, we use the equation given by Boyle's law. This law states that pressure is directly proportional to the volume of the gas at constant temperature.

The equation given by this law is:

[tex]P_1V_1=P_2V_2[/tex]

where,

[tex]P_1\text{ and }V_1[/tex] are initial pressure and volume.

[tex]P_2\text{ and }V_2[/tex] are final pressure and volume.

We are given:

[tex]P_1=?\\V_1=13.81L\\P_2=261.1kPa\\V_2=3.63L[/tex]

Putting values in above equation, we get:

[tex]P_1\times 13.81L=261.1\times 3.63L\\\\P_1=68.6kPa[/tex]

Thus pressure  before its volume was decreased was 68.6 kPa

The answer is Y < X < Z

Final answer:

The order of increasing strength of intermolecular forces for substance X (liquid), Y (gas), and Z (solid) is: Y < X < Z, with the gas having the weakest and the solid having the strongest intermolecular forces.

Explanation:

If we consider substances X, Y, and Z, which are a liquid, a gas, and a solid respectively, and they are all at the same temperature and pressure, the order of increasing strength of their intermolecular forces can be determined based on their states of matter. Given that substances with stronger intermolecular forces are more likely to be a solid at room temperature and will have a higher boiling point, it follows that the solid will have the strongest forces, followed by the liquid, and then the gas. Consequently, substance Z (the solid) would have the strongest intermolecular forces, substance X (the liquid) would have intermediate forces, and substance Y (the gas) would have the weakest forces.

Answer:

200 mph

Explanation:

600/3=200

Answer: the percentage of acetic acid will be low.

Explanation: The major aim during titration of acids and bases is to  determine the endpoint , that is exact point where the acid  in the beaker changes colour, (in this case, pink )with an additional  drop from the burette containing the base, since it is usually difficult to mark the equivalence point that tells us when  all the substrate in the beaker has been neutralized completely with the buretted substance.

Overshooting the end point is  an error which can occur when the person involved in the  the titration accidently goes beyond this  endpoint by adding too much of the substance(base) from the burette into the beaker missing the exact endpoint.

This implies that the person  has  added too much of the burreted liquid, ie the base than required  , making the acid in the beaker to continue to react resulting  to a lower concentration of the acid (acetic acid)  with excess base.(NaOH)

Answer:

For the reaction N2 (g) and 2N (g) the energy is required to break the bond in N2 to from N atoms. This means AH is positive, is an endothermic reaction.

Explanation:

Entropy increases that  is positive  because atoms are now free to move.

Answer : The amount of heat required is, 2160 cal.

Explanation :

The process involved in this problem are :

[tex](1):H_2O(s)(0^oC)\rightarrow H_2O(l)(0^oC)\\\\(2):H_2O(l)(0^oC)\rightarrow H_2O(l)(100^oC)\\\\(3):H_2O(l)(100^oC)\rightarrow H_2O(g)(100^oC)[/tex]

The expression used will be:

[tex]Q=[m\times \Delta H_{fusion}]+[m\times c_{p,l}\times (T_{final}-T_{initial})]+[m\times \Delta H_{vap}][/tex]

where,

[tex]Q[/tex] = heat required for the reaction = ?

m = mass of ice = 3 g

[tex]c_{p,l}[/tex] = specific heat of liquid water = [tex]1cal/g^oC[/tex]

[tex]\Delta H_{fusion}[/tex] = enthalpy change for fusion = [tex]80cal/g[/tex]

[tex]\Delta H_{vap}[/tex] = enthalpy change for vaporization = [tex]540cal/g[/tex]

Now put all the given values in the above expression, we get:

[tex]Q=[3g\times 80cal/g]+[3g\times 1cal/g^oC\times (100-0)^oC]+[3g\times 540cal/g][/tex]

[tex]Q=2160cal[/tex]

Therefore, the amount of heat required is, 2160 cal.

To vaporize a 3 g ice cube initially at 0°C, a total heat of 2160 cal is required. This includes the heat required to melt the ice, heat the melted ice to water's boiling point, and vaporize the water.

The process to vaporize a 3 g ice cube at 0°C consists of three steps. First, the ice cube needs to melt. This requires an amount of heat given by Q = mass x latent heat of fusion. i.e., Q = 3 g x 80 cal/g = 240 cal.`

Then, the water obtained from melted ice at 0°C needs to be heated up to 100°C. The required heat is Q = mass x specific heat x ΔT, i.e., Q = 3 g x 1 cal/g°C x (100°C-0°C) = 300 cal.

