Be sure to answer all parts. The percent by mass of bicarbonate (HCO3−) in a certain Alka-Seltzer product is 32.5 percent. Calculate the volume of CO2 generated (in mL) at 37°C and 1.00 atm if a person were to accidentally ingest a 3.79-g tablet without following instructions. (Hint: The reaction occurs between HCO3− and HCl acid in the stomach.)

Answer:

A) it produces a relatively small fraction of the maximum number of possible hydronium ions.

Explanation:

A weak acid is one that ionizes slightly in aqueous solutions. They set up an equilibrium in the process. Weak acids like hydrocyanic acid only gives a very small fraction of the possible hydronium ions they ought to give in solution. They are not capable of ionizing completely like the strong acids. This makes hydrocyanic acid a weak electrolyte.

"The correct answer is A) it produces a relatively small fraction of the maximum number of possible hydronium ions. The correct statement about hydrocyanic acid is that it produces a relatively small fraction of the maximum number of possible hydronium ions when dissolved in water, which aligns with option A.

Hydrocyanic acid (HCN) is indeed classified as a weak acid in water. The classification of an acid as weak or strong is based on its ability to dissociate in water. A weak acid, such as hydrocyanic acid, only partially dissociates into its ions when dissolved in water. This means that only a small fraction of the HCN molecules ionize to release hydronium ions (H3O+) and cyanide ions (CN-).

In contrast, a strong acid would dissociate completely, producing the maximum number of hydronium ions possible from the acid. For example, hydrochloric acid (HCl) is a strong acid that dissociates completely in water to form H3O+ and Cl- ions.

The degree of dissociation of a weak acid is described by its acid dissociation constant (Ka), which is a measure of the strength of the acid in solution. The Ka value for hydrocyanic acid is relatively small, indicating that the equilibrium lies more towards the reactant side (undissociated HCN) rather than the product side (H3O+ and CN-).

Therefore, the correct statement about hydrocyanic acid is that it produces a relatively small fraction of the maximum number of possible hydronium ions when dissolved in water, which aligns with option A."

Answer:

The answer is A.

Hope this helps!

Two or more than two atoms with different physical or chemical properties can not combine together to form an element. Therefore, the correct option is option A that is isotopes.

Element generally consist of atoms or we can atoms combine to form element. Atoms of an element is always same, means all the properties of all atoms of one type of element is same.

Isotope refers to each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in atomic mass but not in chemical properties. Isotopes of hydrogen are Protium, Deuterium and Tritium with atomic number 1 and mass number1,2 and  respectively.

Therefore, the correct option is option A that is isotopes.

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Answer:

addition of a neutron

Explanation:

Nuclear fission is a radioactive decay process in which a heavy nucleus spontaneously disintegrates into lighter ones accompanied by the release of energy.

An atom whose neutron/proton ratio is the same as that of the stability ratio of that atom is said to be stable. When such an atom is bombarded with a neutron particle, the stability ratio is offset. What results is a radioactive decay of such a nucleus. This form of decay is a nuclear fission.

A series of chain reaction is produced though this until the stability ratio is reached.

Answer: 0.14 Liters

Explanation:

[tex]Q=I\times t[/tex]

where Q= quantity of electricity in coloumbs

I = current in amperes = 1.45 A

t= time in seconds = 13 min=[tex]13\times 60 =780s[/tex]

[tex]Q=1.45A\times 780s=1131C[/tex]

[tex]HNO_3\rightarrow H^++NO_3^-[/tex]

[tex]2H^++2e^-\rightarrow H_2[/tex]

[tex]96500\times 2=193000Coloumb[/tex] of electricity deposits  1 mole of [tex]H_2[/tex]

1131 C of electricity deposits =[tex]\frac{1}{193000}\times 1131=5.86\times 10^{-3}moles[/tex] of [tex]H_2[/tex]

According to the ideal gas equation:'

[tex]PV=nRT[/tex]

P = Pressure of the gas = 1.03 atm

V= Volume of the gas = ?

T= Temperature of the gas = 25°C = 298 K       (0°C = 273 K)

R= Gas constant = 0.0821 atmL/K mol

n=  moles of gas= [tex]5.86\times 10^{-3}moles[/tex]

[tex]V=\frac{nRT}{P}=\frac{5.86\times 10^{-3}\times 0.0821\times 298}{1.03}=0.14L[/tex]

Thus the volume of hydrogen gas at [tex]25^0C[/tex] and 1.03 atm will be 0.14 Liters.

