Which is an example of the practical pursuit of alchemy

Answer:

16.0 g/mol (3 s.f.)

Explanation:

Molar mass is the mass of a mole of substance.

1 mole of CH₄ has 1 C atom and 4 H atoms.

Since the molar mass is numerically equal to the molecular mass of a compound, let's find the molecular mass of CH₄ first.

Molecular mass= sum of all the atomic mass in a molecule

Molecular mass of CH₄

= 12.011 amu +4(1.008 amu)

= 16.043 amu

Thus the molar mass of CH₄ is 16.043g/mol, or 16.0g/mol to 3 significant figures.

Answer:

a. 14.9g/L

b. 1.49x10⁻⁶

c. 1.49x10⁷

Explanation:

You can write the buffer Ksp of Co(OH)₂ as follows:

Co(OH)₂(s) ⇄ Co²⁺ + 2OH⁻

Ksp = 1.6x10⁻¹⁵ = [Co²⁺] [OH⁻]²

To have buffered the solutions means  [OH⁻] is fixed. From the equilibrium of water we can relate  [OH⁻] with pH as follows:

[OH⁻] = 10^[14-pH]

With [OH⁻] and Ksp we can solve for [Co²⁺]. Its concentration is equal to solubility (That is the amount of Co(OH)₂ that can be dissolved).

[Co²⁺] is in mol/L. With molar mass of Co(OH)₂ -92.948g/mol-, We can obtain, in the end, its solubility in g/L.

-Molar concentration of [Co²⁺] and solubility:

a. [OH⁻] = 10^[14-7.00] = 1x10⁻⁷

[Co²⁺] = 1.6x10⁻¹⁵ / [1x10⁻⁷]²

[Co²⁺] = 0.16mol / L = Solubility.

In g/L = 0.16mol / L ₓ(92.948g/mol) =

14.9g/L

b. [OH⁻] = 10^[14-10.00] = 1x10⁻⁴

[Co²⁺] = 1.6x10⁻¹⁵ / [1x10⁻⁴]²

[Co²⁺] = 1.6x10⁻⁸mol / L = Solubility.

In g/L = 1.6x10⁻⁸mol / L ₓ(92.948g/mol) =

1.49x10⁻⁶g/L

c.[OH⁻] = 10^[14-4.00] = 1x10⁻¹⁰

[Co²⁺] = 1.6x10⁻¹⁵ / [1x10⁻¹⁰]²

[Co²⁺] = 1.6x10⁵mol / L = Solubility.

In g/L = 1.6x10⁵mol / L ₓ(92.948g/mol) =

1.49x10⁷g/L

As you can see, and as general rule, all hydroxides are solubles in acids.

Answer:

A. The neutral-charged neutrons and positive-charged protons are found within the nucleus, and the negative-charged electrons orbit outside the nucleus of the atom.

Explanation:

Before examining the options, it's important to know that the atom is made up of three sub atomic particles which are; Protons, Neutrons and Electrons.

The protons are positively charged and are found in the nucleus of an atom. The Neutron A=are neutral in terms of charge and are also found in the nucleus of an atom. The electrons on the other hand are negatively charged and are found outside the nucleus if an atom, more specifically on the orbitals.

The option that best describes this is; option A.

Answer:

identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through identical membranes simultaneously. After a certain amount of time, it was found that 6.23 mL of O2 had passed through the membrane, but only 3.85 mL of of the unknown gas had passed through. What is the molar mass of the unknown gas

identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through identical membranes simultaneously. After a certain amount of time, it was found that 6.23 mL of O2 had passed through the membrane, but only 3.85 mL of of the unknown gas had passed through. What is the molar mass of the unknown gas

Answer:

Negligible

Explanation:

According to the kinetic theory of gases, the degree of intermolecular interaction between gases is minimal and gas molecules tend to spread out and fill up the volume of the container.

If the attraction between gas molecules increases, then the volume of the gas decreases accordingly. This is because, gas molecules become highly attracted to each other.

This intermolecular attractive force may be so strong, such that the actual volume of the gas become negligible compared to the volume of the container.