Finally, the 100°C water needs to be vaporized. This requires an amount of heat given by Q = mass x latent heat of vaporization. i.e., Q = 3 g x 540 cal/g = 1620 cal.

So, the total heat required to vaporize a 3 g ice cube initially at 0°C is 240 cal + 300 cal + 1620 cal = 2160 cal.

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Answer:

B. The amount of oxygen will decreases

Explanation:

According to Le Châtelier’s Principle, when the condition of the system changes the equilibrium will shift to compensate for the changes. When temperature decrease, the pressure will also decrease and this will shift the equilibrium to the side with exothermic reaction or less molecule count.

The question is not giving the equilibrium reaction of oxygen, so I assume its

O2 + Hb = HbO2

Since the number of molecules in the right side is lower, then the number of oxygen will decrease since the reaction will shift to the right.

Final answer:

When the system is at equilibrium with specific initial pressures and the volume of the container is reduced by half, the pressure of each gas changes accordingly.The pressure of NO₂ will be 1.634 atm, and the pressure of N₂O₄ will be 0.1334 atm.

Explanation:

When the system is at equilibrium, it contains NO₂at a pressure of 0.817 atm, and N₂O₄ at a pressure of 0.0667 atm. If the volume of the container is reduced to half its original volume, the pressure of each gas will change.

According to the ideal gas law, the pressure of each gas will double when the volume is reduced by half. So, after re-establishing equilibrium, the pressure of NO₂ will be 1.634 atm, and the pressure of N₂O₄ will be 0.1334 atm.

Answer:

an electron is part of the 3 things that are in an atom, it has a negative charge

Answer:

The answer to your question is 0.04 M

Explanation:

Data

mass of Na₂SO₄ = 14.2 g

volume = 2.50 l

Molarity = ?

Process

1.- Calculate the molar mass of Na₂SO₄

Na₂SO₄ = (23 x 2) + (32 x 1) + (16 x 4) = 46 + 32 + 64 = 142 g

2.- Calculate the number of moles of Na₂SO₄

                    142 g of Na₂SO₄ ------------------- 1 mol

                     14.2 g of Na₂SO₄ ------------------  x

                                   x = (14.2 x 1) / 142

                                   x = 0.1 moles

3.- Calculate the molarity

Molarity = moles /volume

-Substitution

Molarity = 0.1 / 2.5

-Result

Molarity = 0.04

Answer:

[tex] = 1.92*10^-^3^0 C.m[/tex]

Explanation:

Given:

[tex] r_ca_^2_^+ = 0.100 nm[/tex]

[tex] r_o_^2_^- = 0.14 nm [/tex]

Let's find the distance of separation between cation and anion when there is no applied electric field with the formula:

[tex] d = r_ca_^2_^+ + r_o_^2_^- [/tex]

d = 0.100 nm + 0.140 nm

= 0.240 nm

Let's also calculate the distance of separation between anion and cation when there is an applied electric field.

We use the formula:

∆d = 5%d => 0.05d

= 0.05 * 0.024 nm

∆d = 0.0120 nm

[tex]0.120* 10^-^9m[/tex]

[tex]= 1.20*10^-^1^1m[/tex]

Given magnitude of each dipole= [tex]1.602*10^-^1^9 C [/tex]

Let's find the dipole moment, with the formula:

p = q∆d

Substituting figures in the formula, we have:

[tex]p = 1.602*10^-^1^9 * 12*10^-^2^1 [/tex]

[tex] = 1.92*10^-^3^0 C.m[/tex]

Answer:

Explanation:

Answer:

= 1.92*10^-^3^0 C.m

Explanation:

Given:

r_ca_^2_^+ = 0.100 nm

r_o_^2_^- = 0.14 nm

Let's find the distance of separation between cation and anion when there is no applied electric field with the formula:

d = 0.100 nm + 0.140 nm = 0.240 nm

Let's also calculate the distance of separation between anion and cation when there is an applied electric field.

