Answer:
Laboratory is a place where all the experiments are to be done by the students or teachers so it should be safe and clean. I will not allow anyone inside until the glass peaces are cleaned
A patient is prescribed 100mg/day of antibiotic for two weeks. The antibiotic is available in vials that contain 20mg/vial of the drug. How many vials are necessary for the entire treatment?
Answer:
70
Explanation:
100/20 =5
5 x each day over 2 weeks (14 days) = 70
The vials are necessary for the entire treatment is 70 vials
We have to first calculate the total number of antibiotics taken by the patient in two weeks, then find the total vials neccessary for the entire treatment.
The total antibiotics for a period of two weeks = (100 mg/day)(2 weeks)
Total = 100 mg/day×14 days
Total = 1400 mg for two weeks.
If the antibiotics contain vials in 20 mg/vials of the drugs,
Then the vials necessary for the entire treatment is
vial for the entire treatment = 1400/20
total vials = 70 vials
Hence the vials are necessary for the entire treatment is 70 vials
Learn more about vials here : https://brainly.com/question/11861753
QUICK WILL MARK BRAINLIEST!!
Match each of the unknown ions to its appropriate description.
A− A) A nonmetal that gained one electron
B+ B) A metal that lost one electron
C2− C) A metal that lost two electrons
D2+ D) A nonmetal that gained two electrons
Answer:
c2-c
Explanation:
A mental that lost two electrons just joking I don't k ow but I think it ain't the first o e because of comment sense to the 5th power
Answer:
A and B
Explanation:
metal form ion by lossing elecron
non metal form ion by gaining electron
Hydrogen was collected over water using the approach in the manual. The water temperature was 220C and the measured pressure inside the tube was determined to be 715mmHg. Use Appendix F in your lab manual to determine the pressure of the collected hydrogen gas.
Answer:
Pressure of hydrogen gas = 695.2 mmHg
Explanation:
Given:
Water temperature = 22°C
Pressure inside the tube = 715 mmHg
Find:
Pressure of hydrogen gas
Computation:
Using vapor pressure of water table
Water pressure at 22°C = 19.8 mmHg
Pressure inside the tube = Pressure of hydrogen gas + Water pressure at 22°C
715 = Pressure of hydrogen gas + 19.8
Pressure of hydrogen gas = 715 - 19.8
Pressure of hydrogen gas = 695.2 mmHg
Is it a spontaneous or non-spontaneous change?
During an exothermic chemical reaction, two moles of gaseous reactants are turned into four moles of gaseous products.
Spontaneous Non-spontaneous
During an endothermic chemical reaction, four moles of gaseous reactants are turned into two moles of gaseous products.
Spontaneous Non-spontaneous
A gas expands without absorbing or releasing heat.
Spontaneous Non-spontaneous
What volume of a 0.124 M KOH solution neutralizes 23.4 mL of 0.206 M HCl solution?
A) 15.9 mL
B) 38.9 mL
C) 31.8 mL
D) 1.00 × 104 mL
E) 5.00 × 102 mL
The volume of KOH required for the neutralization of acid has been 38.9 ml. Thus, option B is correct.
Neutralization reaction has resulted in the formation of salt and water with the reaction of acid and base.
In the neutralization reaction, the strength of the acid and base can be given by:
Molarity of acid [tex]\times[/tex] Volume of acid = Molarity of base [tex]\times[/tex] Volume of base
Given, the molarity of KOH base = 0.124 M
The volume of acid (HCl) = 23.4 ml
Molarity of acid (HCl) = 0.206 M.
Substituting the values:
0.206 [tex]\times[/tex] 23.4 = 0.124 × Volume of base (KOH)
Volume of base (KOH) = 38.874 ml.
Volume of KOH = 38.9 ml
The volume of KOH required for the neutralization of acid has been 38.9 ml. Thus, option B is correct.
