Ba(OH)₂ + H₂SO₄ → BASO₄ + 2 H₂O is the correct balanced equation for the neutralized of barium hydroxide with sulfuric acid. Therefore, the correct option is option A.
A neutralisation reaction is a chemical process whereby an acid or a base combine to produce water and salt as the end products. H+ ions and OH- ions combine to generate water during a neutralisation reaction. Acid-base neutralisation is the most common type of neutralisation reaction. Ba(OH)₂ + H₂SO₄ → BASO₄ + 2 H₂O is the correct balanced equation for the neutralized of barium hydroxide with sulfuric acid.
Therefore, the correct option is option A.
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A galvanic cell consists of a Mg electrode in a 1 M Mg(NO3)2 solution and another metal electrode X in a 1 M X(NO3)2 solution.
The galvanic cell has an E°cell value of 1.61 V. Which of the following elements fits the identity of X. (Use table table 18.1)
Select one:
a.
Pb
b.
Zn
c.
Ni
d.
Fe
e.
Mn
Answer:
To determine the identity of metal X, we need to compare the standard reduction potentials of the possible metals with the standard reduction potential of the Mg half-reaction.
From Table 18.1, we can find the standard reduction potentials for each of the metals listed:
Pb: -0.13 V
Zn: -0.76 V
Ni: -0.25 V
Fe: -0.44 V
Mn: -1.18 V
The reduction half-reaction for the Mg electrode is:
Mg2+ + 2e- → Mg E° = -2.37 V
The overall reaction for the galvanic cell is:
Mg(s) + X2+(aq) → Mg2+(aq) + X(s)
The standard cell potential is given by:
E°cell = E°(cathode) - E°(anode)
where the cathode is the reduction half-reaction and the anode is the oxidation half-reaction.
Substituting the given values, we get:
1.61 V = E°(X2+/X) - (-2.37 V)
Simplifying, we get:
E°(X2+/X) = 1.61 V + 2.37 V = 3.98 V
Comparing E°(X2+/X) with the standard reduction potentials in Table 18.1, we see that only zinc (Zn) has a reduction potential that is more negative than 3.98 V. Therefore, the metal X is zinc (Zn).
Therefore, the answer is (b) Zn.
Methane gas, CH4, can be produced by the direct combination of the elements at very high temperatures and pressures. If 5.00 L of hydrogen gas at 600°C and 95.0 ATM of pressure is reacted with excess carbon, calculate how many liters of methane at STP would be produced.
Liters of methane at STP would be produced is 13.2L.
To solve this problem, we need to use the combined gas law to convert the initial conditions of hydrogen gas to STP:
Gas laws are a set of physical laws that describe the behavior of gases under various conditions. There are several gas laws, including Boyle's law, Charles's law, Gay-Lussac's law, and the combined gas law.
Boyle's law states that at a constant temperature, the volume of a gas is inversely proportional to its pressure. In other words, as the pressure of a gas increases, its volume decreases, and vice versa.
5.0 atm x 5.00 L x 273 K)/(1 atm x 873 K) = 123.1 L
So we now know that 5.00 L of hydrogen gas at 600°C and 95.0 atm is equivalent to 123.1 L at STP.
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Select the correct answer.
How does a catalyst increase the speed of a reaction?
The catalyst increase the speed of the reaction as it lowers the activation energy.
The catalyst will increases the rate of the reaction as it will lowers the activation energy. The catalyst will increases the rate of the reaction in the both the forward and the backward directions as it providing the alternate pathway with the lower activation energy.
Because of the activation energy is reduced, the more reactants will cross the energy barrier and it will make the rate of the reaction increases. The catalyst is increases the rate of the reaction and without itself undergoes any of the permanent chemical change.
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This question is incomplete, the complete question is :
Select the correct answer.
How does a catalyst increase the speed of a reaction?
It lowers the activation energy.
It increases the activation energy.
Draw the valence bond picture for the formation of the molecule 02.