Answer:

The given reaction is:  

Ca(OH)₂ (s) + CO₂ (g) ⇒ CaCO₃ (s) + H₂O (g)

The ΔH°f of Ca(OH)₂ (s) is -986.09 kJ/mole, the ΔH°f of CO₂ (g) is -393.509 kJ/mol, the ΔH°f of CaCO₃ (s) is -1207.6 kJ/mol, and the ΔH°f of H₂O (g) is -241.83 kJ/mol.  

ΔH°rxn = 1 × ΔH°f of CaCO₃ (s) + 1 × ΔH°f of H₂O (g) - 1 × ΔH°f of Ca(OH)₂ (s) - 1 × ΔH°f of CO₂ (g)

ΔH°rxn = 1 (-1207.6) + 1(-241.83) - 1 (-986.09) - 1 (-393.509)

ΔH°rxn = -69.831 kJ

b) The molecular mass of calcium hydroxide is 74.096 gram per mole.  

The mass of calcium hydroxide given is 7.50 Kg or 7500 grams.  

The number of moles of calcium hydroxide is,  

n = Mass of Ca(OH)₂ / Molecular mass of Ca(OH)₂

n = 7500 / 74.1

n = 101.21 moles

As ΔH is negative, therefore, release of heat is taking place. Thus, when one mole of calcium hydroxide reacts, the heat released is -69.831 kJ. Therefore, 101.21 moles of calcium hydroxide will release the heat,  

= 101.21 × 69.831 kJ

= 7.067 × 10³ kJ

Answer:

Total mass: 170.3 g

Fraction of NaCl: 0.089%

Percent of NaCl: 8.98%

3.43 g of NaCl in 38.2 g of solution

1 mL . (170.3 g of solution / 1.07 g solution) = 159.1 mL

159.1 mL . (2 g NaCl / 15.3 g NaCl) = 20.8 mL

Explanation:

Our scenario is 15.3 g of NaCl in 155 g of water

Total mass: 15.3 g + 155 g = 170.3 g of solution

Our solute is NaCl - Our solvent is water.

To determine the fraction we divide:

15.3 g / 170.3 g = 0.0898

To determine percent, we multiply the fraction by 100

0.089 . 100 = 8.98 %

We can make a conversion factor to determine the mass of NaCl in 38.2 g of solution. If 15.3 g of NaCl are in 170.3 g of solution and we need 38.2 g, we can propose → (15.3 / 170.3) . 38.2 = 3.43 g of NaCl

The conversion factors are to find what volume of solution is on 2g of NaCl are:

Density data always reffers to solution. So 1.07 grams of solution are contained in 1 mL of solution

1 mL . 170.3 g of solution / 1.07 g solution = 159.1 mL

This is the volume for our 15.3 g of NaCl so:

159.1 mL . (2 g NaCl / 15.3 g NaCl) = 20.8 mL

Answer:

81 molecules

Explanation:

The reaction between C5H12 and O2 is a combustion reaction and is represented by the following equation;

C5H12 + 8O2 --> 5CO2 + 6H2O

The ratio of C5H12 to O2 from the above equation is 1 : 8.

Aplying the conditins of the question; 24 molecules each of C5H12 and O2 we have;

3C5H12 + 24O2 --> 15CO2 + 18H2O

This means we have 24 - 3 = 21 molecules of C5H12 that are unreacted.

Total molecules is given as;

3(C5H12) + 24(O2) + 15(CO2) + 18(H2O) + 21(Unreacted C5H12) = 81 molecules

Answer:

Protecting group

Explanation:

TMS groups can be used as protecting and leaving groups for the synthesis of siloxane-based molecules.   It is also used as protecting group for alcohols.

A protecting group is a temporary group added during organic synthesis to prevent a portion of molecule from reacting.