For more information about neutralization reaction, refer to the link:
https://brainly.com/question/9691296
Identify if the following are chemical or physical properties: "CP" for
chemical property and "PP" for physical property
1. Oxygen is odorless and colorless
2. Copper turns green when exposed to the environment
3. The piece of metal is magnetic
4. The density of water is 1.0 g/cm3
5. Diamonds are a very hard substance
6. The tree is 8 meters high
Answer:
1.pp
2.cp
3.pp
4.pp
5.pp
6.pp
What is the maximum number of moles of nickel carbonate (NiCO3) that can form during the precipitation reaction
Answer:
The correct answer is : 0.025.
Explanation:
The precipitation reaction is as follows in this procedure:
NiSO4.6H20 (aq) + Na2CO3.10H2O (aq)⇒ NiCO3 (s) + Na2SO4 (aq) + 16H2O
So, the number of moles of reactants can be found by
number of moles : mass used/ molar mass
n (NiSO4×6H2O) = (6.57 g)/(262.84 g/mol) = 0.025 mol (for Ni)
n (Na2CO3×10H2O) = (7.15 g)/(286.14 g/mol) = 0.0250 mol (for CO3).
Thus, The maximum number of moles of NiCO3 that can form is 0.025 mol.
What areas of the work force can science be applied to?
Select all that apply
Answer:
1. the study of the structure, properties, and interactions of materials and the changes they undergo
2. the study of matter and energy and how they interact
3. the systematic study and analysis of facts
4. a process to test a proposed solution to a problem
Click again to see term
Until the 1600s, people who investigated problems related to our understanding of the natural world were called _____.
Click ca
Explanation:
What is the wavelength of radiation emitted when an electron goes from the n = 7 to the n = 4 level of the Bohr hydrogen atom? Give your answer in nm.
Answer:
the wavelength of radiation emitted is [tex]\mathbf{\lambda= 2169.62 \ nm}[/tex]
Explanation:
The energy of the Bohr's hydrogen atom can be expressed with the formula:
[tex]\mathtt{E_n =- \dfrac{13.6\ ev}{n^2}}[/tex]
For n = 7:
[tex]\mathtt{E_7 =- \dfrac{13.6\ ev}{7^2}}[/tex]
[tex]\mathtt{E_7 =-0.27755 \ eV}[/tex]
For n = 4
[tex]\mathtt{E_4=- \dfrac{13.6\ ev}{4^2}}[/tex]
[tex]\mathtt{E_4 =- 0.85\ eV}[/tex]
The electron goes from the n = 7 to the n = 4, then :
[tex]\mathtt{E_7-E_4 = (-0.27755 - (-0.85) ) \ eV}[/tex]
[tex]\mathtt{= 0.57245\ eV}[/tex]
Wavelength of the radiation emitted:
[tex]\mathtt{\lambda= \dfrac{hc}{0.57245 \ eV}}[/tex]
where;
hc = 1242 eV.nm
[tex]\mathtt{\lambda= \dfrac{1242 \ eV.nm }{0.57245 \ eV}}[/tex]
[tex]\mathbf{\lambda= 2169.62 \ nm}[/tex]
Which particle j j Thomson discovered
Sir Joseph John Thomson OM PRS (18 December 1856 – 30 August 1940) was a British physicist and Nobel Laureate in Physics, credited with the discovery of the electron, the first subatomic particle to be discovered.
how does heat flow in air and ocean currents
Answer:
the transfer of heat energy within the atmosphere, hydrosphere, and the earth's surface and interior occurs as a result of radiation, convection, and conduction. ocean currents play a significant role in transferring this heat toward the poles.
Use the balanced chemical equation below. How many grams of the product are formed when 2.34 g of sulfur is completely reacted with fluorine? S8 + 16F2(g) → 8SF4
Answer:
7.89 g
Explanation:
Step 1: Write the balanced equation
S₈ + 16 F₂(g) → 8 SF₄
Step 2: Calculate the moles corresponding to 2.34 g of S₈
The molar mass of S₈ is 256.52 g/mol.
