What mass (grams) of silver oxide would you need to decompose in order to produce 120.6 grams of silver?

Ag2O --> Ag + O2

a. We will be able to release 37,827 kJ. b. You can cook a maximum of 19 hamburgers without exceeding the limit of 0.750 kg of carbon dioxide.

a. We need to use the balanced chemical equation and the enthalpy change of the reaction.

Therefore, moles  [tex]CO_2[/tex] produced are[tex]0.750 kg / 44.01 g/mol = 17.03 mol.[/tex]

The enthalpy change of the reaction is -2220.1 kJ/mol. Thus, the maximum number of kilojoules that can be released is:

[tex]\Delta Hrxn * moles of[/tex] [tex]CO_2[/tex] = [tex]-2220.1 kJ/mol * 17.03 mol = -37,827 kJ[/tex]

We need to reverse the sign of the answer, giving us 37,827 kJ.

b. If it requires 1900 kJ to cook one hamburger, we can divide the maximum number of kilojoules that can be released by the energy required to cook one hamburger:

37,827 kJ / 1900 kJ/hamburger = 19.91 hamburgers

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Here are some questions on Personal Care services on E2020 are:

An infection is the entrance and growth of dangerous microorganisms in the body that harm the host, such as bacteria, viruses, fungus, or parasites.

Infections can be systemic (affecting the entire body) or localized (affecting a particular area of the body), and they can be moderate to severe.

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The mass of Fe₂O₃ produced is 101.9 g.

The balanced chemical equation for the combustion of iron pyrite is:

4FeS₂(s) + 11O₂(g) → 2Fe₂O3(s) + 8SO₂(g)

From the equation, 11 moles of oxygen are required to produce 2 moles of Fe₂O₃. Convert the given volume of oxygen to moles:

n(O2) = PV/RT = (2.97 atm)(74 L)/(0.0821 L·atm/mol·K)(161 + 273 K) = 3.51 mol

Since the reaction requires 11 moles of O₂ for every 2 moles of Fe₂O₃, calculate the moles of Fe₂O₃ produced:

n(Fe₂O₃) = (2/11) × n(O₂) = (2/11) × 3.51 mol = 0.638 mol

Finally, use the molar mass of Fe₂O₃ to convert moles to grams:

m(Fe₂O₃) = n(Fe₂O₃) × M(Fe₂O₃) = 0.638 mol × 159.69 g/mol = 101.9 g

Therefore, the mass of Fe₂O₃ produced is 101.9 g.

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A zinc chloride solution is prepared by dissolving 0.316 g of anhydrous zinc chloride in 100.0 mL of [tex]H_2O[/tex] . The mass of zinc chloride present in 19.97 mL of the solution is  0.316 g.

We can use the formula:

C1V1 = C2V2

where C1 is the concentration of the original solution, V1 is the volume of the original solution, C2 is the concentration of the final solution, and V2 is the volume of the final solution.

First, let's calculate the concentration of the original solution:

concentration = (0.316 g) / (100.0 mL) = 0.00316 g/mL

Now, we can use the formula to find the mass of zinc chloride in 19.97 mL of the solution:

C1V1 = C2V2

0.00316 g/mL x 100.0 mL = C2 x 19.97 mL

C2 = (0.00316 g/mL x 100.0 mL) / 19.97 mL

C2 = 0.01583 g/mL

So the concentration of zinc chloride in the final solution is 0.01583 g/mL.

Now we can use this concentration to calculate the mass of zinc chloride in 19.97 mL of the solution:

mass = concentration x volume

mass = 0.01583 g/mL x 19.97 mL

mass = 0.316 g

Therefore, there are 0.316 g of zinc chloride present in 19.97 mL of the solution.

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The partial pressure of the Helium gas is  0.9 atm.

The pressure that a gas exerts on its own when it is collected over water, independent of the pressure that the water vapor in the collecting vessel also produces, is known as its partial pressure.