In the formation of O2 molecule, each oxygen atom has six valence electrons. One of these electrons in each oxygen atom is unpaired.
To complete their octets, they share two electrons and form a double bond between them. This can be represented using a Lewis structure, where each oxygen atom shares two electrons with the other oxygen atom.
The valence bond picture for O2 shows two oxygen atoms with unpaired electrons, each forming a sigma bond by overlapping their 2p orbitals in the region between them. The two unpaired electrons of each oxygen atom then overlap to form a pi bond perpendicular to the plane of the sigma bond. The resulting molecule has a triple bond with a bond order of 2, consisting of one sigma bond and two pi bonds.
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The compound that is not an organic alcohol is:
C 3H 7OH
CH 3CH(OH)CH 3
C 6H 5COOH
(CH 3) 2CHCH(OH)CH 2CH 3
Answer:
The compound that is not an organic alcohol is C6H5COOH.
C3H7OH is propyl alcohol, CH3CH(OH)CH3 is 2-propanol, and (CH3)2CHCH(OH)CH2CH3 is 3-pentanol, all of which are organic alcohols.
On the other hand, C6H5COOH is benzoic acid, which is not an alcohol but an organic acid. It contains a carboxylic acid (-COOH) functional group and not the -OH functional group of alcohols.
Solar and wind energy are both intermittent resources that cannot be relied upon for a constant stream of energy production. Explain why developing better ways to store energy is an important part of making these energy sources more practical to use.
By removing the need to build additional transmission lines and equipment, energy storage may reduce costs for utilities and their customers.
By removing the need to build additional transmission lines and equipment, energy storage may reduce costs for utilities and their customers. Energy storage's inherent ability to offer backup power in the event of grid failure is a feature that both residential consumers and commercial owners find highly desirable.
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What is the difference in energy levels of the sodium atom if emitted light has a wavelength of 589 nm?
The energy levels of a sodium atom are determined by the wavelength of light emitted by it.
A sodium atom's energy levels may be determined using the equation E = hc/, where h is Planck's constant, c is the speed of light, and is the wavelength.
If the wavelength of the emitted light is 589 nm, the energy levels of the sodium atom are E = hc/589nm = 6.626 x 10-34 x 3 x 108/589 x 10-9 = 4.62 x 10-19 J. This is the energy level of the sodium atom when light with a wavelength of 589 nm is emitted.
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A weather balloon is filled with 14.9 L helium at sea level where the pressure is 1.00 atm at 20.0 °C. The balloon bursts after ascending until the pressure is 26.0 torr at -50.0 °C. Determine the volume (in L) at which the balloon bursts.
The volume at which the balloon bursts is 150.7 L.
To solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas.
The combined gas law is expressed as:
(P1 x V1) / (T1) = (P2 x V2) / (T2)
We can convert the initial pressure to torr by multiplying by 760 torr/1 atm, and convert the temperatures to Kelvin by adding 273.15 to the Celsius temperatures.
Substituting the given values into the equation, we get:
(1.00 atm x 14.9 L) / (293.15 K) = [tex](26.0\ torr *V2) / (223.15 K)[/tex]
Solving for V2, we get:
V2 = [tex](1.00\ atm * 14.9 L * 223.15 K) / (293.15 K * 26.0\ torr)[/tex]
= 150.7 L
Therefore, the volume at which the balloon bursts is 150.7 L.
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If HCl, HNO3, and NaOH solutions were prepared at higher concentrations, will it affect the experimental results? Will the change in concentration make the measurement more accurate or less accurate? Please explain your answers in detail.
If HCl, HNO3, and NaOH solutions were prepared at higher concentrations, the change in concentration will make the measurement more accurate.
Concentration in chemistry is calculated by dividing a constituent's abundance by the mixture's total volume. Mass concentration, concentration in moles, numerical concentration, or volume concentration are four different categories of mathematical description.
