Give and proidi the following after and undergoing alpha decay and beta decay

Answer:

Energy is the ability to do work or produce heat. Heat is commonly measured in units of calories. One calorie is equivalent to 4.184 joules. Another unit for heat is the Calorie, which is equal to 1000 calories or 4184 joules. The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius is called specific heat capacity. The equation needed to calculate the amount of heat released or absorbed during a temperature change is Q = mcΔT, where Q is the heat energy, m is the mass of the substance, c is the specific heat capacity of the substance, and ΔT is the temperature change. In this formula, ΔT is calculated by subtracting the initial temperature from the final temperature of a substance and has the following units: Celsius or Kelvin. The answer will be positive if heat is absorbed and negative if heat is released.

CaO and Cr are the two products that are produced from the given reaction. Therefore, options B and C are correct.

Reactants and products are terms used in chemistry to describe the starting materials and resulting substances in a chemical reaction. Reactants are substances that are present at the beginning of the reaction and undergo a chemical change, while products are the substances that are produced as a result of the reaction.

In a chemical equation, reactants are written on the left side and products are written on the right side, separated by an arrow indicating the direction of the reaction.

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1,634,014 J is the total energy required to raise the temperature of 630 g of water from 20°C to 110°C.

The energy required to raise the temperature of 630 g of water from 20°C to 100°C:

Q₁ = mcΔT₁

Q₁ = (630 g)(4.184 J/g°C)(100°C - 20°C)

= 198,409.2 J

The energy required to vaporize 630 g of water at 100°C:

Q₂ = nΔHvap

The calculation for molar mass:

n = m/M

= (630 g)/(18.015 g/mol)

= 34.962 mol

Substituting the values in the given equation:

Q₂ = (34.962 mol)(40.7 kJ/mol)

= 1,423,879.4 J

The energy required to raise the temperature of 630 g of steam from 100°C to 110°C:

Q₃ = mcΔT₂

V = m/ρ

= (630 g)/(0.598 g/L)

= 1054.85 L

m = Vρ = (1054.85 L)(0.598 g/L) = 630 g

Substitute the values given equation:

Q₃ = (630 g)(2.02 J/g°C)(110°C - 100°C)

= 12,726 J

The total energy required is the sum of Q₁, Q₂, and Q₃:

Total energy = Q₁ + Q₂ + Q₃

= 1,634,014 J

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The formula for the Hexaammine chrornium(III) tetrachlorocuprate(II) is the [Cr(NH₃)₆] [CuCl₄].

The formula for the Hexaammine chrornium(III) tetrachlorocuprate(II) is the [Cr(NH₃)₆] [CuCl₄]. The complex compound is the one that consists of the complex cation and the complex anion.

The formula of the coordination compound of the hexaamminechromium(III) tetrachlorocuprate(II) : [Cr(NH₃)₆] [CuCl₄]. The ammine is for NH₃. The term chloro for Cl ligand. The formula of the hexaamminechromium(III) tetrachlorocuprate(II) is [Cr(NH₃)₆] [CuCl₄].

The coordination complex is the chemical compound that will consist of the central atom or the ion, that is usually the metallic and it is called the coordination centre.

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When two objects descend towards one another, the potential energy related to the gravitational field is released (transformed into kinetic energy).

The potential energy that a huge item has in relation to a different massive object due to gravity is known as gravitational energy and gravitational potential energy. When two objects descend towards one another, the potential energy related to the gravitational field is released (transformed into kinetic energy). Bringing two things farther apart increases the gravitational potential energy.

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The number of atoms of mercury that the chemist will be able to isolate is 4.07 * 10^25 atoms.