[tex]2.34g \times \frac{1mol}{256.52g} = 9.12 \times 10^{-3} mol[/tex]
Step 3: Calculate the moles of SF₄ produced from 9.12 × 10⁻³ mol of S₈
The molar ratio of S₈ to SF₄ is 1:8. The moles of SF₄ produced are 8/1 × 9.12 × 10⁻³ mol = 0.0730 mol
Step 4: Calculate the mass corresponding to 0.0730 moles of SF₄
The molar mass of SF₄ is 108.07 g/mol.
[tex]0.0730 mol \times \frac{108.07 g}{mol} = 7.89 g[/tex]
A sample of 23.2 g of nitrogen gas is reacted with
23.2 g of hydrogen gas to produce ammonia, NH3.
Using the balanced equation below, what is the
maximum amount, in moles, of ammonia that can be
produced?
N2 + 3H2
2NH3
IN
[?] moles NH3
Answer:
1.66 moles.
Explanation:
We'll begin by calculating the number of mole in 23.2 g of nitrogen gas, N2.
This is illustrated below:
Molar mass of N2 = 2x14 = 28 g/mol
Mass of N2 = 23.2 g
Mole of N2 =.?
Mole = mass /Molar mass
Mole of N2 = 23.2/28
Mole of N2 = 0.83 mole
Next, we shall determine the number of mole in 23.2 g of Hydrogen gas, H2.
This is illustrated below:
Molar mass of H2 = 2x1 = 2 g/mol
Mass of H2 = 23.2 g
Mole of H2 =?
Mole = mass /Molar mass
Mole of H2 = 23.2/2
Mole of H2 = 11.6 moles
Next, the balanced equation for the reaction. This is given below:
N2 + 3H2 —> 2NH3
From the balanced equation above,
1 mole of N2 reacted with 3 moles of H2 to produce 2 moles of NH3.
Next, we shall determine the limiting reactant. This can be obtained as follow:
From the balanced equation above,
1 mole of N2 reacted with 3 moles of H2.
Therefore, 0.83 moles will react with = (0.83 x 3) = 2.49 moles of H2.
From the calculations made above, we can see that only 2.49 moles out of 11.6 moles of H2 is required to react completely with 0.83 mole of N2.
Therefore, N2 is the limiting reactant.
Finally, we shall determine the maximum amount of NH3 produced from the reaction.
In this case, we shall use the limiting reactant because it will give the maximum yield of NH3 since all of it is consumed in the reaction.
The limiting reactant is N2 and the maximum amount of NH3 produced can be obtained as follow:
From the balanced equation above,
1 mole of N2 reacted to produce 2 moles of NH3.
Therefore, 0.83 mole of N2 will react to produce = (0.83 x 2) = 1.66 moles of NH3.
Therefore, the maximum amount of NH3 produced from the reaction is 1.66 moles.
Gold atoms form small clusters containing a fixed number of atoms. What is the mass (in grams) of oneAu31 cluster
Answer:
[tex]m_{Au_{31}}=6106.07 g[/tex]
Explanation:
Hello,
In this case, since one gold atom has a mass of 196.97 g, for the given gold cluster that has 31 gold atoms, the mass will be:
[tex]m_{Au_{31}}=31*196.97g\\\\m_{Au_{31}}=6106.07 g[/tex]
Whereas we consider the mass of all the 31 gold atoms to compute the overall mass.
Best regards.