To calculate the volume of hydrogen gas produced at the cathode, Faraday's laws of electrolysis and the Ideal Gas Law are applied. The charge passed through the circuit is determined by the product of current and time, and the volume of H2 is calculated using the number of moles of hydrogen, pressure, and temperature.

Explanation:

Calculation of Hydrogen Gas Volume

To calculate the volume of hydrogen gas (H2) produced at the cathode during electrolysis, we use Faraday's laws of electrolysis which state that the amount of substance altered at an electrode during electrolysis is proportional to the amount of electricity that passes through the circuit. Here, we need to know the charge passed through the circuit, which can be calculated by multiplying the current (I) by the time (t), where I = 1.45 A and t = 13.00 min (converted to seconds).

The reaction at the cathode for the electrolysis of aqueous HNO3 will produce hydrogen gas according to the reaction:

2H2O(l) + 2e- → H2(g) + 2OH-

This means that 2 moles of electrons are required to produce 1 mole of H2. By using the Faraday constant (96,485 C/mol e-), we can calculate the moles of hydrogen produced:

Moles of electrons (n) = It/F, where F is the Faraday constant.

Finally, we can find the volume of H2 gas using the Ideal Gas Law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles of hydrogen, R is the Ideal Gas Constant (0.0821 L·atm/mol·K) and T is the temperature in Kelvin.

With the given temperature (25.0°C) and pressure (1.03 atm), we convert the temperature to Kelvin, then rearrange the Ideal Gas Law to solve for V. Remember to use the number of moles of H2, not the number of moles of electrons.

Answer:

Explanation:

Volatile organic compounds are the  organic chemicals that get easily vaporized in air.

The secondary chemicals or the secondary pollutants are the photochemical substances that are formed in the presence of sunlight.

The amount of gases and small particles present in the atmosphere, responsible for influencing ecosystem and the wellness of human beings is known as the Air Quality

Air pollution refers to the high concentrations of gases or small particles that are present in the atmosphere, which can cause harm to the humans and other living organisms and structures established by humans.

Aerosols are the tiny particles present in liquid or solid state, that are suspended in air.

Answer:

The concentration of the potassium ions in the original potassium chromate solution is 4.2927 mol/L.

The concentration of the chromate ions in the final solution is 1.0731 mol/L.

Explanation:

[tex]K_2CrO_4+2AgNO_3\rightarrow Ag_2CrO_4+2KNO_3[/tex]

Volume of solution A i.e. solution of silver nitrate = 466.0 mL = 0.466 L

Volume of solution B i.e. solution of potassium chromate = 466.0 mL = 0.466 L

Moles of silver chromate =[tex]\frac{331.8}{331.73 g/mol}=1.0002 mol[/tex]

According to reaction , 1 mol of silver chromate is produce from 2 moles of silver nitrate.

Then, 1.0002 moles of silver chromate will be formed from:

[tex]\frac{1}{2}\times 1.0002 mol=0.5001 mol[/tex] of silver nitrate.

According to reaction , 1 mol of silver chromate is produce from 1 mole of potassium chromate.

Then, 1.0002 moles of silver chromate will be formed from:

[tex]\frac{1}{1}\times 1.0002 mol=1.0002 mol[/tex] of potassium chromate

[tex]Concentration =\frac{Moles}{Volume (L)}[/tex]

a) The concentration of the potassium ions in the original potassium chromate solution.

Volume of the original solution = 0.466 L

1 mol of potassium chromate dissociates into 2mol of potassium ions and 1 mol of chromate ions:

Moles of potassium ions = 2 × 1.0002 mol = 2.0004 mol

[tex][K^+]=\frac{2.0004 mol}{0.466 L}=4.2927 mol/L[/tex]

b) The concentration of the chromate ions in the final solution

Volume of the final solution = 0.466 L + 0.466 L

Moles of chromate ions = 1 × 1.0002 mol = 1.0002 mol

[tex][CrO_4^{2+}]=\frac{1.0002 mol}{0.466 L+0.466L}=1.0731 mol/L[/tex]

Answer:

[tex]\boxed{\text{-4.25 kJ}}[/tex]

Explanation:

ΔE = q + w

By convention, anything leaving the system is negative and anything entering the system is positive.

Data:

q = -3.30 kJ

w = -950 J = -0.950 kJ

Calculation

ΔE = -3.30 - 0.950 = -4.25 kJ

[tex]\text{The change in E is }\boxed{\textbf{-4.25 kJ}}[/tex]

Final answer:

The change in internal energy (ΔE) for the decomposition of NI3 is -4250 J, which indicates the system lost energy.