We use the formula:

∆d = 5%d => 0.05d

= 0.05 * 0.024 nm

∆d = 0.0120 nm

0.120* 10^-^9m

= 1.20*10^-^1^1m

Given magnitude of each dipole= 1.602*10^-^1^9 C

Let's find the dipole moment, with the formula:

p = q∆d

Substituting figures in the formula, we have:

p = 1.602*10^-^1^9 * 12*10^-^2^1

= 1.92*10^-^3^0 C.m

Answer:

Explanation:

The terms 'anode' and 'cathode' are applied to electrodes based on the chemistry occurring at a specified electrode. That is, the anode is ALWAYS the site of oxidation and the cathode is ALWAYS the site of the reduction reaction in electrochemical process. The charge (+ or -) results from the chemistry. In Voltaic Cells the anode is always the site of oxidation and is negative (-) and the cathode is the site of reduction and is always positive (+). However, in 'Electrolytic Cells' the charges are opposite at the electrodes. That is, at the electrode where oxidation is taking place in the electrolytic cell the charge on the electrode will be positive (+) and the charge on the electrode where reduction is taking place the charge will be negative (-).

As far as acronyms (or memory devices) one might consider each type cell separately...

Voltaic Cells

Anode => A Negative -ode (always site of oxidation) ... the other electrode is positive and site of reduction.                  

Electrolytic Cells

For electrolytic cells, just remember the electrode charges are opposite those of the Voltaic Cell but the chemistry is always the same. Charge is due to chemistry and type of cell, but anode is always oxidation and cathode is always reduction.      

Answer: An acid has more hydrogen ions in solution.

Explanation: Acids increase hydrogen/hydronium ion concentration in a solution, have pH's less than seven, have a low hydroxide concentration, and increase positive ions in a solution.

The correct definition of an acid is: An acid has more hydrogen ions in solution. Thus, the correct answer is option with 'An acid has more hydrogen ions in solution'.

An acid is characterized by its ability to increase the concentration of hydrogen ions (H⁺) when dissolved in water. This results in a pH lower than 7, indicating increased acidity. The pH scale measures the acidity or basicity of a solution; acids have pH values less than 7.

Let's understand other options given:

An acid has a pH of 7:

An acid has hydroxide ions:

An acid has fewer positive ions in solution:

Therefore, the defining characteristic of an acid is the presence of more hydrogen ions (H⁺) in solution.

Final answer:

The correct option is (a), which states that the precipitate formed when sodium sulfate and silver nitrate solutions are mixed is silver sulfate, and it provides the correct net ionic equation for this precipitation reaction.

Explanation:

When solutions of sodium sulfate (Na2SO4) and silver nitrate (AgNO3) are mixed together, a double-replacement reaction occurs. The balanced chemical equation for this reaction is:

Na2SO4(aq) + 2AgNO3(aq) → Ag2SO4(s) + 2NaNO3(aq)

The precipitate formed in this reaction is silver sulfate (Ag2SO4). The net ionic equation for the formation of the precipitate is:

2Ag+(aq) + SO42-(aq) → Ag2SO4(s)

Answer (a) is the correct option, as it accurately identifies the precipitate and provides the correct net ionic equation for its formation.

Answer:

Heating is the best method

Explanation:

When a mass of crystals containing Water of crystallization is heated sufiiciently to a high temperature, water vapor may be driven off the crystals by the action of heat alone.

Answer:

Explanation:

If solid/crystals, compound can be dried by applying heat to remove the water of crystallization.

Drying agents are also utile in removing moisture from compounds in a dessicator. Substances which absorb water from air can be used as drying agents for gases. For instance, [tex]CaCl_{2}[/tex], CaO or silica gel is suitable for drying gases, depending on reactivity of the substance.

Antoine Lavoisier divided elements into four categories. Dmitri Mendeleev arranged elements by atomic mass and predicted undiscovered elements. Johann Wolfgang Dobereiner created groups of three elements based on similar properties, whereas John Newlands also arranged elements by atomic weights and predicted some properties of missing elements.

The Periodic Table has been created thanks to several scientists who categorized elements by different methods. Antoine Lavoisier, known as the father of modern chemistry, divided elements into four categories: gases, non-metals, metals, and earths. Consequently, the scientist who divided elements into four categories was Antoine Lavoisier. Dmitri Mendeleev arranged elements according to their atomic mass and used this order to predict the properties of undiscovered elements. Hence, Dmitri Mendeleev is the scientist who used patterns to predict undiscovered elements. Johann Wolfgang Dobereiner, suggested a law of triads, where patterns among groups of three elements were identified based on their properties. Thus, Dobereiner is the scientist who created groups of three elements, each based on similar properties. Lastly, John Newlands arranged elements in order of atomic weights, predicting some properties of missing elements.

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The answer for the following problem is mentioned below.