Answer:
The mass (in grams) of one Au31cluster = [tex]1.014*10^{-20}grams[/tex]Explanation:
Atomic mass of Au = 197u
So, mass of 1 Au31 cluster (in u)
[tex]= 197 * 31\\\\= 6107u[/tex]
So, mass of 1 Au31 cluster (in gram)
[tex]= 6107 * 1.66*10^{-24}\\\\= 1.014*10^{-20}grams[/tex]
For more information, visit
https://brainly.com/subject/chemistry
In an electrolytic cell, the magnitude of the standard cell potential is the:______
a. minimum voltage that must be supplied for a redox reaction to occur
b. maximum voltage that willallow the redox reaction to occur
c. always equal to Eanode - Ecathode
d. none of the above
Answer:
a. minimum voltage that must be supplied for a redox reaction to occur
c. always equal to Eanode - Ecathode
Explanation:
In an electrolytic cell; The electromotive force(the maximum standard potential difference) of the cell formed by the system is defined as the standard electrode potential of the right handed electrode minus the standard electrode potential of the left hand electrode. (i.e [tex]\mathbf{E^{\theta}_{cell}=E_{anode} - E_{cathode}}[/tex] )
As we all known that the process by which chemical energy is being converted to electrical energy is called the Electrochemical cell. It consists of two half cells , an oxidation half cell reaction and a reduction half-cell reaction.The overall redox reaction results in a flow of electrons in an electric current which is produced by a minimum voltage.
Therefore, option a and c are both correct.
Draw the structure of the amine and carboxylic acid reactants required to form the following amide in an amidation reaction.Draw the starting amine. Be sure to draw nonbonding electron pairs.
Draw the starting carboxylic acid. Be sure to draw nonbonding electron pairs.
Answer:
Explanation:
Amidation is a reaction with the formation of an amide. It involves a process where series of reaction between amine and carboxylic acid takes place.
The main objective of this question is to draw with the aid of a diagram.
the structure of the amine and carboxylic acid reactants required to form the following amide in an amidation reaction.
But before that,
we are to draw the starting amine and to be sure to include the nonbonding electron pairs.
Also, to draw starting carboxylic acid and to be sure to include the nonbonding electron pairs.
The whole series of the diagrammatic expression for the amine formation can be found in the diagram attached below.
Which species have the same electron arrangements?
I. O2-, F-. Ne
II. Li+, Na+, K+
III. S2-, Ar, K+
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
Answer:
the answer will be B.1 and 3 only
Explanation:1. O2- means it has in total 10 electrons as atomic no of oxygen is 8
again F- has also 10 electrons as flourine has atomic no 9
and neon also has 10 electrons
incase of 3rd no S2- has 18 electrons as atomic no of sulfur is 16 as its an ion so it will take 2 more electrons
argon is an inert gas so it has 18 electrons and potassium has 19 electrons eliminating 1 we will 18
# incase of the second option lithium + contains 2 electrons and Na+ contains 10 and K+ contains 18 electrons so all of them are not same
ANS is 1 and 3 only(B.i and iii) only
thank u
Calculate the solubility at of AgCl in pure water and in a ).0010 M solution. You'll find data in the ALEKS Data tab. Round both of your answers to significant digits.
Answer:
1.34x10⁻⁵ mol / L is the solubility of AgCl
Explanation:
Ksp of AgCl is defined as:
AgCl(s) ⇄ Ag⁺(aq) + Cl⁻(aq)
If 0.010M of AgCl is added, some Ag⁺ and Cl⁻ will be produced until:
Ksp = [Ag⁺] [Cl⁻]
Ksp for AgCl = 1.8x10⁻¹⁰ (Taken from ALEKS Data tab):
Some Ag⁺ and Cl⁻ are produced, you can take this "some" as X:
[Ag⁺] = X
[Cl⁻] = X
Where X is the amount of AgCl that dissolvesin water. X = solubility:
Ksp = 1.8x10⁻¹⁰ = [Ag⁺] [Cl⁻]
1.8x10⁻¹⁰ = [X] [X]
1.8x10⁻¹⁰ = X²
X =
1.34x10⁻⁵ mol / L is the solubility of AgCl
Question 7
How many molecules of water are in 0.042 Lof pure water (ignoring any temperature
effect)?
Express your answerin e-notation using as many decimal places as necessary
Example: 1,000,001 should be expressed as 1.000001e+6
Notes: Avogadro's constant = 6.02214076e+23 mol 1
Explanation:
Moles of 0.042 L of Pure water = 0.042 / 22.4
[tex]Moles \: of \: 0.042 L \: of \: Pure \: water \: = 1.87 \times {10}^{ - 3} [/tex]
[tex]Molecules \: in \: 0.042 L \: of \: Pure \: water \: = moles \times avogadro \: number[/tex]
Molecules in 0.042 L of Pure Water
= 1.126 * 10^21
What are 1A, 3B, and 7A examples of on the periodic table?