Answer:

Activation energy for the reaction is 39029J/mol

Explanation:

Arrhenius equation is an useful equation that relates rate of reaction at two different temperatures as follows:

[tex]ln\frac{K_2}{K_1} = \frac{-Ea}{R} (\frac{1}{T_2} -\frac{1}{T_1} )[/tex]

Where K₁ and K₂ are rate of reaction, Ea is activation energy and R is gas constant (8.314J/molK

If the reaction at 400K is 50 times more faster than at 300K:

K₂/K₁ = 50 where T₂ = 400K and T₁ = 300K:

[tex]ln50 = \frac{-Ea}{8.314J/molK} (\frac{1}{400K} -\frac{1}{300K} )[/tex]

[tex]ln 50 = 1x10^{-4}Ea[/tex]

Ea = 39029 J/mol

The activation energy for this chemical reaction is equal to 39,029.24 J/mol.

Given the following data:

Ideal gas constant, R = 8.314 J/molK

To determine the activation energy for this chemical reaction, we would use the Arrhenius' equation:

Mathematically, Arrhenius' equation is given by the formula:

[tex]ln\frac{K_2}{K_1} = \frac{-E_a}{R} (\frac{1}{T_2} - \frac{1}{T_1})[/tex]

Where:

Substituting the given parameters into the formula, we have;

[tex]ln50 = \frac{-E_a}{8.314} (\frac{1}{400} - \frac{1}{300})\\\\3.9120 = \frac{-E_a}{8.314} (\frac{-1}{1200})\\\\3.9120 = \frac{E_a}{9976.8} \\\\E_a = 9976.8 \times 3.9120\\\\E_a = 39,029.24 \;J/mol[/tex]

Read more: https://brainly.com/question/24212500

Answer:

Normality N = 0.2 N

Explanation:

Normality is the number of gram of equivalent of solute divided of volume of solution, where the number of gram of equivalent of solute is weight of the solute divided by the equivalent weight.

Normality is represented by N.

Mathematically, we have :

[tex]\mathbf{Normality \ N = \dfrac{Number \ of \ gram \of \ equivalent\ of\ solute }{volume \ of \ solution}}[/tex]

Given that:

number of gram of equivalent of solute = 90 milliequivalents 90 × 10⁻³ equivalent

volume of solution (HCl) = 450 mL 450 × 10⁻³ L

[tex]\mathbf{Normality \ N = \dfrac{90 \times 10^{-3}}{450 \times 10^{-3}}}[/tex]

Normality N = 0.2 N

Answer:

1) evolution of gas

2) evolution of heat

Explanation:

In this reaction, glucose is broken down into its constituents; carbon dioxide and water. The question is to decipher indicators of a chemical reaction from the equation.

If we look at the equation carefully, we will notice that a gas was evolved (CO2). The evolution of a gas indicates that a chemical reaction must have taken place. Secondly, energy is given off as heat. This is another indication that a chemical reaction has taken place.

Answer:

The answer is "29.081"

Explanation:

when the empty 2.00 L container of 1000 kg, a sample of HI (9.30 x 10-3 mol) has also been placed.  

[tex]\text{calculating the initial HI}= \frac{mol}{V}[/tex]

                                       [tex]=\frac{9.3 \times 10 ^ -3}{2}[/tex]

                                      [tex]=0.00465 \ Mol[/tex]

[tex]\text{Similarly}\ \ I_2 \ \ \text{follows} \ \ H_2 = 0 }[/tex]

Its density of I 2 was 6.29x10-4 M if the balance had been obtained, then we have to get the intensity of equilibrium then:

[tex]HI = 0.00465 - 2x\\\\ I_{2} \ eq = H_2 \ eq = 0 + x \\\\[/tex]

It is defined that:

[tex]I_2 = 6.29 \times 10^{-4} \ M \\\\x = I_2 \\\\[/tex]

[tex]HI \ eq= 0.00465 - 2x \\[/tex]

          [tex]=0.00465 -2 \times 6.29 \times 10^{-4} \\\\ = 0.00465 -\frac{25.16 }{10^4} \\\\ = 0.003392\ M[/tex]

Now, we calculate the position:  

For the reaction [tex]H 2(g) + I 2(g)\rightleftharpoons 2HI(g)[/tex], you can calculate the value of Kc at 1000 K.  