Explanation:

The change in internal energy (ΔE) of the system can be calculated using the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system (q) minus the work done by the system (w): ΔE = q - w. In this scenario, the sample of NI3 decomposes, releasing heat (q = -3.30 kJ, since the system loses heat) and doing work (w = 950 J).

First, it is important to make sure both q and w are in the same units. We can convert kilojoules to joules by multiplying by 1000: -3.30 kJ = -3300 J.

Therefore, the change in internal energy ΔE is:

ΔE = q - w
ΔE = (-3300 J) - (950 J)
ΔE = -4250 J

The negative sign indicates that the total energy of the system decreased by 4250 joules.

Answer:

C₄H₈O₂.

Explanation:

n = mass/atomic mass,

mol C = mass/(atomic mass) = (54.5 g)/(12.0 g/mol) = 4.54 mol.

mol H = mass/(atomic mass) = (9.3 g)/(1.0 g/mol) = 9.3 mol.

mol O = mass/(atomic mass) = (36.2 g)/(16.0 g/mol) = 2.26 mol.

∴ C: H: O = (4.54 mol/2.26 mol) : (9.3 mol/2.26 mol) : (2.26 mol/2.26 mol) = 2: 4: 1.

∴ Empirical formula mass of (C₂H₄O) = 2(atomic mass of C) + 4(atomic mass of H) + 1(atomic mass of O) = 2(12.0 g/mol) + 4(1.0 g/mol) + (16.0 g/mol) = 44.0 g/mol.

∴ Number of times empirical mass goes into molecular mass = (88.0 g/mol)/(44.0 g/mol) = 2.0 times.

∴ The molecular formula is, 2(C₂H₄O), that is; (C₄H₈O₂)

Answer:

H₂S; CO₂; SiH₄

Explanation:

London dispersion forces are larger in molecules that are large and have more atoms or electrons.

A. H₂O or H₂S

H₂S. S is below O in the Periodic Table, so it is the larger atom. Its electrons are more polarizable.

B. CO₂ or CO

CO₂. CO₂ has more atoms. It is also linear, so the molecules can get close to each other and maximize the attractive forces.

C. CH₄ or SiH₄

CH₄. Si is below C in the Periodic Table, so it is the larger atom. Its electrons are more polarizable.

Differences are stronger in bigger and heavier atoms than in lighter and smaller ones. Its number of electrons inside a larger atom is, in general, farther away from the nuclei than in a small atom.

Therefore, the answer is "[tex]\bold{H_2S\ , CO_2\ or \ SiH_4}[/tex]"

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Answer:

99.24%.

Explanation:

NaCl + AgNO₃ → AgCl(↓) + NaNO₃,

1.0 mol of NaCl reacts with 1.0 mol of AgNO₃ to produce 1.0 mol of AgCl and 1.0 mol of NaNO₃.

no. of moles of AgCl = mass/molar mass = (2.044 g)/(143.32 g/mol) = 0.0143 mol.

using cross multiplication:

1.0 mol of NaCl produce → 1.0 mol of AgCl, from the stichiometry.

∴ 0.0143 mol of NaCl produce → 0.0143 mol of AgCl.

mass of pure NaCl = (no. of moles of pure NaCl)(molar mass of NaCl) = (0.0143 mol)(58.44 g/mol) = 0.8357 g.

∴ The percentage of NaCl in the impure sample = [(mass of pure NaCl)/(mass of the impure sample)] x 100 = [(0.8357 g)/(0.8421 g)] x 100 = 99.24%.

An impure sample of table salt that weighed 0.8421 g and treated with excess AgNO₃ formed 2.044 g of AgCl, has a percentage of NaCl of 98.98%.

Let's consider the reaction between NaCl and AgNO₃ to produce AgCl and NaNO₃.

NaCl + AgNO₃ ⇒ AgCl + NaNO₃

We can calculate the mass of NaCl that produced 2.044 g of AgCl using the following relations.

[tex]2.044 g AgCl \times \frac{1molAgCl}{143.32 g AgCl} \times \frac{1molNaCl}{1molAgCl} \times \frac{58.44gNaCl}{1molNaCl} = 0.8335gNaCl[/tex]

An impure sample of mass 0.8421 g contains 0.8335 g of NaCl. The percentage of NaCl in the impure sample is:

[tex]\% NaCl = \frac{0.8335g}{0.8421g} \times 100\% = 98.98\%[/tex]

An impure sample of table salt that weighed 0.8421 g and treated with excess AgNO₃ formed 2.044 g of AgCl, has a percentage of NaCl of 98.98%.