When gas is collected over water, some of the water vapor will dissolve in it and change the overall pressure in the collecting vessel. Water vapor has its own partial pressure, which is affected by the relative humidity and temperature of the air around it. This is why it behaves in this way.

We have that;

Vapor pressure of the gas = 19.8 mmHg or 0.026 atm

Partial pressure of the Helium gas = 0.926 atm - 0.026 atm

= 0.9 atm

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There are approximately 223.2 grams of oxygen in 615 grams of N2O.

To find the number of grams of O in 615g of N2O, we first need to understand the chemical formula of N2O. N2O is a compound made up of two nitrogen atoms (N) and one oxygen atom (O). Therefore, the molecular weight of N2O would be:
(2 x atomic weight of N) + (1 x atomic weight of O)
= (2 x 14.01 g/mol) + (1 x 16.00 g/mol)
= 44.01 g/mol
Now, to calculate the number of grams of O in 615g of N2O, we need to know the proportion of O in the compound. Since there is only one oxygen atom in each molecule of N2O, we can find the proportion of O by dividing the atomic weight of O by the molecular weight of N2O:
Atomic weight of O / Molecular weight of N2O
= 16.00 g/mol / 44.01 g/mol
= 0.363
This means that oxygen makes up 36.3% of the total weight of N2O. To find the number of grams of O in 615g of N2O, we can multiply the total weight by the proportion of O:
615g x 0.363
= 223.2g

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C₂H₄O₂ + NaHCO₃ —> NaC₂H₃O₂ + H₂O + CO₂ the amount of Carbon dioxide produced is 5.28 mg.

Water, CO₂ , and C₂H₃NaO₂ were produced when acetic acid and NaHCO₃ were combined. The chemistry is as follows: The reaction between vinegar and baking soda was endothermic.

Acetic acid:  2(12.01 g/mol) + 4(1.01 g/mol) + 2(16.00 g/mol)

                                              = 60.05 g/mol

NaHCO₃ 22.99 g/mol + 1.01 g/mol + 3(16.00 g/mol)

                                             = 84.01 g/mol

100 mg of Acetic acid is equal to 0.1 g, and 10 mg of NaHCO₃ is equal to 0.01 g.

Number of moles of Acetic acid = 0.1 g / 60.05 g/mol

                                             = 0.00167 mol

Number of moles of NaHCO₃  = 0.01 g / 84.01 g/mol

                                               = 0.00012 mol

Since NaHCO₃ has fewer moles, it is the limiting reactant.

Therefore, 0.00012 mol of NaHCO₃  will produce 0.00012 mol of CO₂

The mass of CO₂ produced can be calculated as follows:

Mass of CO₂ = Number of moles of CO₂  x Molar mass of CO₂

Mass of CO₂ = 0.00012 mol x 44.01 g/mol

                             = 0.00528 g or 5.28 mg

Therefore, the amount of CO₂ produced is 5.28 mg.

The theoretical yield of CO₂ is 0.00012 mol x 44.01 g/mol

                               = 0.00528 g or 5.28 mg.

This is equal to the actual yield of CO₂ produced.

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Mark would need a thermometer to determine the temperature change of a solution during a chemical reaction. A thermometer is a tool used to measure temperature and can be used to monitor and record changes in temperature during a chemical reaction. So the answer is thermometer .

There are different types of thermometers, such as liquid-in-glass thermometers, bimetallic strip thermometers, digital thermometers, and infrared thermometers, among others. The choice of thermometer depends on the specific requirements of the experiment or process being carried out.

By measuring the initial and final temperatures of the solution before and after the chemical reaction, Mark can determine the temperature change, which is an important parameter in many chemical reactions as it provides information about the heat energy involved in the reaction, and helps in understanding the thermodynamics and kinetics of the process. Therefore the answer is thermometer .

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1. The star that has a temperature of approximately 9000 K and luminosity about 20 times greater than the Sun’s luminosity is Vega.