data expression for Kc

[tex]2HI \rightleftharpoons H_2 + I_2 \\\\\to Kc = \frac{H_2 \times I_2}{HI^2}[/tex]

         [tex]= \frac{6.29\times10^{-4} \times 6.29 \times 10^{-4}}{0.003392^2} \\\\= \frac{6.29\times 6.29 \times 10^{-8}}{0.003392^2} \\\\= \frac{39.564 \times 10^{-8}}{1.150 \times 10-5} \\\\= 0.034386[/tex]

calculating the reverse reaction

[tex]H_2(g) + I_2(g)\rightleftharpoons 2HI(g)[/tex]

[tex]Kc = \frac{1}{Kc} \\\\[/tex]

     [tex]= \frac{1}{0.034386}\\ \\= 29.081\\[/tex]

The Kc of the reaction is 40.

Molarity of the HI = 9.30×10^−3mol/ 2.00 L = 4.65 × 10^-3 M

Let the concentrations of I2 and H2 be x, but we are told in the question that 6.29×10^−4M was present at equilibrium.

The molarity of HI at equilibrium now becomes; 4.65 × 10^-3 M - 6.29×10^−4M

= 4 × 10^-3 M

But;

Kc = [HI]^2/[H2] [I2]

Kc = ( 4 × 10^-3)^2/(6.29×10^−4)^2

Kc = 40

Learn more: https://brainly.com/question/755860

Answer:

H₂SO₄  

Explanation:

A Brønsted acid is a proton donor.  It loses protons.

This equation may be easier to understand if we write it ionically.

[tex]\underbrace{\hbox{H$_{2}$SO$_{4}$}}_{\hbox{Br$\o{}$nsted acid}} + 2 \text{NH}_{3} \longrightarrow \, \underbrace{\hbox{SO$_{4}^{2-}$}}_{\hbox{Br$\o{}$nsted base}} + \text{2 NH}_{4}^{+}[/tex]

We see that the H₂SO₄ has lost two protons to become SO₄²⁻, so it is a Brønsted acid.

Answer:

0.02 moles of O₂ will be leftover.

Explanation:

The reaction is:

2NO(g) + O₂(g) → 2NO₂(g)    (1)

We have the mass of NO and O₂, so we need to find the number of moles:

[tex] n_{NO} = \frac{m}{M} = \frac{24.7 g}{30.01 g/mol} = 0.82 moles [/tex]

[tex] n_{O_{2}} = \frac{m}{M} = \frac{13.8 g}{31.99 g/mol} = 0.43 moles [/tex]

From equation (1) we have that 2 moles of NO reacts with 1 mol of O₂ to produce 2 moles of NO₂, so the excess reactant is:

[tex] n_{NO} = \frac{2}{1}*0.43 moles = 0.86 moles [/tex]          

[tex]n_{O_{2}} = \frac{1}{2}*0.82 moles = 0.41 moles[/tex]                                                                                

Hence, from above we can see that the excess reactant is O₂ since 0.41 moles react with 0.86 moles of NO and we have 0.43 moles in total for O₂.

The number of moles of excess reactant is:

[tex]n_{T} = 0.43 moles - 0.41 moles = 0.02 moles[/tex]  

Therefore, 0.02 moles of O₂ will be leftover.

I hope it helps you!                    

The number of moles of excess reactant that would be left over is 0.0197 mole

From the question,

We are to determine the number of moles of excess reactant that would be left over.