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Answer:

C. Sr (NO3)2 •2 H2O

Explanation:

A 30.7 g sample of Strontium nitrate, Sr(NO3)2⋅nH2O, is heated to a contstent mass of 22.9.

Therefore, the calculated hydration number is Sr (NO3)2 •2 H2O.

Answer:

C

Explanation:

Answer:

reduces; facilitating

Explanation:

Carbonic anhydrases is a type of metalloenzyme containing zinc metal which catalyze interconversion between the carbon dioxide gas and water and dissociated ions of the carbonic acid.

The reaction that is catalyzed by enzyme, carbonic anhydrase is:

HCO₃⁻ + H⁺ ⇄ CO₂ + H₂O

The enzyme maintains the acid-base balance in the body and helps in the transportation of carbon dioxide through out the body.

The carbon dioxide formed as a by-product of metabolism which is transported to blood in the form of bicarbonate ions by the action of carbonic anhydrase.

Thus,

By converting CO₂ to H₂CO₃, Carbonic anhydrase reduces the PCO₂ in endothelial cells, red blood cells, and plasma, thereby facilitating diffusion of CO₂ from tissue cells to these locations.

Carbonic anhydrase reduces PCO₂ by converting CO₂ to H₂CO₃, which leads to an increase in the diffusion of CO₂ from tissue to blood.

By converting CO₂ to H₂CO₃ (carbonic acid), carbonic anhydrase lowers the PCO₂ (partial pressure of carbon dioxide) in endothelial cells, red blood cells, and plasma, thereby increasing diffusion of CO₂ from tissue cells to these locations. This enzyme catalyzes the reversible hydration of carbon dioxide, forming bicarbonate ions (HCO₃⁻) and protons (H⁺). The reduction in PCO₂ creates a pressure gradient that favors the diffusion of CO₂ from the tissues, where its concentration is higher, towards the blood where it’s lower due to the action of carbonic anhydrase.

Using Faraday's laws of electrolysis, it takes approximately 344.91 minutes to electroplate 29.6 grams of nickel using a current of 4.7 A.

The student is asking how long it would take to electroplate 29.6 grams of nickel using a current of 4.7 amps. To calculate the time required for electroplating, we'll use Faraday's laws of electrolysis, which relate the chemical amount of substance produced at an electrode to the amount of electricity used.

The half-reaction for nickel plating is [tex]Ni^{+2}[/tex] + 2e-
ightarrow Ni(s) and the molar mass of nickel is approximately 58.69 g/mol. Nickel has a valency of 2, which means it requires 2 moles of electrons (2 Faradays) to deposit one mole of nickel. Based on Faraday's law, the charge (Q) in coulombs required to deposit a substance is Q = n x F, where n is the number of moles and F is Faraday's constant (96485 C/mol).

First, we need to convert the mass of nickel to moles using the molar mass: 29.6 g / 58.69 g/mol
gives approximately 0.504 moles of Ni. Thus, the total charge needed will be 0.504 moles x 2 x 96485 C/mol, which equals 97262.2 C.

Next, we find how long it takes for this charge to pass through the solution using the current (I) given: Time (t) = Q / I, where
t = time in seconds. So, t = 97262.2 C / 4.7 A
gives approximately 20694.51 seconds. Converting that to minutes, we divide by 60, resulting in about 344.91 minutes.

Answer:

Which species of beetles are most closely related.

Explanation:

Molecular clocks are often used to determine where species diverge. This helps scientists determine the different mutations that had occurred to cause the separation of species. It can help find common ancestors within different species, so it can also determine how closely related species are.

Answer:

Which species of beetles are most closely related.

Explanation:

Answer:

527.68 mL

Explanation:

We will assume that nitrogen is behaving as ideal gas here.

For ideal gas the gas law is:

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

Where

P1= initial pressure = 740 torr

V1= initial volume = 500mL

T1= initial temperature = 25⁰C = 298 K

P2= final pressure = 760 torr

V2= final volume = ?

T2= final temperature = 50⁰C = 323 K

Putting values in the gas law

Final volume = [tex]\frac{740X500X323}{298X760}= 527.68 mL[/tex]

Final answer:

The average rate of decomposition of N2O5 over each time interval was calculated using changes in concentration over time, resulting in rates of 0.00123 M/s, 0.00105 M/s, and 0.00085 M/s for the respective intervals of 0-195 s, 195-556 s, and 556-825 s.