2. The type of star that is considered part of the main sequence is red dwarfs.

3. The star that is cooler than the Sun is Barnard’s Star.

4. The Sun is classified as a main sequence star.

5. The force most responsible for the formation of stars is gravity.

6. The star that has a higher luminosity and a lower temperature than the Sun is Aldebaran.

7. Compared to the temperature and luminosity of the star Polaris, the star Sirius is hotter and more luminous.

Answer: As they develop theories, chemists use models to attempt to explain their findings. Chemists assess the model they are using as new evidence becomes available and, if required, continue to refine it by making modifications.

Explanation:

The equilibrium constant for the reaction at 655 K is [tex]e^{6.96}[/tex] ≈ 1.05 × 10^3.

The equilibrium constant (K) for a reaction is related to the change in Gibbs free energy (ΔG) through the equation:

ΔG = -RTlnK

where R is the gas constant, T is the temperature in kelvin, and ln is the natural logarithm. Since ΔG and ΔH (the change in enthalpy) are related by the equation:

ΔG = ΔH - TΔS

where ΔS is the change in entropy, we can rearrange the first equation to get:

lnK = -ΔH ÷ RT + ΔS ÷ R

At 298 K, we can use the given values of ΔH and K to solve for ΔS:

lnK = -ΔH ÷ RT + ΔS ÷ R

ln(1.4 × 10³) = (-(-25.8 × 10³ J/mol) ÷ (8.314 J/mol K × 298 K)) + ΔS ÷ 8.314 J/mol K

ΔS = 78.2 J/mol K

Now we can use the equation above to solve for lnK at 655 K, using the same value of ΔH and the newly calculated value of ΔS:

lnK = -ΔH ÷ RT + ΔS ÷ R

lnK = -(-25.8 × 10³ J/mol) ÷ (8.314 J/mol K × 655 K) + (78.2 J/mol K) ÷ 8.314 J/mol K

lnK = 6.96

e ≈ 1.05 × 10³

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Answer:

If an atom loses or gains electrons, it will become a positively or negatively charged particle, called an ion. The loss of one or more electrons results in more protons than electrons and an overall positively charged ion, called a cation.

Hope it helped! :)

The pressure of the gas in the smaller flask at the new temperature is approximately 168.5 mm Hg.

To solve this problem, we can use the combined gas law equation, which relates the initial and final states of a gas sample undergoing changes in pressure, volume, and temperature. The equation is:
[tex]P_1V_1/T_1 = P_2V_2/T_2[/tex]

where [tex]P_1[/tex] and [tex]P_2[/tex] are the initial pressure and final pressure, [tex]V_1[/tex] and [tex]V_2[/tex] are the initial and final volumes, and [tex]T_1[/tex] and [tex]T_2[/tex] are the initial and final temperatures in Kelvin.

[tex]V_1[/tex] = 245 mL
[tex]T_1[/tex] = 23.5°C + 273.15 = 296.65 K
[tex]P_1[/tex] = 37.8 mm Hg
[tex]V_2[/tex] = 54 mL
[tex]T_2[/tex] = 0°C (ice water) + 273.15 = 273.15 K

We need to find [tex]P_2[/tex] . Plug the given values into the equation and solve for [tex]P_2[/tex] :
(37.8 mm Hg * 245 mL) / 296.65 K = (P2 * 54 mL) / 273.15 K

Rearrange the equation to isolate [tex]P_2[/tex] :
[tex]P_2[/tex] = (37.8 mm Hg * 245 mL * 273.15 K) / (296.65 K * 54 mL)
[tex]P_2[/tex] ≈ 168.5 mm Hg
So, the pressure of the gas is approximately 168.5 mm Hg in the smaller flask at the new temperature.