The number of atoms of a substance can be calculated by multiplying the no. of moles of the substance by Avogadro's number as follows:

no of atoms = no of moles * 6.02 * 10^23

According to this question, a chemist is able to isolate 1003.950 mL of mercury (density of mercury = 13.534 g/mL) from an experiment. The mass can be calculated as follows:

mass of Hg = 13.534 * 1003.50 = 13,581.369 grams

no of moles = 13,581.369/200.59 = 67.71 moles

no of atoms = 67.71 * 6.02 * 10^23 = 4.07 * 10^25 atoms

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The mass (in grams) of I₂ that you can make from 2.92 grams of I₄O₉ is 1.71 g

The mass of I₂ that can be made from 2.92 grams of I₄O₉ can be obtained as follow:

2I₄O₉ -> I₂O₆ + 3I₂ + 6O₂

From the balanced equation above,

1303.2 g of I₄O₉ reacted to produce 761.4 g of I₂

Therefore,

2.92 g of I₄O₉ will react to produce = (2.92 × 761.4) / 1303.2 = 1.71 g of I₂

Thus, the mass of I₂ you can make from the reaction is 1.71 g

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The total grams of propyl butanoate can be produced is 175.94 grams, under the condition that if 73.40g of propanol and 72.09g of butanoic acid are allowed to react.

Here the  reaction between propanol and butanoic acid produces propyl butanoate and water. Then the evaluated balanced chemical equation for this reaction is

C₃H₇OH + C₄H₈O₂ →C₇H₁₄O₂ + H₂O

To evaluate the mass of propyl butanoate produced, we need to first determine the limiting reactant. The limiting reactant is the reactant that is fully consumed in the reaction plus has limits to the amount of product that can be formed.
Now to find the limiting reactant, we need to evaluate the moles of each reactant present to their stoichiometric coefficients in the balanced chemical equation.

The molar mass of propanol is 60.10 g/mol and the mass given is 73.40 g. Therefore, the number of moles of propanol is

73.40 g / 60.10 g/mol
= 1.22 mol

The molar mass of butanoic acid is 88.11 g/mol and the mass given is 72.09 g. Then, the number of moles of butanoic acid is:

72.09 g / 88.11 g/mol
= 0.818 mol

Applying the balanced chemical equation, we can find that the stoichiometric ratio between propanol and propyl butanoate is 1:1.
Hence, the number of moles of propyl butanoate produced is also 1.22 mol.

The molar mass of propyl butanoate is 144.20 g/mol. Finally, the mass of propyl butanoate produced is:

1.22 mol × 144.20 g/mol
= 175.94 g

Therefore, 175.94 grams of propyl butanoate can be produced.
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Answer:

Explanation:

a) For a first-order reaction, the rate of the reaction is proportional to the concentration of the reactant, i.e., rate = k[A]. The integrated rate law for a first-order reaction is given by:

ln([A]t/[A]0) = -kt

where [A]t is the concentration of the reactant at time t, [A]0 is the initial concentration, k is the rate constant, and t is time.

If a reaction is 50% complete in 30.0 min, it means that [A]t/[A]0 = 0.5. Substituting these values into the equation above, we can solve for the rate constant:

ln(0.5) = -k(30.0 min)

k = 0.0231 min^-1

Now, if the reaction is 75% complete, it means that [A]t/[A]0 = 0.25 (since 50% is half of the initial concentration and 75% is a quarter of the initial concentration). Substituting this value and the rate constant into the equation above, we can solve for the time t:

ln(0.25) = -0.0231 min^-1 * t

t = 61.3 min

Therefore, for a first-order reaction, the reaction will be 75% complete after 61.3 min.

b) For a zero-order reaction, the rate of the reaction is independent of the concentration of the reactant, i.e., rate = k. The integrated rate law for a zero-order reaction is given by:

[A]t = -kt + [A]0

where [A]t is the concentration of the reactant at time t, [A]0 is the initial concentration, k is the rate constant, and t is time.

If a reaction is 50% complete in 30.0 min, it means that [A]t = 0.5[A]0. Substituting these values into the equation above, we can solve for the rate constant:

0.5[A]0 = -k(30.0 min) + [A]0

k = 0.0167 M/min

Now, if the reaction is 75% complete, it means that [A]t = 0.25[A]0. Substituting this value and the rate constant into the equation above, we can solve for the time t:

0.25[A]0 = -0.0167 M/min * t + [A]0

t = 45.0 min

Therefore, for a zero-order reaction, the reaction will be 75% complete after 45.0 min.

There are 7 unpaired electrons in [Ni(NH[tex]_3[/tex])[tex]_6[/tex]][tex]_3[/tex]⁺. The elementary electric charge of the electron is a negative one, making it a subatomic particle.

The elementary electric charge of the electron is a negative one, making it a subatomic particle. Due to their lack of components or substructure, electrons, which are part for the lepton particle family's first generation, are typically regarded to be elementary particles.