Explanation:

 Given:

Initial pressure ([tex]P_{1}[/tex]) = 600 mm of Hg

Final pressure ([tex]P_{2}[/tex]) = 1200 mm of Hg

Initial volume ([tex]V_{1}[/tex]) = 200 ml      

To find:

Final volume ([tex]V_{2}[/tex])

We know;

According to the ideal gas equation,

    P × V = n × R × T

Where;

P represents the pressure of the gas

V represents the volume of the gas

n represents the no of moles of the gas

R represents the universal gas constant

T represents the temperature of the gas

So,

 From the above mentioned equation,

        P × V = constant

[tex]\frac{P_{1} }{P_{2} }[/tex] = [tex]\frac{V_{1} }{V_{2} }[/tex]

Where,

([tex]P_{1}[/tex]) represents the initial pressure of the gas

([tex]P_{2}[/tex]) represents the final pressure of the gas

([tex]V_{1}[/tex])  represents the initial volume of the gas

([tex]V_{2}[/tex])  represents the final volume of the gas

So;

[tex]\frac{600}{1200}[/tex] = [tex]\frac{V_{2} }{200}[/tex]    

[tex]V_{2}[/tex] = 100 ml

Therefore the final volume of the gas is 100 ml.                                                                                                                                                                              

Final answer:

Using Boyle's Law, which states that the product of pressure and volume for a gas is constant at a fixed temperature, it is calculated that the new volume of the CO2 (g) sample when the pressure is doubled to 1200 mmHg at constant temperature is 100 mL.

Explanation:

The question asks about the change in volume of a gas sample when the pressure is increased while keeping the temperature constant. This scenario is described by Boyle's Law, which states that for a given mass of gas at constant temperature, the volume of the gas varies inversely with the pressure. The initial condition for the CO2 (g) is 200 mL at 600 mmHg, and after the pressure is increased to 1200 mmHg, we want to find the new volume.

Boyle's Law can be expressed as P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume, respectively. Using this relationship, when P1 = 600 mmHg, V1 = 200 mL, P2 = 1200 mmHg, we need to solve for V2. When we plug these values into the equation, we get V2 = (P1 * V1) / P2 = (600 mmHg * 200 mL) / 1200 mmHg = 100 mL.

Therefore, the new volume of the CO2 (g) sample when the pressure is increased to 1200 mmHg at constant temperature is 100 mL.

Answer:E is an acidic

Explanation:

Soo he should avoid the drink E and in pH measurement the more acidic is below 7 and the the more alkali is above 7 and the neutral drink is B and it may a water ...

Answer:

The solvent is Nitrogen and the solute is oxygen

Explanation:

Normally the solvent always contains higher amount of substance than the solute in a particular solution

Answer:

Sea water, a solution composed of a variety of salts dissolved in water. The salt is the SOLUTE

Soda water, a solution composed of carbon dioxide gas dissolved in water. The water is the SOLVENT

Air, a solution composed of 78% nitrogen and 21% oxygen. The nitrogen is the  SOLVENT

Explanation:

its right on EDGE

The equation which represents the chemical equilibrium is  2 NO₂ ⇄ N₂0₄

Explanation:

           2 NO₂ ⇄ N₂0₄.

Answer:

Acid-base equilibrium.

Explanation:

At low temperatures the amines react with carboxylic acids as bases and not as nucleophiles. This acid-base reaction is disadvantageous on heating, with the nucleophilic attack that will form the amide prevailing under these conditions.

Answer:

Ag+(aq) + Cl-(aq) <--->AgCl(s)

Ksp = [Ag+] [Cl-]

aii) Pb2+(aq) + 2Cl-(aq) <--->PbCl2(s)

Ksp = [Pb+] [Cl-]^2

Explanation:

In this question, we are to write the net ionic equation and corresponding Ksp expression for the salts in the question.

We proceed as follows;

Ag+(aq) + Cl-(aq) <--->AgCl(s)

Ksp = [Ag+] [Cl-]

aii) Pb+2(aq) + 2Cl-(aq) <--->PbCl2(s)

Ksp = [Pb+] [Cl-]^2

Final answer:

To write net ionic equations for AgCl and PbCl2, the equations are AgCl(s)
ightarrow Ag+(aq) + Cl-(aq) with Ksp = [Ag+][Cl-], and PbCl2(s)
ightarrow Pb2+(aq) + 2Cl-(aq) with Ksp = [Pb2+][Cl-]^2. These represent the dissolution of silver chloride and lead (II) chloride, respectively.