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Answer:

7. C. 2326 J

8. B

Explanation:

7. Use the equation q=m*c* change in temp, where m is mass, c is specific heat capacity.

q= 68 g* (0.9 J/g*c) * (93-55) C

q= 2326 J

8. An exothermic reaction is characterized by a negative delta H (change in enthalpy) since energy is released during the reaction. B is the only choice with a negative delta H.

The pH of the solution is 5.72, which is slightly acidic.

pH is a measure of the acidity or basicity of a solution. It is defined as the negative logarithm of the hydrogen ion concentration (H+) in a solution. The pH scale ranges from 0 to 14, where a pH of 7 is neutral, pH below 7 is acidic, and pH above 7 is basic. The formula to calculate pH is pH = -log[H+], where [H+] represents the concentration of hydrogen ions in moles per liter.
Given the H+ concentration of 1.9x10-6, we can calculate the pH of the solution as follows:
pH = -log(1.9x10-6) = 5.72
It is important to note that pH is an important factor in various chemical and biological processes. It can affect the solubility of certain substances, enzymatic activity, and the growth and survival of living organisms. Maintaining the appropriate pH is crucial for the proper functioning of these processes.

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Answer: C

Explanation:

Answer: C

Explanation:

Answer:

Water can dissolve many substances because it has a partial charge on each side of its molecules.

Explanation:

Water is a polar molecule, meaning that it has an uneven distribution of electrons between its hydrogen and oxygen atoms. This creates a partial negative charge on the oxygen side of the molecule and a partial positive charge on the hydrogen side. These partial charges allow water molecules to attract and surround other charged or polar molecules, such as ions and polar compounds, and separate them from each other. This process of surrounding and separating other substances in a solution is known as hydration or dissolution, and it is what allows water to dissolve many substances. Therefore, the correct option is: "it has a partial charge on each side of its molecules."

Answer:

5. 0.566 g
6. A. 100 times more

Explanation:

5. The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration. For a solution with pH=2, the concentration of hydrogen ions is 10^-2 mol/L. Since HBr is a strong acid, it dissociates completely in water to produce H+ and Br- ions. Therefore, the concentration of HBr in the solution is also 10^-2 mol/L.

The molar mass of HBr is 80.91194 g/mol

So, in a 700 mL solution (0.7 L), there are

0.7 L * 10^-2 mol/L = 0.007 mol of HBr.

This corresponds to 0.007 mol * 80.91194 g/mol = 0.566 g of HBr dissolved in the solution.

6. The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration. This means that for each decrease in pH by 1 unit, the hydrogen ion concentration increases by a factor of 10. Since the difference in pH between the two solutions is 3 units (6-3=3), the hydrogen ion concentration in the solution with pH=3 is 10^3 = 100 times more than in the solution with pH=6.

The Lewis structure of the compound[tex]CH_{3} Br[/tex] is shown in the image attached.

The Lewis structure of a molecule or ion is produced by arranging the atoms in a manner that lessens the attraction between their valence electron pairs and then distributes the valence electrons among the atoms to form covalent bonds.

The octet rule, which states that atoms normally gain or lose electrons to obtain a stable configuration with eight valence electrons, frequently serves as a guidance when arranging electrons in the Lewis structure.

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We can use the formula:

Q = mcΔT

where Q is the heat absorbed or released, m is the mass, c is the specific heat, and ΔT is the change in temperature.

First, let's calculate the heat absorbed by the crown:

Q1 = mcΔT

Q1 = (1130 g)(0.129 J/g C)(98.8 C - 25.83 C)

Q1 = 107,776.6 J

Next, let's calculate the heat released by the crown into the water:

Q2 = mcΔT

Q2 = (m)(c)(ΔT)

Q2 = (1340 g)(4.184 J/g C)(27.84 C - 25.83 C)

Q2 = 11096.64 J

Since Q1 = -Q2 (heat lost by the crown is equal to heat gained by the water),

mcΔT = -mcΔT

We can then solve for the specific heat of the crown:

c = -(Q2/mΔT)

c = -(11096.64 J)/(1130 g)(27.84 C - 25.83 C)

c = 0.131 J/g C

The specific heat of pure gold is 0.129 J/g C, and the specific heat of the crown is 0.131 J/g C. Since the specific heat of the crown is slightly higher than that of pure gold, it is possible that the crown is not pure gold. However, other factors such as impurities or alloying metals can also affect the specific heat, so further analysis would be necessary to confirm if the crown is pure gold.