Any type of chemical mixture can be referred to by the term "concentration," however solvents and solutes in solutions are most usually mentioned. If HCl, HNO3, and NaOH solutions were prepared at higher concentrations, the change in concentration will make the measurement more accurate.
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Which aqueous solution below is the most acidic?
A.) 11.5 B.) 9.2 C.) 6.7 D.) 2.5
HI is the aqueous solution which is the most acidic. Any aqueous solution in chemistry can be divided into one of three groups, including neutral, basic, or acidic solutions.
Any aqueous solution in chemistry can be divided into one of three groups, including neutral, basic, or acidic solutions. Any aqueous solution with a pH 7.0 ([H+] > 1.0 x 10-7 M) is considered an acidic solution.
Water serves as the solvent in an aqueous solution. Solutions that are acidic are sour, whereas alkaline solutions are soapy, thus it's rarely a good idea to try an unfamiliar solution. HI is the aqueous solution which is the most acidic.
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A 5.4 g sample of a metal is heated to 100.0 °C and is placed in a beaker containing 142 g of water at 24.2 °C. The final temperature of the water is 25.1 °C. What is the specific heat of the metal?
Answer:
We can use the principle of conservation of energy to solve this problem. The heat lost by the metal is equal to the heat gained by the water:
Q metal = -Q water
where Q metal is the heat lost by the metal, and Q water is the heat gained by the water.
The heat lost by the metal can be calculated using the formula:
Q metal = m metal * c metal * ΔT metal
where m metal is the mass of the metal, c metal is its specific heat, and ΔT metal is the change in temperature of the metal.
The heat gained by the water can be calculated using the formula:
Q water = m water * c water * ΔT water
where m water is the mass of the water, c water is its specific heat, and ΔT water is the change in temperature of the water.
We know the values of all the variables except c metal, so we can solve for it. We can start by calculating the values of Q metal and Q water:
Q metal = -Q water
m metal * c metal * ΔT metal = -m water * c water * ΔT water
Substituting the given values, we get:
5.4 g * c metal * (100.0 °C - T) = -142 g * 4.18 J/(g*°C) * (T - 24.2 °C)
Simplifying and solving for c metal, we get:
c metal = [142 g * 4.18 J/(g*°C) * (T - 24.2 °C)] / [5.4 g * (100.0 °C - T)]
Multiplying out, we get:
c metal = [593.56 J/(°C) * (T - 24.2 °C)] / [5.4 g * (100.0 °C - T)]
To solve for c metal, we need to find the value of T that satisfies the equation. We can do this by substituting the given value of ΔT water = 0.9 °C into the equation and solving for T:
c metal = [593.56 J/(°C) * (T - 24.2 °C)] / [5.4 g * (100.0 °C - T)]
c metal = [593.56 J/(°C) * (T - 24.2 °C)] / [540 g - 5.4 g * T]
0.9 g * [593.56 J/(°C) * (T - 24.2 °C)] = [540 g - 5.4 g * T] * c metal
535.2044 J/(°C) * (T - 24.2 °C) = 540 g * c metal - 5.4 g * T * c metal
535.2044 J/(°C) * T - 12931.7808 J = 540 g * c metal - 5.4 g * c metal * T
5.4 g * c metal * T + 535.2044 J/(°C) * T = 540 g * c metal + 12931.7808 J
T * (5.4 g * c metal + 535.2044 J/(°C)) = 540 g * c metal + 12931.7808 J
T = [540 g * c metal + 12931.7808 J] / [5.4 g * c metal + 535.2044 J/(°C)]
Substituting the given values, we get:
T = [540 g * c metal + 12931.7808 J] / [5.4 g * c metal + 535.2044 J/(°C)]
T = [540 g * c metal + 12931.7808 J] / [5.4 g * c metal + 535.2044 J/(°C)]
T ≈ 23.3 °C
Therefore, the specific heat of the metal is:
c metal = [142 g * 4.18 J/(g°C) * (T - 24.2 °C)] / [5.4 g * (100.0 °C - T)]
c metal ≈ 0.39 J/(g°C)
So the specific heat of the metal is approximately 0.39 J/(g*°C).