Explanation:

The average rate of a reaction is calculated by the change in concentration of a reactant or a product over a certain time period. For the decomposition of N2O5, the average rate over each time interval can be found using the formula: rate = -(Δ[N2O5])/(Δt), where Δ represents the change in concentration or time.

For the interval from 0 s to 195 s, the average rate is:
rate = - (1.86 M - 2.10 M) / (195 s - 0 s) = - (-0.24 M) / 195 s = 0.00123 M/s

For the interval from 195 s to 556 s, the average rate is:
rate = - (1.48 M - 1.86 M) / (556 s - 195 s) = - (-0.38 M) / 361 s = 0.00105 M/s

For the interval from 556 s to 825 s, the average rate is:
rate = - (1.25 M - 1.48 M) / (825 s - 556 s) = - (-0.23 M) / 269 s = 0.00085 M/s

The equilibrium constants for the reactions can be calculated using the standard free energy change and the formula K = e^{(-ΔG°/(RT))}, but specific ΔG° values or tables referenced are needed to complete the calculations.

To calculate the equilibrium constant for the reactions at 25 °C, we use the given thermodynamic data from the tables and apply the relation between the standard free energy change (ΔG°) and the equilibrium constant (K). The relation is given by the equation ΔG° = -RTlnK, where R is the gas constant (8.314 J/mol·K), T is the temperature in Kelvin, and K is the equilibrium constant. For each reaction with a given ΔG° value, we can rearrange the formula to solve for K: K = e^{(-ΔG°/(RT))}.

For the provided exercises:

When the necessary thermodynamic data is provided, each reaction's equilibrium constant can be calculated using the formula K = e^{(-ΔG°/(RT))}, with R = 8.314 J/mol·K, and T = 298.15 K (since 25 °C is equivalent to 298.15 K).

Answer : The enthalpy of reaction [tex](\Delta H_{rxn})[/tex] is, 67.716 KJ/mole

Explanation :

First we have to calculate the moles of [tex]AgNO_3[/tex] and [tex]HCl[/tex].

[tex]\text{Moles of }AgNO_3=\text{Molarity of }AgNO_3\times \text{Volume}=(0.100mole/L)\times (0.05L)=0.005mole[/tex]

[tex]\text{Moles of }HCl=\text{Molarity of }HCl\times \text{Volume}=(0.100mole/L)\times (0.05L)=0.005mole[/tex]

Now we have to calculate the moles of AgCl formed.

The balanced chemical reaction will be,

[tex]AgNO_3(aq)+HCl(aq)\rightarrow AgCl(s)+HNO_3(aq)[/tex]

As, 1 mole of [tex]AgNO_3[/tex] react with 1 mole of [tex]HCl[/tex] to give 1 mole of [tex]AgCl[/tex]

So, 0.005 mole of [tex]AgNO_3[/tex] react with 0.005 mole of [tex]HCl[/tex] to give 1 mole of [tex]AgCl[/tex]

The moles of AgCl formed  = 0.005 mole

Total volume of the solution = 50.0 ml + 50.0 ml = 100.0 ml

Now we have to calculate the mass of solution.

Mass of the solution = Density of the solution × Volume of the solution

Mass of the solution = 1.00 g/ml × 100.0 ml = 100 g

Now we have to calculate the heat.

[tex]q=m\times C\Delta T=m\times C \times (T_2-T_1)[/tex]

where,

q = heat

C = specific heat capacity = [tex]4.18J/g^oC[/tex]

m = mass = 100 g

[tex]T_2[/tex] = final temperature = [tex]24.21^oC[/tex]

[tex]T_1[/tex] = initial temperature = [tex]23.40^oC[/tex]

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

[tex]q=100g\times (4.18J/g^oC)\times (24.21-23.40)^oC[/tex]

[tex]q=338.58J[/tex]

Now  we have to calculate the enthalpy of the reaction.

[tex]\Delta H_{rxn}=\frac{q}{n}[/tex]

where,

[tex]\Delta H_{rxn}[/tex] = enthalpy of reaction = ?

q = heat of reaction = 338.58 J

n = moles of reaction = 0.005 mole

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

[tex]\Delta H_{rxn}=\frac{338.58J}{0.005mole}=6771.6J/mole=67.716KJ/mole[/tex]

Conversion used : (1 KJ = 1000 J)

Therefore, the enthalpy of reaction [tex](\Delta H_{rxn})[/tex] is, 67.716 KJ/mole

For this reaction, the heat of reaction is -67.8 KJ/mol.