Answer:

1.02 J/g°C.

Explanation:

We can use the equation:

q = m * c * ΔT

where q is the heat absorbed or released, m is the mass of the substance (in grams), c is the specific heat, and ΔT is the change in temperature (in Celsius).

First, we can calculate the heat gained by the water:

q_water = m_water * c_water * ΔT_water

where m_water is the mass of the water (in grams), c_water is the specific heat of water (4.184 J/g°C), and ΔT_water is the change in temperature of the water.

m_water = 120 g

c_water = 4.184 J/g°C

ΔT_water = (32°C - 24°C) = 8°C

q_water = (120 g) * (4.184 J/g°C) * (8°C) = 4009 J

This means that the heat lost by the unknown solid is equal to the heat gained by the water:

q_solid = -q_water

q_solid = -4009 J

Next, we can calculate the change in temperature of the solid:

ΔT_solid = (32°C - 80°C) = -48°C

Now, we can solve for the specific heat of the solid:

q_solid = m_solid * c_solid * ΔT_solid

-4009 J = (90.0 g) * c_solid * (-48°C)

c_solid = -4009 J / (90.0 g * -48°C)

c_solid = 1.02 J/g°C

Therefore, the specific heat of the unknown solid is 1.02 J/g°C.

_______________________________

2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g)

Moles of NA = Given Mass (g) ÷ Molecular Mass (g/mol)

= 27.5 ÷ 22.9897

= 1.196 mol

Moles of H2 Produced = Mol of NA × 1 mol H2 ÷ 2 Mol NA

= 1.196 × 1 ÷ 2

= 0.60 mol

Number of Molecules = Moles × Avogadro's Number

= 0.60 × 6.023 × 10²³ mol - 1

= 3.61 × 10²³

The Number of Molecules of Hydrogen Gas Produced When Added To Water Is 3.61 × 10²³

_________________________________

The information given can be used to construct the empirical formula for a tin oxide. We must first determine the mass of tin in the sample. This may be achieved by deducting the mass of the crucible, cover, and sample (21.76 g) from the mass of the empty crucible and cover (19.66 g).

This gives us a mass of 2.10 g of tin in the sample. The mass of oxygen in the sample must then be determined. To achieve this, we must deduct the mass of the crucible, cover, and sample (21.76 g) from the mass of the same components (22.29 g) prior to protracted heating. This provides us with an oxygen mass of 0.53 g.

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We need to carry at least 187 CCCs on board the space shuttle to absorb all the CO2 produced by the crew during the 18-day mission.

To solve this problem, we need to use the following information:

First, we need to calculate the total amount of CO2 that will be expelled during the mission:

Total CO2 = 6 crew members x 42.0 g CO2/hour x 24 hours/day x 18 days = 136,080 g CO2

Next, we need to calculate the amount of LIOH needed to absorb this CO2. The balanced chemical equation for the reaction between CO2 and LIOH is:

CO2 + 2 LIOH → Li2CO3 + H2O

The molar mass of CO2 is 44.01 g/mol, and the molar mass of LIOH is 23.95 g/mol.

This means that 2 moles of LIOH are needed to absorb 1 mole of CO2.

So, to absorb 136,080 g of CO2, we need:

136,080 g CO2 x (1 mol CO2/44.01 g) x (2 mol LIOH/1 mol CO2) x (23.95 g LIOH/1 mol) = 139,648 g LIOH

Since each CCC contains 750 g of LIOH, we need:

139,648 g LIOH / 750 g CCC = 186.2 CCCs

Therefore, we need to carry at least 187 CCCs on board the space shuttle to absorb all the CO2 produced by the crew during the 18-day mission.