A 5.4 g sample of the metal is heated to the 100.0 °C and is placed in the beaker containing 142 g of the water at 24.2 °C. The specific heat of the metal is 1.322 J/ g °C.
The mass of the metal = 5.4 g
The final temperature = 25.1 °C
The initial temperature = 100 °C
The specific heat capacity of metal = x
The mass of the water = 142 g
The final temperature = 25.1 °C
The initial temperature = 24.2 °C
The specific heat capacity of water = 4.184 J/ g °C
Loss of Heat of Metal = Gain of Heat by Water
-q metal = + q metal
- 5.4 × x × ( 25.1 - 100 ) = 142 × 4.184 ( 25.1 - 24.2 )
404.46 x = 534.71
x = 1.322 J/ g °C
The specific heat capacity of metal is 1.322 J/ g °C.
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Question 14
point)
Helium gas is contained in a tank with a pressure of 14.4 MPa. If the temperature
inside the tank is 24.6 °C and the volume of the tank is 19.4 L, determine the mass,
in grams, of the helium in the tank.
Complete the input-output table for the linear function y = 3x.
x y
-2
-1
0
1
2
3
a=
a
ماس
-3
0
3
b
С
b=
C=
share the imporatant lesson that you have learned in organic chem
We study the reactions that chemists utilise to create bizarre carbon-based structures in organic chemistry.
The study of the makeup, properties, and responses of organic compounds including organic materials, or matter in any of its many forms that contains carbon atoms, is the subject of the branch of science known as organic chemistry. Their structural formula is determined by study of structure.
We will study the reactions that chemists utilise to create bizarre carbon-based structures in organic chemistry, in addition to the analytical techniques used to characterise them. We'll also consider the molecular reaction mechanisms that are driving those reactions.
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PLEASE ANSWER THE MULTIPLE CHOICE QUESTIONS IN THE IMAGE BELOW THIS IS DUE AT 6:00 TODAY
African Americans should take advantage of their power in the labour industry and demand their rights. Therefore, the correct option is option A.
African Americans are a race of Americans who have some or all of their heritage in one of the many black racial groupings of Africa (also known as Black Americans or Americans). The phrase "African American" typically refers to people who were born in the United States but are descended from slaves from Africa.
After White Americans or Hispanic and Latino Americans, African Americans are the third-largest racial and ethnic group in the United States. African Americans should take advantage of their power in the labour industry and demand their rights.
Therefore, the correct option is option A.
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Summarize the main challenges and constraints that engineers must overcome in the design of a low-cost, portable water purification system.
Engineers must take into account the cultural, social, and economic factors that may affect the adoption and sustainability of the system in the target communities.
The main challenges and constraints that engineers must overcome in the design of a low-cost, portable water purification system include:
Designing a water purification system that meets these challenges and constraints requires careful consideration of the materials, technology, and resources available.
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For the equilibrium: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) KC = 10.0
If 1.6 mol of CO and 1.6 mol of water are initially added to a 2.0 liter flask and the flask is then heated
until the system comes to equilibrium, the concentration of hydrogen will then be _______ M
Which statement most likely describes the formation of dunite?
OA. It formed when sediment was cemented together at the bottom of
a lake.
OB. It formed when magma cooled slowly below ground.
OC. It formed when lava cooled quickly aboveground.
OD. It formed when layers of rock deep underground experienced heat
and pressure.
The formation of dunite is most likely to be described by option (B) "It formed when magma cooled slowly below ground."
Dunite is an igneous rock that is composed almost entirely of olivine minerals. It is believed to form from magma that is rich in magnesium and poor in silica.
As the magma cools slowly beneath the Earth's surface, the olivine crystals have time to grow and settle out, forming a rock that is dominated by olivine.
Option (A) is more likely to describe a sedimentary rock, formed by the compaction and cementation of sediment. Option (C) is more likely to describe an extrusive igneous rock, formed from lava that cools quickly above the ground.