Answer:
Groups
Explanation:
1 A, 3 B, and 7 A are examples of group number on the periodic table
Group 1A are the alkali metals includes lithium sodium and potassium.
Group 3B in most periodic tables, lanthanum and actinium are considered to be a part of Group3B.
Group 7A are the halogens includes chlorine ,bromine and iodine.
What are some characteristics of Group1A elements ?
They are all soft, silver metals. Due to their low ionization energy, these metals have low melting points and are highly reactive. The group 1A elements with their ns1 valence electron configurations are very active metals. They lose their valence electrons very readily.
All the Group 3B elements are rather soft, silvery-white metals, although their hardness increases with atomic number. They have higher ionization energies than the Group 1A and 2A elements, and are ionized to form a 3+ charges.
They have very high electronegativity. They have seven valence electrons . They are highly reactive, especially with alkali metals and alkaline earths metals.
Learn more about Group 1A,Group 3B and Group 7A,here:
https://brainly.com/question/2826808
#SPJ6
What mass (in grams) of aspirin (C₉H₈O₄) is produced from 57.6 g of C₇H₆O₃ assuming 95.0% yield from the reaction below? C₇H₆O₃ (s) + C₄H₆O₃ (s) → C₉H₈O₄ (s) + HC₂H₃O₂ (aq).
Answer:
71.3 g
Explanation:
molar mass of C₇H₆O₃ = 138.13 g
molar mass of [tex]C_{9}H_{8}O_{4}[/tex] = 180.17 g
find the moles of reactant: C₇H₆O₃
C₇H₆O₃ that reacted = mass/molar mass = 57.6 g C₇H₆O₃ / 138.13 g C₇H₆O₃
= 0.417 mol [tex]C_{7}H_{6}O_{3}[/tex]
From the reaction equation, 1 mole of C₇H₆O₃ yields one mole of aspirin
find theoretical yield of aspirin:
0.417 mol C7H6O3 x 180.17 g C9H8O4 / 1 mol C9H8O4[tex]\frac{0.417 mol C_{7}H_{6}O_{3}}{} x \frac{180.17 g C_{9}H_{8}O_{4}}{1 mol C_{9}H_{8}O_{4}}[/tex]
= 75.1 g C9H8O4
Actual yield= % yield × theoretical yield/100
Actual yield = 95.0 × 75.1/100
Actual yield = 71.3 g
Taking into account the reaction stoichiometry and actual yield, the mass of C₉H₈O₄ produced from 57.6 g of C₇H₆O₃ assuming 95.0% yield is 57.0285 grams.
The balanced reaction is:
22 C₇H₆O₃ (s) + 32 C₄H₆O₃ (s) → 24 C₉H₈O₄ (s) + 33 HC₂H₃O₂ (aq)
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
C₇H₆O₃: 22 moles C₄H₆O₃: 32 moles C₉H₈O₄: 24 moles HC₂H₃O₂: 33 molesThe mass molar of each compound is:
C₇H₆O₃: 138 g/moleC₄H₆O₃: 102 g/mole C₉H₈O₄: 180 g/moleHC₂H₃O₂: 60 g/moleThen by reaction stoichiometry, the following amounts of mass of each compound participate in the reaction:
C₇H₆O₃: 22 moles× 138 g/mole= 3036 gramsC₄H₆O₃: 32 moles× 102 g/mole= 3264 grams C₉H₈O₄: 24 moles× 180 g/mole= 4320 gramsHC₂H₃O₂: 33 moles× 60 g/mole= 1980 gramsThen you can apply the following rule of three: if by stoichiometry 3036 grams of C₇H₆O₃ produce 3264 grams of C₉H₈O₄, 57.6 grams of C₇H₆O₃ will produce how many mass of C₉H₈O₄?