Explanation:

To write the net ionic equations and corresponding Ksp expressions for the dissolution of solid silver chloride (AgCl) and lead (II) chloride (PbCl2), you should consider both substances dissolving separately in water:

AgCl

Net ionic equation: AgCl(s)
ightarrow Ag+(aq) + Cl-(aq)

Ksp expression: Ksp = [Ag+][Cl-]

This represents the solubility product for silver chloride, which is given as 1.8  imes 10^-10.

PbCl2

Net ionic equation: PbCl2(s)
ightarrow Pb2+(aq) + 2Cl-(aq)

Ksp expression: Ksp = [Pb2+][Cl-]^2

This represents the solubility product for lead (II) chloride, which is given as 1.6  imes 10^-5. Note that because there are two chloride ions for every lead ion that dissolves, the concentration of chloride appears squared in the expression.

Answer:

32.232 L

Explanation:

-Given the volume at 1.58atm is 20.4 L

-At standard pressure, the pressure is 1.00atm

-We apply Charle's Law to find the volume at STP:

[tex]P_1V_1=P_2V_2\\\\\\1.58\ atm\times 20.4\ L=1.00\ atm\times V_2\\\\V_2=\frac{1.58\times 20.4}{1.00}\\\\\\\\=32.232\ L[/tex]

Hence, the volume of the gas at STP is 32.232 L

Answer:

oxidation number

Explanation:

Describes the degree of oxidation of an atom in a chemical compound.

Answer: The mass of solution the student should use is 256 g

Explanation:

Given : 29.3 % w/w which means that 29.3 g of solute is present in 100 g of solution

Thus 100 g of solution contains = 29.3 g of solute

0.50 kg or 500 g of solution contains = [tex]\frac{29.3}{100}\times 500=146.5[/tex] g of solute   (1kg=1000g)

146.5 g of solute is available in = 500 g of solution

Thus 75 g of solute is available in = [tex]\frac{500}{146.5}\times 75 g=256g[/tex] of solution

Thus the mass of solution the student should use is 256 g

Answer:

ΔSv = 0.1075 KJ/mol.K

Explanation:

Binary solution:

∴ a: solvent

∴ b: solute

in equilibrium:

⇒ Ln (1 - Xb) = ΔG/RT

∴ ΔG = ΔHv - TΔSv

⇒ Ln(1 -Xb) = ΔHv/RT - ΔSv/R

∴ Xb → 0:

⇒ Ln(1) = ΔHv/RT - ΔSv/R

∴ T = T*b....normal boiling point

⇒ 0 = ΔHv/RT*b - ΔSv/R

⇒ ΔSv = (R)(ΔHv/RT*b)

⇒ ΔSv = ΔHv/T*b

∴ T*b = 80°C ≅ 353 K

⇒ ΔSv = (38 KJ/mol)/(353 K)

⇒ ΔSv = 0.1075 KJ/mol.K

Answer:

204.78 mL

Explanation:

- use Charle's law and rearrange formula

- change C to K

- Hope this helped! Let me know if you need further explanation.

The following questions are answered below

Explanation:

1.a. 1.0 liter of a 1.0 M mercury (II) chloride (HgCl2) solution

  1.0 L 1 mol 271.49 g

    L        1 L    1 mol

= 271.49 g

= HgCl₂ = 271.49 g HgCl₂

1.b. 2.0 liters of a 1.5 M sodium nitrate (NaNO3) solution

[tex]\frac{2.0 L}{1}[/tex][tex]\frac{1.5 mol}{L}[/tex][tex]\frac{85.01 g}{1 mol}[/tex]

= 255.03 g

= 255 g NaNo₃

1.c. 5.0 liters of a 0.1 M Ca(OH)2 solution

= 37 g Ca(OH)2

1.d. 100 mL of a 0.5 M (NH4)3PO4 solution

= 7.5 g (NH₄)₃PO₄

2. To find the molarity of the following solutions

2.a. 12 g of lithium hydroxide (LiOH) in 1.0 L of solution

= 0.50 m (LiOH)

2.b. 198 g of barium bromide (BaBr2) in 2.0 L of solution

= 0.33 m (BaBr₂)

2.c. 54 g of calcium sulfide (CaS) in 3.0 L of solution

= 0.25 m (CaS)

3. To find the volume of each solution

3.a. 1.0 M solution containing 85 g of silver nitrate (AgNO3)

= 0.50 L (AgNO₃)

3.b. 0.5 M solution containing 250 g of manganese (II) chloride (MnCl2)

= 4.0 L MnCl2

3.c. 0.4 M solution containing 290 g of aluminum nitrate (Al(NO3)3)

= 3.4 L (Al(NO₃)₃)