Option (D) is more likely to describe the formation of metamorphic rock, which is formed from existing rock that has been subjected to heat and pressure.
Hence Option B, describes the formation of dunite.
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The calculated ΔH reaction will be (too high/ too low/ unaffected), because ΔH reaction is (directly proportional to/ inversely proportional to/ independent of) the value of the heat capacity of the solution.
The calculated ΔH reaction will be unaffected because ΔH reaction is independent of the value of the heat capacity of the solution.
Understanding heat of reactionHeat of reaction is also known as enthalpy of reaction and is defined as the amount of heat energy released or absorbed during a chemical reaction that occurs at constant pressure.
It is the difference between the total enthalpy of the products and the total enthalpy of the reactants, and is usually expressed in units of joules (J) or kilojoules (kJ).
The heat capacity of the solution refers to the amount of heat required to raise the temperature of the solution by a certain amount, whereas ΔH reaction refers to the heat of the chemical reaction itself and is independent of the heat capacity of the solution.
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2c4h10+13o2=8co2+10h2o how many moles of oxygen do you need to react with 0.78 moles of the lighter fluid
The concept stoichiometry is used here to determine the moles of oxygen needed. Stoichiometry is used for the calculation of products and reactants in a chemical reaction. The number of moles of O₂ is
Chemical stoichiometry refers to the quantitative study of the reactants and products involved in a chemical reaction. It is an important concept in chemistry which use the balanced equation to calculate the amounts of reactants and products.
2C₄H₁₀ +13O₂ ⟶ 8CO₂+10H₂O
We want to convert moles of C₄H₁₀ to moles of O₂.
Moles of O₂ = 0.78 mol C₄H₁₀ × 13 mol O₂/2 mol C₄H₁₀ = 5.07 moles
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Calculate the energy in joules and the wavelength in nanometer of the spectra lines produced in the hydrogen spectrum when an electron falls from 4th orbital to the first. Which region of this electromagneric spectrum is in this line?
The concept Rydberg formula is used here to determine the wavelength in nanometer of the spectra lines produced in the hydrogen spectrum when an electron falls from 4th orbital to the first. Here wavelength is -9.72 × 10⁻⁸ m and energy is 12.756 J.
The Rydberg formula is:
1 / λ = RH [ 1 / n₁² - 1 / n₂²]
1 / λ = 1.097 × 10⁷ [ 1 / 4² - 1 / 1² ] = -0.9375
1 / λ = - 10,284,375
λ = -9.72 × 10⁻⁸ m
The energy of hydrogen spectrum is:
Eₙ = -13.606 eV / n²
E₄ = -13.606 / 4² = -0.85
E₁ = -13.606 / 1 = -13.606
E = Eupper - E lower
E = -0.85 - (-13.606) = 12.756 J
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Suppose you heat a metal object with a mass of 34.5 g to 95.5 °C and transfer it to a calorimeter containing 100.0 g of water at 17.5 °C. The water and metal reach a final temperature of 24.9 °C.
Metal in a covered cup with a thermometer and heat indicated as leaving the metal.
What is the specific heat of the metal in J/g⋅∘C
physical proceses? 2. (a). Calculate the maximum work done when the pressure of 10g of hydrogen is reduced from 20atm to 10atm at a constant temperature of 273°K. If the gas behaves ideally, will there be a change in internal energy? Hence determine the value of q in the process.
help for 1 though 7 pls
Answer:
Explanation:
1/ I
2/ III
3/ V
4/ II
5/ IV
6/ 5
7/ 55
Using the formula for the ideal gas law and the value for the gas law constant of 0.08206 L.atm/K/mol, what is the volume (in L) of 9.84 grams of dry hydrogen at 23.4 degrees C and 757 torr?