The equation of the reaction is;

AgNO3(aq) + HCl(aq) -----> AgCl(s) + HNO3(aq)

Number of moles of AgNO3 = 50/1000 L ×  0.100 M = 0.005 M

Number of moles of HCl = 50/1000 L  ×  0.100 M = 0.005 M

Temperature change =  24.21 °C - 23.40 °C = 0.81°C

Total volume of solution =  50.0 mL +  50.0 mL = 100 mL

Since the density of solution= 1.00 g/mL

Total mass of solution = 100g

Heat absorbed by solution = mcθ

m = mass of solution

c = specific heat capacity of solution

θ = temperature change

Heat absorbed by solution = 100g ×  4.18 J/g ∙ °C  × 0.81°C = 0.339 KJ

ΔHrxn = -( 0.339 KJ)/ 0.005 M

ΔHrxn = -67.8 KJ/mol

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Answer: The temperature of the unknown sample is 64.65 °C

Explanation:

To calculate the temperature of the unknown sample, we use the following equation:

[tex]T=\frac{(V-V_1)}{(V_2-V_1)}\times (T_2-T_1)+T_1[/tex]

where,

T = temperature of the unknown sample = ?

V = thermistor reading of the unknown sample = 116 mV

[tex]T_1[/tex] = melting point of ice = 0°C

[tex]V_1[/tex] = thermistor reading of ice = -45 mV

[tex]T_1[/tex] = boiling point of water = 100°C

[tex]V_1[/tex] = thermistor reading of water = 204 mV

Putting values in above equation, we get:

[tex]T=\frac{(116-(-45))}{(204-(-45))}\times (100-0)+0\\\\T=64.65^oC[/tex]

Hence, the temperature of the unknown sample is 64.65 °C

The temperature of the unknown sample in C° is approximately 45.00°C.

To find the temperature of the unknown sample, we first need to establish a relationship between the voltage read by the thermistor and the temperature in degrees Celsius. We have two calibration points: ice water and boiling water, which correspond to 0°C and 100°C, respectively.

Let's denote the voltage read by the thermistor as \( V \) and the temperature as \( T \). We can then set up two equations based on the calibration points:

1. For ice water (0°C), the thermistor reads -45 mV:

[tex]\[ V_{ice} = -45 \text{ mV} \] \[ T_{ice} = 0°C \][/tex]

2. For boiling water (100°C), the thermistor reads 204 mV:

[tex]\[ V_{boiling} = 204 \text{ mV} \] \[ T_{boiling} = 100°C \][/tex]

We can assume a linear relationship between voltage and temperature for the thermistor, which allows us to use a simple linear interpolation formula:

[tex]\[ T = T_{ice} + \frac{(V - V_{ice}) \times (T_{boiling} - T_{ice})}{V_{boiling} - V_{ice}} \][/tex]

Now, we need to find the temperature \( T \) when the thermistor reads 116 mV for the unknown sample:

[tex]\[ T = 0°C + \frac{(116 \text{ mV} - (-45 \text{ mV})) \times (100°C - 0°C)}{204 \text{ mV} - (-45 \text{ mV})} \] \[ T = 0°C + \frac{(116 \text{ mV} + 45 \text{ mV}) \times 100°C}{204 \text{ mV} + 45 \text{ mV}} \] \[ T = 0°C + \frac{161 \text{ mV} \times 100°C}{249 \text{ mV}} \] \[ T = 0°C + \frac{161}{2.49} \times 100°C \] \[ T = 0°C + 64.6586345 \times 100°C \] \[ T = 64.6586345°C \][/tex]

Rounding to two decimal places, the temperature of the unknown sample is approximately 45.00°C.

Answer:

  c.  0 °C

Explanation:

Standard temperature is 273.15 K, or 0 °C, or 32 °F, as defined by the International Union of Pure and Applied Chemistry (IUPAC) in 1982.

Answer:

Standard temperature is exactly (C) 0ºC

Explanation:

STP means standard temperature pressure at which

T = 0℃ or 273K and Pressure = 1 atm

NTP means Normal temperature pressure which means room temperature and  pressure at which

T = 20℃ or 293 K and Pressure = 1 atm

SATP means standard Ambient temperature pressure at which

T = 25℃ or 298K and P = 1atm

In tropical countries, the climate will be warm and hence room temperature usually  considered as

T = 25℃ or 298K and P = 1 atm  

Lab temperature is same as that of room temperature.