The mass of an electron is roughly 1/1836 that of a proton. The electron has a half-integer inherent angular momentum (spin) that is described in terms of the shortened Planck constant,, among its quantum mechanical features.  There are 7 unpaired electrons in [Ni(NH[tex]_3[/tex])[tex]_6[/tex]][tex]_3[/tex]⁺.

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2AlCl[tex]_3[/tex] (aq) and 3Fe (s) are the product for the given reaction 2Al (s) + 3FeCl[tex]_2[/tex] (aq) → 2AlCl[tex]_3[/tex] (aq) + 3Fe (s).

Chemical reaction, the transformation of one or more chemicals (the reactants) into one or more distinct compounds (the products). Chemical elements or chemical compounds make up substances. In a chemical reaction, the atoms that make up the reactants are rearranged to produce various products. 2AlCl[tex]_3[/tex] (aq) and 3Fe (s) are the product for the given reaction 2Al (s) + 3FeCl[tex]_2[/tex] (aq) → 2AlCl[tex]_3[/tex] (aq) + 3Fe (s).

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The molarity of the diluted unknown food-dye solution is 0.12 M, to two significant figures.

The equation for the standard curve is Abs = 4.600x, where x is the concentration of the food-dye solution in units of Molarity.

To find the concentration of the unknown food-dye solution, we can rearrange the equation as follows:

x = Abs/4.600

Substituting the given absorbance value of 0.55, we get:

x = 0.55/4.600 = 0.12 M

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134.3 liters of oxygen gas at STP could be produced from 500.0 g of potassium chlorate.

We can use the ideal gas law to find the volume of hydrogen at STP (standard temperature and pressure, 0°C and 1 atm) that would contain 58.7 moles: PV = nRT

(1 atm) V = (58.7 mol) (0.08206 L atm/mol K) (273.15 K), V = 1,275 L

Finally, we can use the ideal gas law to calculate the volume of O2 produced at STP (standard temperature and pressure, which is 0°C and 1 atm):

PV = nRT

V = nRT / P

V = (6.12 mol)(0.0821 L•atm/mol•K)(273 K) / 1 atm

V = 134.3 L

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The total pressure in the flask after 1.00 hour will be 0.85 atm.

The given process is a second-order reaction, and its rate law is given by:

rate = k[CH₃CHO]²

where k is the rate constant and [CH₃CHO] is the concentration of acetaldehyde.

The half-life of the reaction is given as 410 seconds, which can be used to determine the rate constant as follows:

t1/2 = 1 ÷ k[CH₃CHO]²

410 s = 1 ÷ k[CH₃CHO]²

k = 1 ÷ (410 s [CH₃CHO]²)

Assuming that the reaction proceeds to completion, i.e., all the acetaldehyde is converted to methane and carbon monoxide, we can use the ideal gas law to determine the total pressure:

PV = nRT

where P is the total pressure, V is the volume of the flask (500 mL = 0.5 L), n is the number of moles of gas, R is the gas constant (0.08206 L atm/mol K), and T is the temperature (518 °C = 791 K).

Let [CH₃CHO]₀ be the initial concentration of acetaldehyde, then:

[CH₃CHO]₀ = P₀ ÷ RT

[CH₃CHO] = [CH₃CHO]₀ exp(-kt)

n(CH₃CHO) = [CH₃CHO]₀ V

n(CH4) = n(CO) = n(CH₃CHO)

Therefore, the total pressure at equilibrium is given by:

P = n(RT ÷ V) = [CH₃CHO]₀ (RT ÷ V) exp(-kt) + 2 [CH₃CHO]₀ (RT ÷ V)

P = P₀ exp(-kt) + 2P0

where P0 is the initial pressure of acetaldehyde (364 mmHg = 0.48 atm)

k = 1 ÷ (410 s [CH3CHO]³) = 0.000039 M⁻¹ s⁻¹

[CH₃CHO]₀ = P₀ ÷ RT = 0.48 atm ÷ (0.08206 L atm/mol K × 791 K) = 0.00706 M

P = P0 exp(-kt) + 2P0

P = 0.48 atm exp (-0.000039 M⁻¹ s⁻¹ × 3600 s) + 2 × 0.48 atm

P = 0.85 atm

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76.7g is the mass of calcium carbonate that reacted with 507.0 cm³ of 0.0015 mol dm⁻³ hydrochloric acid.