The given balanced chemical equation for the reaction is

2NO(g) + O₂(g) → 2NO₂ (g)

This means,

2 moles of NO is needed to completely react with 1 mole of O₂

Now, we will determine the number of moles of each reactant present

Mass = 24.7 g

Molar mass = 30.01 g/mol

From the formula

[tex]Number\ of\ moles = \frac{Mass}{Molar\ mass}[/tex]

∴ Number of moles of NO present = [tex]\frac{24.7}{30.01}[/tex]

Number of moles of NO present = 0.823059 mole

Mass = 13.8 g

Molar mass = 32.0 g/mol

∴ Number of moles of O₂ present = [tex]\frac{13.8}{32.0}[/tex]

Number of moles of O₂ present = 0.43125 mole

Since,

2 moles of NO is needed to completely react with 1 mole of O₂

Then,

0.823059 mole of NO is will react with completely react with [tex]\frac{0.823059 }{2}[/tex] mole of O₂

[tex]\frac{0.823059 }{2} = 0.4115295[/tex]

∴ Number of moles of O₂ that reacted is 0.4115295 mole

This means O₂ is the excess reactant and NO is the limiting reactant

Now, for the number of moles of excess reactant left over

Number of moles of excess reactant left over = Number of moles of O₂ present - Number of moles of O₂ that reacted

∴ Number of moles of excess reactant left over = 0.43125 mole - 0.4115295 mole

Number of moles of excess reactant left over = 0.0197205 mole

Number of moles of excess reactant left over ≅ 0.0197 mole

Hence, the number of moles of excess reactant that would be left over is 0.0197 mole

Learn more here: https://brainly.com/question/18757768

Answer:

1.7 ppm

Explanation:

Original amount N' = 2.6 ppm

time to testing t = 24 hr

final amount N = 2.1 ppm

Using exponential inhibited decay, we have

N = N'e^(-kt)

Where

N is the new reading

N' is the original reading

t is the decay time

k is the decay constant

Substituting, we have

2.1 = 2.6 x e^(-k x 24)

2.1 = 2.6 x e^(-24k)

0.808 = e^(-24k)

We take the natural log of both sides of the equation

Ln 0.808 = Ln (e^(-24k))

-0.213 = - 24k

K = 0.213/24 = 0.00886

After 48 hrs, the reading of free chlorine will be

N = 2.6 x e^(-0.00886 x 48)

N = 2.6 x e^(-0.425)

N = 2.6 x 0.654

N = 1.7 ppm

Answer: The initial rate of appearance of chlorite ion under those same conditions is [tex] 1.15\times 10^{-1}M/s[/tex]  

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

[tex]2ClO_2(aq)+2OH^-(aq)\rightarrow ClO_2^{-}(aq)+ClO_3^{-}(aq)+H_2O(l)[/tex]

 The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.

Rate in terms of disappearance of =  

Rate in terms of appearance of =  

The rate of disappearance of chlorine dioxide = [tex]2.30\times 10^{-1} M/s[/tex]

[tex]\frac{d[ClO_2]}{2dt}=\frac{d[ClO_2^{-}]}{dt}[/tex]  

[tex]\frac{2.30\times 10^{-1}}{2}=\frac{d[ClO_2^{-}]}{dt}[/tex]  

[tex]\frac{d[ClO_2^{-}]}{dt}=1.15\times 10^{-1}M/s[/tex]  

The initial rate of appearance of chlorite ion under those same conditions is [tex] 1.15\times 10^{-1}M/s[/tex]  

If the initial rate of disappearance of ClO₂ is 2.30 × 10⁻¹ M/s, the rate of appearance of ClO₂⁻ is 1.15 × 10⁻¹ M/s.

Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation:

2 ClO₂(aq) + 2 OH⁻(aq) → ClO₂⁻(aq) + ClO₃⁻(aq) + H₂O(l)

In this problem, we want to find an initial rate of reaction.

The rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time.

We can relate the rate of disappearance of ClO₂ and the rate of appearance of ClO₂⁻, using the molar ratios.

Molar ratios state the proportions of reactants and products that are used and formed in a chemical reaction.

The molar ratio of ClO₂ to ClO₂⁻ is 2:1.

If the initial rate of disappearance of ClO₂ is 2.30 × 10⁻¹ M/s, the rate of appearance of ClO₂⁻ is:

2.30 × 10⁻¹ mol ClO₂/L.s × (1 mol ClO₂⁻/2 mol ClO₂) = 1.15 × 10⁻¹ M/s

If the initial rate of disappearance of ClO₂ is 2.30 × 10⁻¹ M/s, the rate of appearance of ClO₂⁻ is 1.15 × 10⁻¹ M/s.