Answer:

Neither accurate nor precise

Explanation:

The values were not near or even the same as the accepted value thus making it neither accurate nor precise.

Answer: neither accurate nor precise​

Explanation:

Accuracy is defined as how close the measured value is to a standard value. For example if the given volume of water is 20 ml and the two measured values are 19 ml and 18 ml then the former measured value is more accurate than the later.  

Precision is defined as how measured values are close to each other. For example, if the length of the wire of 10 m. If the first person measures the length of the same wire thrice and got values 9.7, 9.8 and 9.75 m whereas the second person got values 9.5 , 9.6 and 9.8. In such a case the first person’s measured value is more precise.

Thus as the accepted value is 1.43 and measured values are 1.29 , 1.93 and 0.88 , the experimental data is neither accurate nor precise.

The final concentration after 172 seconds is 1.15 M. To obtain this answer, use the the integrated rate law for the order of reaction. Based on the problem, this is a second order reaction. The units of the rate constant also support that it is a second order reaction.

Further Explanation:

The solution to this problem is straightforward.

STEP 1: Since the reaction is a second order reaction, the integrated rate law will be:

[tex]\frac{1}{C_{f}} = \ kt \ + \frac{1}{C_{i}}[/tex]

where:

C(f) is the final concentration

k is the rate constant

t is the time

C(i) is the initial concentration

STEP 2: Plugging in the values given in the problem into the equation, the following equation should be obtained:

[tex]\frac{1}{C_{f}} \ = (1.30  \ x \ 10^{-3} \frac{ \ 1 }{ \ M-s})(172 \ s) \ + \ \frac{1}{1.54 \ M} \\[/tex]

STEP 3: Using algebra to solve for C(f):

[tex]\frac{1}{C_{f}} = \ 0.87295\\ \\C_{f} = \ 1.14554 \ M[/tex]

Since the given values only have 3 significant figures, the final answer must be expressed with 3 significant figures as well.

Therefore,

[tex]\boxed {C_{f}\ =  \ 1.15 \ M}[/tex]

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Keywords: rate law, second order, integrated rate law

when aqueous solution of [tex]CH_{3} NH_{3}Cl[/tex] is taken it dissociates and gives hydronium ion so it is acidic in nature. It is example of hydrolysis reaction

Hydrolysis reaction is a reaction in which bond is broken down with the help of water. Lysis term stands for breaking of anything.

Example: Hydrolysis of ester produces alcohol and acid. Hydrolysis of ester is done both in acid and basic condition.

Any acidic solution that contains acidic acid when put in water produces hydronium ion or we can say that any species that produces hydronium ion in water is acidic in nature.

In our case when [tex]CH_{3} NH_{3}Cl[/tex] is put in water it easily gives hydronium ion in water this shows that it is acidic in nature. and the reaction can be shown as:

[tex]CH_{3} NH_{3}Cl +H_{2}O\rightarrow CH_{3}NH_{2}Cl^{-} +H_{3}O^{+}[/tex]

Thus[tex]CH_{3} NH_{3}Cl[/tex] is acidic in nature and is a hydrolysis reaction.

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An aqueous solution of CH3NH3Cl is acidic due to the hydrolysis reaction that occurs when the compound is dissolved in water, producing CH3NH3+ ions that increase the concentration of H+ ions in the solution.

Aqueous solutions of CH3NH3Cl are acidic due to the hydrolysis reaction that occurs when the compound is dissolved in water. The hydrolysis reaction of CH3NH3Cl can be represented by the chemical equation:

CH3NH3Cl + H2O → CH3NH3+ + Cl- + H2O

In this reaction, CH3NH3Cl dissociates into CH3NH3+ and Cl- ions. The CH3NH3+ acts as a weak acid, releasing H+ ions into the solution, resulting in an overall acidic pH.

Answer: Option (b) is the correct answer.

Explanation:

In liquid state, particles do have kinetic energy that helps in partially overcoming the intermolecular forces between the molecules. But still the particles are close together and they are able to slide past each other.

So, when we apply pressure on a liquid then its molecules partially gets compressed.

On the other hand, molecules of a solid are held together by strong intermolecular forces of attraction. Hence, they have definite shape and volume. As a result, solids do not get compressed.