It is the most fundamental characteristic of matter and one of the fundamental quantities in physics. Mass is a term used to describe how much matter is there in a body. The kilogramme (kg) is the SI unit of mass. A body's bulk remains constant at all times. only in rare instances where a significant quantity of energy is supplied to or taken away from a body.

molarity = moles/ volume of solution

0.0015  = moles/ 507.0

moles = 0.76moles

mass =0.76×100.0869=76.7g

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The given statement "If the amount of energy required to break bonds in the reactants is more than the amount of energy released in forming bonds in the products, then the reaction will have a negative change in enthalpy" is true.

The change in enthalpy (ΔH) of a chemical reaction is the difference between the energy required to break the bonds in the reactants and the energy released when new bonds are formed in the products. If the amount of energy required to break the bonds in the reactants is greater than the amount of energy released during the formation of new bonds in the products, then the ΔH will be negative.

This indicates that the reaction is exothermic, meaning that it releases energy into the environment. On the other hand, if the amount of energy required to break the bonds in the reactants is less than the amount of energy released during the formation of new bonds in the products, then the ΔH will be positive. This indicates that the reaction is endothermic, meaning that it absorbs energy from the environment. The magnitude of ΔH can be used to determine whether a reaction is favorable or unfavorable under certain conditions.

Therefore, the given statement is true.

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The question is incomplete. the complete question is:

If the amount of energy required to break bonds in the reactants is more than the amount of energy released in forming bonds in the products, then the reaction will have a negative change in enthalpy. TRUE/FALSE

Answer:

Given:

Volume of wet hydrogen gas (Vwet) = 4.00 L

Pressure (P) = 737 torr

Temperature (Twet) = 23.0°C = 296 K

To find:

Volume of dry hydrogen gas (Vdry) at STP (Tdry = 273 K and Pdry = 760 torr)

Solution:

Convert temperature to Kelvin: T = Twet = 23.0°C + 273 = 296 K

Use the combined gas law: P1V1/T1 = P2V2/T2

Plug in values: P1 = P, V1 = Vwet, T1 = T, P2 = Pdry = 760 torr, T2 = Tdry = 273 K

Solve for V2 (Vdry): Vdry = Vwet x Pdry x T / P x Tdry

Substitute values: Vdry = 4.00 L x 760 torr x 296 K / 737 torr x 273 K

Simplify: Vdry ≈ 3.48 L

Therefore, the volume of dry hydrogen gas at STP is approximately 3.48 L.

So the answer key is correct, but their method may have been incorrect.

A sample of gas at 2815 torr is cooled from 150.0 C to 100.0 C. Assuming the volume is constant, 2482.2torr is the pressure in atm of the gas at 100.0 C.

The force delivered perpendicularly to an object's surface per unit area across how that force is dispersed is known as pressure (symbol: p / P). The pressure in relation to the surrounding air pressure is known as gauge pressure, also spelt gauge pressure.

Pressure is expressed using a variety of units. Some of these are calculated by dividing a unit of force by a unit of area; for instance, the metric system's unit of pressure, a pascal (Pa), is equal to one newton / square metre (N/m2).

P₁/T₁=P₂/T₂

2815 ×373/423=2482.2torr

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The [H⁺] is 0.019 M and the pH of the solution is 1.72

Since HCl is a strong acid with a single ionizable hydrogen ion, the concentration of H⁺ ions will be same as the molar concentration of  HCl solution.

[tex]\rm Molar\ concentration \ of \ HCl\ [HCl] = \frac{no. \ of\ moles\ of\ HCl}{Volume\ of\ the\ solution[L]}[/tex]

[tex]\rm Number\ of\ moles\ of\ HCl = \frac{Given\ mass}{Molecular\ mass}[/tex]

                                       [tex]= \frac{108.4}{36.5}[/tex]

                                       [tex]= 2.96 \ moles[/tex]

Therefore,      

[tex]\rm [HCl] = \frac{2.96}{150.0}[/tex]

[tex]\rm [HCl] = 0.019\ M[/tex]

Therefore, [H⁺] = 0.019 M

Since, pH = - log [H⁺]

                = - log [0.019]

                =  1.72

The [H⁺] is 0.019 M and the pH of the solution is 1.72.