Learn more about rates of reaction here: https://brainly.com/question/8592296

Answer:

All three titrations require the same volume of NaOH to reach the first equivalence point.

Explanation:

Statements are:

All three titrations have the same final pH.

All three titrations require the same volume of NaOH to reach the first equivalence point.

All three titrations have the same pH at the first equivalence point.

All three titrations have the same initial pH.

The pH of the titration depends of the nature of the acid: If the acid is a strong acid, pH at the equivalence of the titration is 7. For a weak acid equivalence point depends of the nature of the conjugate base and initial pH of the weak acid. For a diprotic acid also depends of the nature of the acid.

Thus:

All three titrations have the same initial pH, All three titrations have the same pH at the first equivalence point. and All three titrations have the same final pH.  are the three FALSE.

As the concentrations of the acids is 0.10M and are titrated with 0.100M NaOH, The volume to reach the first equivalence point is the same for all the three acids.

Thus:

Answer:

16.7 mL

Explanation:

Convert 250 mL to L.

250 mL = 0.250 L

Calculate the amount of moles of NaOH in 250 mL of 0.300 M NaOH.

0.250 L × 0.300 M = 0.075 mol

Using this amount of moles, you need to find out what volume of 4.50 M will give you that many moles.  You can do this by dividing the amount of moles by the molarity.

(0.075 mol)/(4.50 M) = 0.0167 L

Convert from L to mL.

0.0167 L = 16.7 mL

Answer:

[tex]T_f=-2.58\°C[/tex]

Explanation:

Hello,

In this case, we can compute the the freezing point depression by using the following formula:

[tex]T_f-T_0=-i*m*Kf[/tex]

Whereas the freezing point of pure water is 0 °C van't Hoff factor for glucose is 1, the molality is computed as shown below and the freezing point constant of water is 1.86 °C/m:

[tex]m=\frac{25.0g\ glucose*\frac{1mol\ glucose}{180g\ glucose} }{100g*\frac{1kg}{1000g} }\\ \\m=1.39m[/tex]

Thus, the freezing point of the solution is:

[tex]T_f=T_0-i*m*Kf\\\\T_f=0\°C-1*1.39m*1.86\frac{\°C}{m}\\ \\T_f=-2.58\°C[/tex]

Regards.

The question is incomplete, the complete question is;

The 3d energy level in hydrogen has how many distinct states with different values of the quantum number m?

A. 3

B. 5

C. 6

D. 2

E. 4

Answer:

B. 5

Explanation:

The magnetic quantum number is used in describing the actual orientation of orbitals in space. The name 'magnetic quantum number' was coined because it describes the effect of different orientations of orbitals which was initially observed in the presence of an external magnetic field.

The d orbital can exhibit five orientations corresponding to five values of the magnetic quantum number, these are; -2,-1,0,1,2 hence the answer above.

Answer:

[tex]C_2=1.25 M[/tex]

Explanation:

Hello,

In this case, since the concentration in #1 is 3M, during a dilution process, the moles of the solute (NaCl) remains the same, just the concentration and volume change as shown below:

[tex]n_1=n_2\\\\C_1V_1=C_2V_2[/tex]

In such a way, as the final volume is 1200 microliters, the resulting concentration turns out:

[tex]C_2=\frac{C_1V_1}{V_2}=\frac{3M*500\mu L}{1200\mu L}\\ \\C_2=1.25 M[/tex]

Best regards.

Answer:

The answer is

To find the number of atoms of sodium we use the formula

N = n × L

where

n is the number of moles

N is the number of entities

L is Avogadro's constant which is

[tex]6.02 \times {10}^{23} [/tex]

We need to find the number of moles first

The formula is

[tex]n = \frac{m}{M} [/tex]

where

M is the molar mass

m is the mass

n is the number of moles

From the question

M = 22.9 g/mol

m = 51.0 g

[tex]n = \frac{51}{22.9} [/tex]

n = 2.227 moles

So the number of sodium atoms is

[tex]N = 2.227 \times 6.02 \times {10}^{23} [/tex]

We have the final answer as

Hope this helps you

Answer:

∆H is negative

∆S is negative

Explanation:

The condensation of CS2 implies a phase change from gaseous state to liquid state. The energy of the gaseous particles is greater than that of the liquid particles hence energy is given out when a substance changes from gaseous state to liquid state hence the process is exothermic and ∆H is negative.