[tex]mass of C_{9} H_{8} O_{4} =\frac{57.6 grams of C_{7} H_{6} O_{3} x3264 gramsof C_{9} H_{8} O_{4} }{3036 grams of C_{7} H_{6} O_{3}}[/tex]
mass of C₉H₈O₄= 60.03 grams
On the other side, actual yield is the amount of product actually obtained from a reaction. Assuming 95.0% yield and considering the previously calculated mass the maximum amount of product that can be produced in the reaction, you can apply the following rule of three: If 100% equals 60.03 grams of the compound produced, 95% equals how much mass of the compound?
[tex]mass of C_{9} H_{8} O_{4} =\frac{95 percentx60.03gramsof C_{9} H_{8} O_{4} }{100 percent}[/tex]
mass of C₉H₈O₄= 57.0285 grams
Finally, the mass of C₉H₈O₄ produced from 57.6 g of C₇H₆O₃ assuming 95.0% yield is 57.0285 grams.
Learn more:
brainly.com/question/16487206?referrer=searchResults brainly.com/question/14446695?referrer=searchResults brainly.com/question/11564309?referrer=searchResults brainly.com/question/4025026?referrer=searchResults brainly.com/question/18650135?referrer=searchResultsBRAINLIeSt TO FIRST Which is a correct method used in a scientific experiment involving acid and base solutions? (2 points) Select one: a. Using a pH test strip to measure the oxygen content of a solution b. Adding an indicator to a solution to test its acidity c. Adjusting the recorded pH measurements to prove the hypothesis d. Measuring the pH of a test strip by dipping it into an indicator
Answer:
B, adding an indicator to a solution to test its acidity
Explanation:
Answer:
B - Adding an indicator to a solution to test its acidity
Explanation:
Took the test
Of the following solutions, which has the greatest buffering capacity?
a. 0.365M HC2H3O2 and 0.497 M NaC2H3O2
b. 0.521 M HC2H3O2 and 0.217 M NaC2H3O2
c. 0.821 M HC2H3O2 and 0.713 M NaC2H3O2
d. 0.121 M HC2H3O2 and 0.116 M NaC2H3O2
Answer:
d. 0.121 M HC2H3O2 and 0.116 M NaC2H3O2
Explanation:
Hello,
In this case, since the pH variation is analyzed via the Henderson-Hasselbach equation:
[tex]pH=pKa+log(\frac{[Base]}{[Acid]} )[/tex]
We can infer that the nearer to 1 the ratio of of the concentration of the base to the concentration of the acid the better the buffering capacity. In such a way, since the sodium acetate is acting as the base and the acetic acid as the acid, we have:
a. [tex]\frac{[Base]}{[Acid]}=\frac{0.497M}{0.365M}=1.36[/tex]
b. [tex]\frac{[Base]}{[Acid]}=\frac{0.217M}{0.521M}=0.417[/tex]
c. [tex]\frac{[Base]}{[Acid]}=\frac{0.713M}{0.821M}=0.868[/tex]
d. [tex]\frac{[Base]}{[Acid]}=\frac{0.116M}{0.121M}=0.959[/tex]
Therefore, the d. solution has the best buffering capacity.
Regards.
Which statement explains why spontaneous generation is a mistaken idea? A. Living things do not need to reproduce. B. Living things are produced only by living things. C. Not all living things can maintain homeostasis. D.All living things exhibit binomial nomenclature.
From the following list of observations, choose the one that most clearly supports the conclusion that electrons have wave properties.
A) the emission spectrum of hydrogen
B) the photoelectric effect
C) the scattering of alpha particles by metal foil
D) diffraction
E) cathode "rays"
Answer:
diffraction
Explanation:
Louis de Broglie in 1924 proposed the idea of wave particle duality. In his proposition, matter could exhibit wavelike properties.
Electrons are generally regarded as particles. Electrons may also display wavelike properties such as diffraction patterns. Generally, diffraction is regarded as a property of waves.