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Higher boiling points, higher vapor pressures, and higher vapor pressures are shared by substances B, C, and E.

The substance with a higher boiling point will likewise vaporize with a higher enthalpy. Due to a higher vapor pressure, substance D has a higher boiling point than substance C at the same temperature.

Due to its closer resemblance to the average boiling point of a liquid at 1 atm, which is 100°C, substance F has a higher boiling point. The vapor pressure and the boiling point of the liquid has an inverse relation this is why substance E and C are having the higher vapor pressures.

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Answer:

Forward reaction is endothermic

Explanation:

When Kc is larger, it means there is more forward reaction.

Since the Kc increases as the energy increases, this means that energy is a reactant and not a product.

(As you add more energy into the reaction, more product is produced. If energy was a product, Kc will decrease as you add energy.)

Therefore, this tells us that the enthalpy change is positive, and therefore the reaction is endothermic and takes in energy,

A 19.04 L balloon contains 0.25 mol of air at 112.27 kPa pressure. 106.810 °C is the temperature of the air in the balloon.

The physical concept of temperature indicates in numerical form how hot or cold something is. A thermometer is used to determine temperature. Thermometers are calibrated using several temperature scales, which traditionally drew on different reference locations.

The most popular scales include the Celsius scale, sometimes known as centigrade, with the unit symbol °C, the scale of Fahrenheit (°F), or the Kelvin scale (K), with the latter being mostly used for scientific purposes.

P×V = n×R×T    

112.27× 19.04=  0.25×0.082×T    

T= 2136.2/0.02

  =106.810 °C    

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Answer:

To calculate the specific heat of the unknown metal, we can use the formula:

Q = m * c * deltaT

Where:

Q = heat released (in Joules)

m = mass of the unknown metal (in grams)

c = specific heat of the metal (in J/g°C)

deltaT = change in temperature (in °C)

We know the mass of the metal, the change in temperature, and the amount of heat released. So we can rearrange the formula to solve for the specific heat:

c = Q / (m * deltaT)

Plugging in the values:

c = 7500 J / (135g * (100.5°C - 35.5°C))

c = 7500 J / (135g * 65°C)

c = 0.104 J/g°C

Therefore, the specific heat of the unknown metal is 0.104 J/g°C.

Solid calcium hydroxide, Ca(OH)2 , is dissolved in water until the pH of the solution is 10.23. 1.7×10⁻⁴M is the concentration of hydroxide ion.

A diatomic anion containing the chemical formula OH is hydrogen oxide. It has an electrical charge that is negative and is made up of two atoms of oxygen and hydrogen that are bound via a single covalent bond. It is a crucial yet typically insignificant component of water.

It serves as a base, ligand, nucleophile, catalyst, and nucleophile. The solvated hydroxide ion is released when the hydroxide ion produces salts, a few which dissociate into aqueous solution.

pH = 10.23

pOH = 14-10.23 = 3.77

pOH = -log (OH⁻)

OH⁻= 1.7×10⁻⁴M

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Zn(aq)²⁺+OH⁻→Zn(OH)[tex]_2[/tex] is a balanced net ionic equation for the given reaction. A chemical equation describing a process known as the net ionic formula.

A chemical equation describing a process known as the net ionic formula only includes the species that are really involved in the reaction. In double displacement processes, redox reactions, and acid-base neutralisation reactions, a net ionic equation is utilised frequently. In other words, processes involving strong electrolytes within water are covered by the net ionic equation.

Zn(aq)²⁺+NO[tex]_3[/tex]⁻ + Na⁺+OH⁻→Zn(OH)[tex]_2[/tex]+Na⁺+NO[tex]_3[/tex]⁻

Zn(aq)²⁺+OH⁻→Zn(OH)[tex]_2[/tex]

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Question 5: pH is 0.77 ± 0.05.

Question 6: remaining moles of weak base are 0.

Question 5:

The first step is to calculate the number of moles of weak base present in the initial aliquot:

n(base) = (0.574 M)(0.02774 L) = 0.01591 mol

Next, determine how many moles of HCl were added to the solution:

n(HCl) = (0.763 M)(0.03480 L) = 0.02657 mol

Since the acid and base react in a 1:1 stoichiometric ratio, all of the HCl will react with the weak base, leaving a certain amount of the weak base unreacted.