Changing from gaseous state to liquid states leads to a decrease in entropy hence ∆S is negative. Liquid particles are more orderly than particles of a gas.

Answer:

the expected absorbance of the solution = 0.17

Explanation:

From the information given:

Using Beer's Lambert Law, we have

A = ∈CL

where;

A = Absorbance

∈ = extinction coefficient

C = concentration

L = cell length

Since Absorbance is associated with concentration.

Assuming the measurement were carried out in the same solution; Then  ∈ and L will be constant and A  ∝ C ----- (1)

Let consider the concentration to be C  (mol/L)

5.0 mL of a Sports Drink = 5.0 mL × C (mol)/1000 mL

= 5C/1000 mL

was diluted with water to 10.0 mL

So, when diluted with water to 10.0 mL; we have:

The new concentration to be : [tex]\dfrac{(5 C \times 1000) \ mol }{(1000 \times 10 \times 1000)\ mL}[/tex]

Since :1000mL = 1 L

The new concentration = [tex]\dfrac{C \ mol }{2 \ L}[/tex]

As stated that the initial absorbance reading [tex]A_1[/tex] = 0.34

The expected absorbance reading will be [tex]A_2[/tex] = ???

From (1)

A ∝ C

∴

[tex]\dfrac{A_2}{A_1}=\dfrac{C_2}{C}[/tex]

[tex]A_2 = \dfrac{A_1}{C}[/tex]

[tex]A_2 = \dfrac{0.34}{2}[/tex]

[tex]A_2 = 0.17[/tex]

Thus ; the expected absorbance of the solution = 0.17

Answer:

Equilibrium constant expression for [tex]\rm 2\; H^{+}\, (aq) + {CO_3}^{2-}\, (aq) \rightleftharpoons H_2CO_3\, (aq)[/tex]:

[tex]\displaystyle K = \frac{\left(a_{\mathrm{H_2CO_3\, (aq)}}\right)}{\left(a_{\mathrm{H^{+}}}\right)^2\, \left(a_{\mathrm{{CO_3}^{2-}\, (aq)}}\right)} \approx \frac{[\mathrm{H_2CO_3}]}{\left[\mathrm{H^{+}\, (aq)}\right]^{2} \, \left[\mathrm{CO_3}^{2-}\right]}[/tex].

Where

Explanation:

The equilibrium constant expression of a (reversible) reaction takes the form a fraction.

Multiply the activity of each product of this reaction to get the numerator.[tex]\rm H_2CO_3\; (aq)[/tex] is the only product of this reaction. Besides, its coefficient in the balanced reaction is one. Therefore, the numerator would simply be [tex]\left(a_{\mathrm{H_2CO_3\, (aq)}}\right)[/tex].

Similarly, multiply the activity of each reactant of this reaction to obtain the denominator. Note the coefficient "[tex]2[/tex]" on the product side of this reaction. [tex]\rm 2\; H^{+}\, (aq) + {CO_3}^{2-}\, (aq)[/tex] is equivalent to [tex]\rm H^{+}\, (aq) + H^{+}\, (aq) + {CO_3}^{2-}\, (aq)[/tex]. The species [tex]\rm H^{+}\, (aq)[/tex] appeared twice among the reactants. Therefore, its activity should also appear twice in the denominator:

[tex]\left(a_{\mathrm{H^{+}}}\right)\cdot \left(a_{\mathrm{H^{+}}}\right)\cdot \, \left(a_{\mathrm{{CO_3}^{2-}\, (aq)}})\right = \left(a_{\mathrm{H^{+}}}\right)^2\, \left(a_{\mathrm{{CO_3}^{2-}\, (aq)}})\right[/tex].