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To calculate the mass of KOH needed to make a 5 M solution in 185.5 mL, we need to use the formula:

mass = moles × molar mass

where moles is the amount of KOH in moles and molar mass is the mass of one mole of KOH.

We can calculate the moles of KOH as follows:

moles = Molarity × Volume (in liters)

First, we need to convert the volume from milliliters to liters:

185.5 mL = 0.1855 L

Now we can calculate the moles of KOH:

moles = 5 M × 0.1855 L = 0.9275 moles

The molar mass of KOH is 56.11 g/mol. Therefore, the mass of KOH needed is:

mass = 0.9275 moles × 56.11 g/mol = 52.05 g

Therefore, 52.05 grams of KOH are needed to make a 5 M solution in 185.5 mL.

The number is converted to 60. 2 × 10²²

Index forms are simply described as mathematical forms that are used in the representation of numbers that are too small or too large in more convenient forms.

These index forms are also referred to as scientific notation or standard forms.

Some rules of index forms are;

From the information given, we have that;

0. 0602 × 10 ²⁵

Subtract three from the exponent value and move three spaces right, we have;

60. 2 × 10²⁵⁻³

60. 2 × 10²²

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CH₃CHCl₂COOH is 2,2-dichloropropanoic acid, with the least pH, option (c) is correct.

pH is a measure of the acidity or basicity of a solution. A lower pH indicates a higher acidity. Acidity is due to the presence of hydrogen ions (H⁺) in a solution. The more the concentration of H⁺, the lower the pH. CH₃CH₂COOH is propanoic acid, which has a pH of around 4.9.

CH₂ClCH₂COOH is 2-chloropropanoic acid, which has a pH of around 2.8 due to the electron-withdrawing effect of the chlorine atom. CH₃CH₂CH₂COOH is butanoic acid, which has a pH of around 4.8. Thus, CH₃CHCl₂COOH is 2,2-dichloropropanoic acid, which has the least pH among the given options, around 1.5 due to the presence of two electron-withdrawing chlorine atoms, option (c) is correct.

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The alpha decay of radon is shown by;

222/86Rn ----> 218/84Po + 4/2He

Radon undergoes alpha decay by emitting an alpha particle, which consists of two protons and two neutrons.

Let us note that when there is an alpha decay, the parent nucleus would loose a helium nucleus and the daughter nucleus would less than than the parent in mass by four units and less than the parent in charge by 2 units and this would satisfy the mass and charge balance of the equation. The decay equation is; 222/86Rn ----> 218/84Po + 4/2He

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Missing parts;

Use the equation to complete the activity.

219 86Rn → 215 84Po + a

The nuclear equation shows the transmutation of a form of radon into polonium and an alpha particle. In one to two sentences, explain whether or not the reaction is balanced.

The total mass of products obtained when 130 g of zinc react completely with HCl is 274 g (3rd option)

First, we shall determine the mass of each product obtained. Details below:

For ZnCl₂

2HCl + Zn -> ZnCl₂ + H₂

From the balanced equation above,

65 g of Zn reacted to produce 135 g of ZnCl₂

Therefore,

130 g of Zn will react to produce = (130 × 135) / 65 = 270 g of ZnCl₂

Thus, the mass of ZnCl₂ obtained is 270 g

For H₂

2HCl + Zn -> ZnCl₂ + H₂

From the balanced equation above,

65 g of Zn reacted to produce 2 g of H₂

Therefore,

130 g of Zn will react to produce = (130 × 2) / 65 = 4 g of H₂

Thus, the mass of H₂ obtained is 4 g

Finally, we shall determine the total mass of the product produced. Details below:

Total mass of product = mass of ZnCl₂ + mass of H₂

Total mass of product = 270 + 4

Total mass of product = 274 g (3rd option)

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