Hence, electron diffraction effect owes to the wavelike nature of of electrons when they are passed near matter.
2. Which of these is an extensive property?
a. Density
b. Melting point
Temperature
d. Volume
Volume ..........is the answer
Mass and energy are conserved Question 13 options: A) only in chemical changes. B) always in physical changes and sometimes in chemical changes. C) only in physical changes. D) in chemical changes and physical changes.
Answer:
D) in chemical changes and physical changes.
Explanation:
Mass and energy are conserved in chemical changes and physical changes. Therefore, option D is correct.
What is physical change ?Physical modifications are those that affect a chemical substance's form but not its chemical content. Physical changes may normally be used to separate compounds into chemical elements or simpler compounds, but they cannot be used to separate mixtures into their component compounds.
A change in physical attributes accompanies a physical change. Melting, turning into a gas, changing strength or durability, changing crystal structure or texture, and changing shape, size, color, volume, or density are a few examples of physical qualities.
In a physical change, the substance's shape or appearance changes, but the type of matter it contains stays the same. In contrast, when matter undergoes a chemical transformation, at least one new substance with novel features is created.
Thus, option D is correct.
To learn more about physical change, follow the link;
https://brainly.com/question/3680148
#SPJ2
How many moles of Al are necessary to form 23.6 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) → 2 AlBr₃(s) ?
Answer:
0.088 mole of Al.
Explanation:
First, we shall determine the number of mole in 23.6 g of AlBr₃.
This is illustrated below:
Mass of AlBr₃ = 23.6 g
Molar Mass of AlBr₃ = 27 + 3(80) = 267 g/mol
Mole of AlBr₃ =.?
Mole = mass/Molar mass
Mole of AlBr₃ = 23.6 / 267
Mole of AlBr₃ = 0.088 mol
Next, we shall writing the balanced equation for the reaction.
This is given below:
2Al(s) + 3Br₂(l) → 2AlBr₃(s)
From the balanced equation above,
2 moles of Al reacted with 3 mole of Br₂ to 2 moles AlBr₃.
Finally, we shall determine the number of mole of Al needed for the reaction as follow:
From the balanced equation above,
2 moles of Al reacted to 2 moles AlBr₃.
Therefore, 0.088 mole of Al will also react to produce 0.088 mole of AlBr₃.
0.085 moles of Al are required to form 23.6 g of AlBr₃.
Let's consider the following balanced equation for the synthesis reaction of AlBr₃.
2 Al(s) + 3 Br₂(l) → 2 AlBr₃(s)
First, we will convert 23.6 g to moles using the molar mass of AlBr₃ (266.69 g/mol).
[tex]23.6 g \times \frac{1mol}{266.69g} = 0.0885 mol[/tex]
The molar ratio of Al to AlBr₃ is 2:2. The moles of Al required to form 0.0885 moles of AlBr₃ are:
[tex]0.0885molAlBr_3 \times \frac{2molAl}{2molAlBr_3} = 0.0885molAl[/tex]
0.085 moles of Al are required to form 23.6 g of AlBr₃.
You can learn more about stoichiometry here: https://brainly.com/question/22288091
A scuba diver goes deeper underwater the diver must be aware that the increased pressure affects the human body be increasing the
Answer:
The amount of dissolved gases in the body. Have a good day! =)
Explanation:
What is the concentration of a dextrose solution prepared by diluting 16 mL of a 1.0 M dextrose solution to 25 mL using a 25 mL volumetric flask?
Answer:
0.64 M
Explanation:
Step 1: Given data
Initial concentration (C₁): 1.0 MInitial volume (V₁): 16 mLFinal concentration (C₂): ?Final volume (V₂): 25 mLStep 2: Calculate the final concentration of the dextrose solution
We want to prepare a diluted solution from a concentrated one. We can find the final concentration using the dilution rule.
C₁ × V₁ = C₂ × V₂
C₂ = C₁ × V₁ / V₂
C₂ = 1.0 M × 16 mL / 25 mL
C₂ = 0.64 M