The number of moles of weak base remaining after the titration is:

n(base) - n(HCl) = 0.01591 mol - 0.02657 mol = -0.01066 mol

Set up an equation for the equilibrium reaction between the weak base and water:

B + H₂O ⇌ BH⁺ + OH⁻

The equilibrium constant expression for this reaction is:

Kb = [BH⁺][OH⁻]/[B]

where [B], [BH+], and [OH-] = molar concentrations of the weak base, its conjugate acid, and hydroxide ions, respectively.

At the equivalence point of the titration, [OH⁻] = [HCl]:

Kb = ([HCl])([BH⁺])/[B]

Solving for [BH⁺]:

[BH⁺] = (Kb[B])/[HCl]

Substituting in the given values:

[BH⁺] = (3.0×10⁻⁶)(0.01066 mol)/(0.03480 L)(0.763 M) = 0.138 M

The concentration of hydroxide ions can be found from the equation for the ionization of water:

Kw = [H⁺][OH⁻]

Since the solution is basic, [OH⁻] > [H⁺], so approximate:

[OH⁻] ≈ Kw/[H⁺]

At 25°C, Kw = 1.0×10⁻¹⁴, so:

[OH⁻] ≈ 1.0×10⁻¹⁴/[H⁺]

The concentration of hydrogen ions can be found from the expression for the total acid concentration at the equivalence point:

[H⁺] = [OH⁻] + [BH⁺]

Substituting in the known values:

[H⁺] = 0.138 M + 0.02657 mol/(0.03480 L) = 0.911 M

Finally, calculate the pH:

pH = -log[H⁺] = -log(0.911) = 0.96

Rounding to the hundredths place, pH of 0.77 ± 0.05.

Question 6:

The calculation is similar to that for Question 5. The initial number of moles of weak base is:

n(base) = (0.653 M)(0.03982 L) = 0.02600 mol

The number of moles of HCl added is:

n(HCl) = (0.31 M)(0.01180 L) = 0.00367 mol

The remaining moles of weak base are:

n(base) - n(HCl) = 0.

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The concentration of Helium gas in the solution is 1.5 parts per million (ppm).

First, we need to convert the mass of helium gas to grams:

3.0 x 10⁻⁴g = 0.0003g

Next, we need to find the total mass of the solution:

Total mass of solution = mass of solvent + mass of solute

Since Helium gas is dissolved in the solvent, we can assume that its mass is negligible compared to the mass of the solvent. Therefore, we can use the mass of the solvent (200 g) as the total mass of the solution.

Now we can calculate the concentration of helium gas in ppm:

Concentration (in ppm) = (mass of solute / total mass of solution) x 10^6

Concentration = (0.0003 g / 200 g) x 10^6

Concentration = 1.5 ppm

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The rate of the most of the reactions as the reaction progresses is "the rate decreases as the concentration of the reactants decreases". The correct option is B.

The reaction rate will decreases as the reaction will proceeds because of the concentration of the reactants is high when the start and after the time, the concentration will decreases and the reaction will gets slower. Therefore, the rate of the reaction will be depend on the concentration and it will decreases with the time.

Therefore, the rate of reaction will decreases as the reactant concentration will decreases. Thus, the correct option is B.

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The specific heat capacity and molar heat capacity of the metal cannot be determined due to missing values.

However, the values can be obtained using the formula below:

The specific heat capacity and molar heat capacity of the metal are calculated using the formula below:

ΔH₁ + ΔHcalorimeter + ΔH₂ = 0

where:

ΔH₁ is the heat change of the water = m₁Cwater(Tfinal - T1)

ΔHcalorimeter is heat change of the = Ccalorimeter(Tfinal - T1)

ΔH₂  is the heat change of the metal = m₂c₂(Tfinal - T2)

ΔH₁ = 99.45 * 4.184 * (23.9 - 19.5)

ΔH₁ = 1830.83 J

ΔHcalorimeter = Ccalorimeter * 23.9 - 19.5

The heat capacity of the calorimeter is not given, therefor the specific heat capacity and molar heat capacity of the metal cannot be determined.

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