2. Propane + oxygen yields carbon dioxide and water
Label what type of reaction (synthesis, decomposition, single replacement, double replacement or combustion)
Write the balanced chemical equation
How much propane would you need to produce 1000.0 grams of water?
pleace help i need to do all the work dont splaind just do the work pleace
C[tex]_3[/tex]H[tex]_8[/tex](g) + 5O[tex]_2[/tex] (g) → 3CO[tex]_2[/tex] (g) + 4H[tex]_2[/tex]O(g) is the balanced chemical equation for Propane + oxygen →carbon dioxide +water.
A chemical reaction involves a procedure that causes one group of chemical components to change chemically into another. Chemical bonds among atoms are formed and broken during chemical reactions, which traditionally only involve changes in the locations of electrons.
The study of chemical processes involving unstable and radioactive elements, where both electronic or nuclear changes may take place, is known as nuclear chemistry.
Propane + oxygen →carbon dioxide +water
C[tex]_3[/tex]H[tex]_8[/tex](g) + 5O[tex]_2[/tex] (g) → 3CO[tex]_2[/tex] (g) + 4H[tex]_2[/tex]O(g)
This is a single combustion reaction
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Describes the chemical reaction (s) that produce AMD. Equations
are balanced and formatted to show subscripts.
Pls help I’m so confused
What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 x 10-5.
7.11 × 10⁻⁴ is the solubility (in M) of PbCl[tex]_2[/tex] in a 0.15 M solution of HCl. The Ksp of PbCl[tex]_2[/tex] is 1.6 x 10⁻⁵.
The capability of a material, the solute, to combine with another material, the solvent, is known as solubility in chemistry. Insolubility, or the solute's inability to create such a solution, is the opposite attribute.
The amount of each of the solute within a saturated solution—a solution whereby no more solute is able to be dissolved—is typically used to gauge the degree of a substance's solubility in a particular solvent.
PbCl[tex]_2[/tex] ⇌ Pb[tex]_2[/tex]⁺(x) + 2Cl⁻ (2x)
HCl ⇌H⁺ (0.15M) + Cl⁻ (0.15M)
Ksp = {Pb[tex]_2[/tex]⁺} {Cl⁻}²
Ksp = {x} {2x+ 0.15}²
2x<0.15
Ksp = {x} {0.15}²
x = 7.11 × 10⁻⁴
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3) Sodium azide is an inorganic compound
that decomposes according the following
reaction.
NaN3(s) Na(s) + N2(g)
a) How many grams of N₂ are produced
when 24.0 g sodium azide decomposes with
75.3% yield?
b) Assume that produced N₂ is collected in a
container, and its pressure is suddenly
released from 4.50 atm to 2.60 atm at
25.0°C. How much work, in joules, is done
during this process?
a) 18.2 g of N2 are created when 24.0 g of sodium azide disintegrate with 75.3% yield. The yield of 18.2 g of N2 is obtained by multiplying 24.0 g of sodium azide by 0.753.
b) The formula W = PV may be used to determine how much work was done throughout this operation. Here, the temperature (T) is 25.0°C, the volume change (V) is -1.90 m3, and the pressure (P) is 4.50 atm.
These numbers when entered into the equation result in a work of -7.48 x 105 J. This represents the labour involved in reducing the pressure from 4.50 atm to 2.60 atm.
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Give and proidi the following after and undergoing alpha decay and beta decay
The products of the alpha decay of radium-226 and the beta decay of carbon-14 are radon-222 and nitrogen-14, respectively.
The alpha decay of radium-226 results in the emission of an alpha particle, which is a helium nucleus consisting of two protons and two neutrons.
Therefore, the product of the alpha decay of radium-226 is radon-222:
Ra-226 → Rn-222 + alpha particle
On the other hand, In the case of carbon-14, beta minus decay occurs, in which a neutron is converted into a proton, and an electron and an antineutrino are emitted.
So carbon-14 becomes nitrogen-14:
C-14 → N-14 + beta particle
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--The complete Question is, What is the product of the alpha decay of radium-226 and the beta decay of carbon-14?--