In gases and plasma state of matter, molecules are gar away from each other. So, they are able to get completely compressed when a pressure is applied.

Thus, we can conclude that liquid is the state of matter which consists of particles that can be partially compressed.

Answer:

liquid

Explanation:

Answer: The percent yield of the given reaction is 82 %.

Explanation:

The chemical equation for the reaction of zinc and hydrochloric acid follows:

[tex]Zn+2HCl\rightarrow ZnCl_2+H_2[/tex]

To calculate the percent yield of the reaction, we use the equation:

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

Experimental yield of hydrogen gas = 164 g

Theoretical yield of hydrogen gas = 200 g

Putting values in above equation, we get:

[tex]\%\text{ yield of hydrogen gas}=\frac{164g}{200g}\times 100\\\\\% \text{yield of hydrogen gas}=82\%[/tex]

Hence, the percent yield of the reaction is 82 %.

Answer:

8 proton and 9 neutron.

Explanation:

there are 17 total of protons and neutron

Taking into account the constitution of an atom and the definition of atomic number, the charge of the nucleus in an atom of oxygen-17 is +8.

All atoms are made up of subatomic particles: protons and neutrons, which are part of their nucleus, and electrons, which revolve around them. Protons are positively charged, neutrons are neutrally charged, and electrons are negatively charged (electrons).

In other words, the atomic nucleus is the central part of the atom that is made up of protons and neutrons, while the orbitals or peripheral region is an area where electrons are found.

The neutron is an electrically neutral subatomic particle, while the proton has a positive electrical charge. Electrons have a negative charge, move around the nucleus at different energy levels and are attracted to protons, positive in the atom through electromagnetic force.

Each chemical element is characterized by the number of protons in its nucleus, which is called the atomic number Z.

The periodic table is an arrangement in which chemical elements are arranged by increasing atomic number.

In the periodic table you can see that oxygen has an atomic number of 8. This indicates that in the nucleus of this atom there are 8 protons. Like neutrons, another particle found in the nucleus, has a neutral charge, and protons have a positive charge, the oxygen nucleus has a charge of +8.

In summary, the charge of the nucleus in an atom of oxygen-17 is +8.

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An organism gets carbon by using carbon dioxide in the atmosphere to make sugar molecules. This organism is a producer.

An organism that can make its own nourishment by the use of light, water, carbon dioxide, or other substances is an autotroph. Autotrophs are also referred to as producers because they make their own nourishment.

Producers are living things with the ability to grow their own nourishment. They frequently contain green vegetation. They use the process of photosynthesis to capture solar energy and use it to produce food. Since they are unable to create food on their own, all other creatures rely on producers for nourishment.

Green plants, phytoplankton, and cyanobacteria all have cells that can synthesize oxygen. Photosynthetic cells are highly diverse. Cells create sugar molecules and oxygen during the process of photosynthesis by using carbon dioxide and energy from the sun.

Thus, An organism gets carbon by using carbon dioxide in the atmosphere to make sugar molecules. This organism is a producer.

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The equilibrium concentration of N2O4 in the given reaction can be calculated by setting up an expression for the equilibrium constant in terms of the change in concentration and then solving for the unknown.

This question involves examining a chemical equilibrium problem for the reversible reaction: N2O4(g) ⇄ 2 NO2(g), with the given equilibrium constant, Kc = 5.8 × 10-3. The initial concentration of N2O4 is given as 0.040 M, while the initial concentration of NO2 is given as 0 M. To solve this, we will let 'x' be the amount of N2O4 that decomposes into NO2 at equilibrium. Therefore, the equilibrium concentration of N2O4 would be given as N2O4 = 0.040 - x, and for NO2 it would be 2x (because the stoichiometry of the reaction shows that for each mole of N2O4 decomposed, 2 moles of NO2 are produced).

Now we can set up an expression for the equilibrium constant such that: Kc = [NO2]^2 / [N2O4] = (2x)^2 / (0.040 - x). By substituting 5.8 x 10^-3 for the equilibrium constant and solving for x, we will be able to find the equilibrium concentration of N2O4, which will be 0.040 - x.

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Answer:

B

Explanation:

It has 2 NH4 molecules and 1 CO3 molecule.

NH4 has a molar mass of 18g/mol. Since there are two NH4s, it makes up 36g of the (NH4)2CO3.

CO3 has a molar mass of 60g/mol. Since there is one CO3, it makes up 60g of the (NH4)2CO3.

If you add up 36 and 60, you will get 96g.