That's where the exponent "[tex]2[/tex]" in this equilibrium constant expression came from.

Combine these two parts to obtain the equilibrium constant expression:

[tex]\displaystyle K = \frac{\left(a_{\mathrm{H_2CO_3\, (aq)}}\right)}{\left(a_{\mathrm{H^{+}}}\right)^2\, \left(a_{\mathrm{{CO_3}^{2-}\, (aq)}}\right)} \quad\begin{matrix}\leftarrow \text{from products} \\[0.5em] \leftarrow \text{from reactants}\end{matrix}[/tex].

In dilute solutions, the equilibrium constant expression can be approximated with the concentrations of the aqueous "[tex](\rm aq)[/tex]" species. Note that all the three species here are indeed aqueous. Hence, this equilibrium constant expression can be approximated as:

[tex]\displaystyle K = \frac{\left(a_{\mathrm{H_2CO_3\, (aq)}}\right)}{\left(a_{\mathrm{H^{+}}}\right)^2\, \left(a_{\mathrm{{CO_3}^{2-}\, (aq)}}\right)} \approx \frac{\left[\mathrm{H_2CO_3\, (aq)}\right]}{\left[\mathrm{H^{+}\, (aq)}\right]^2\cdot \left[\mathrm{{CO_3}^{2-}\, (aq)}\right]}[/tex].

Answer:

Pure substance:

Mixtures:

Explanation:

Pure substances exists as either elements or compounds.

A homogeneous mixture has even distribution and a single phase composition of its constituents; whereas heterogeneous mixtures are not uniform and constituents exist in different phases.

Answer:

B. CH_3 CH_2 CH_2 F

Explanation:

The alkyl group contains all univalent group derived from alkanes by the loss of a hydrogen atom. When an alkyl group combines or is bonded with an halogen  family (such as Flourine, Chlorine , Bromine , Iodine) , we have an alkyl halide such as the options given in the question.

Alkyl  halide bond with an sp³ Carbon. Depending on where the halide is bonded to , we can have the primary halide, secondary halide and the tertiary halide.

When alkyl halide react with magnesium metal, we have a reaction that is known as Grignard Reaction. The order of reactivity of alkyl halide with grignard reagents is :

F < Cl < Br < I .

This is because of the nature of the electronegativity and the bond strength.

As we move than the group from the top to the bottom, the electronegativity decreases and the bond strength increase, so as the size. Thus, this is exactly what the reactivity of alkyl halide with Grignard reaction is established for.

Thus since the fluorine have the highest electronegativity and the smallest bond size in the halogen family , then it will be the least reactive alkyl halide in reacting with magnesium metal.

Answer:  The molar mass of butane will be [tex]11.2\times 10^{7}g[/tex]

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP, contains avogadro's number [tex]6.023\times 10^{23}[/tex] of particles. and weighs equal to the molar mass.

To calculate the moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given molecules}}{\text {avogadro's number}}=\frac{4.49\times 10^{16}}{6.023\times 10^{23}}=0.74\times 10^{-7}moles[/tex]

Now [tex]0.74\times 10^{-7}moles[/tex]  weigh = 8.29 g

Thus 1 mole will weigh = [tex]\frac{8.29}{0.74\times 10^{-7}}\times 1=11.2\times 10^{7}g[/tex]

The molar mass of butane will be [tex]11.2\times 10^{7}g[/tex]

Answer:

TRUE.

Explanation:

Hello,

In this case, since the fusion enthalpy of ice is +333.9 J/g and the fusion entropy is defined as:

[tex]\Delta _{fus}S=\frac{m*\Delta _{fus}H}{T_{fus}}[/tex]

We can compute it considering the temperature (0 °C) in kelvins:

[tex]\Delta _{fus}S=\frac{20.6g*333.9J/g}{(0+273)K}\\\\\Delta _{fus}S=25.2J/K[/tex]

Therefore answer is TRUE.

Best regards.