The bottle should relabel as bromine i.e option B
Why bromine is a liquid?
The presence of strong intermolecular interactions prevents bromine from evaporating, Therefore bromine is a liquid.
As it is mentioned in the question, the unidentified element is in a liquid state and is non-metallic. Therefore, it can not be other than bromine due to the following reasons.
• Chlorine and helium both always exist as a gas. So, can not be a liquid
• Arsenic is a metal
Hence, option B is left only and which is correct too.
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An atom of Astatine-214, 21485At, undergoes alpha-decay. Using the chart above, what new isotope will be produced?
If the atom of Astatine-214 undergo alpha particle, it will emit helium element as shown;
[tex]_{85}^{214}At\rightarrow_{83}^{210}Bi+_2^4He[/tex]According to the decay, 4 is subtracted from the mass number and 2 from the atomic number.
According to the reaction, the new isotope produced is Bismuth-210
which of the following have expressions has a product of 36
Answer:
3/4
Explanation:
Everybody wants to be us.
Alkalai Metals
Alkalai Earth Metals
Noble Gasses
Halogens
Answer:
Noble Gases
Explanation:
For this question, what does one of them have that the others don't?
Alkali Metals - These are in column 1 of the periodic table. They are the ones that have a charge of positive 1 since they give away their 1 electron in order to be stable.
Alkali Earth Metals - These are in column 2 of the periodic table. They are the ones that have a charge of positive 2 since they give away their 2 electrons in order to be stable.
Noble Gases - These are the elements in the last column of the periodic table. These elements do not need to give away or accept electrons because they are complete and stable!
Halogens - These are in column 17 in the periodic table. They are right next to the halogens, but still are not complete as they need 1 more electron in order to be stable. These elements have a charge of -1 because they take away an electron from another element (mainly the alkali metals) in order to be stable.
So, based off of their definitions, the only ones that do not need to gain or lose electrons are the noble gases. This is because they are complete and stable, the only ones out of these that do not need anything.
What is the Lewis structure for butyl thiol (CH3CH2CH2CH2SH)?
The Lewis dot structure for butyl thiol.
Lewis systems, also called Lewis dot formulas, Lewis dot systems, electron dot structures, or Lewis electron dot structures, are diagrams that display the bonding among atoms of a molecule, as well as the lone pairs of electrons that could exist inside the molecule.
A Lewis structure is based totally on the idea of the octet rule, in which atoms share electrons so that each atom has 8 electrons in its outer shell. for example, an oxygen atom has six electrons in its outer shell.
A Lewis shape is a totally simplified representation of the valence shell electrons in a molecule. it is used to expose how the electrons are arranged around man or woman atoms in a molecule. Electrons are shown as "dots" or for bonding electrons as a line between the 2 atoms
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How many calories are provided by a medium sized quarter pounder with cheese value meal from McDonald’s. The nutrition information is provided below?
protein: 28
carbs: 38
fat: 30
The calories provided by a medium sized quarter pounder with cheese value meal from McDonald’s is 1050 calories.
What is carbohydrate?Carbohydrate are defined as carbon, hydrogen, and oxygen atoms make up biomolecules. They are a vital source of energy.
Carbohydrates supply the body with glucose, which is converted into energy for use.
There are three main types of carbohydrates.
SugarStarch FiberProteins are defined as the large biomolecules and macromolecules consisting of one or more long chains of amino acid residues.
There are seven types of proteins.
AntibioticContractile proteinsEnzymesHormonal proteinsStructural proteinsStorage proteins Transport proteinsFats are defined as the triglycerides are macronutrient compounds that are an important part of our diet, along with carbohydrates, vitamins, and protein.
Thus, the calories provided by a medium sized quarter pounder with cheese value meal from McDonald’s is 1050 calories.
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Balance the following redox reactions by inspection:
a) KCl(s) + O2(g) --> KClO3
b) NH3(g) + O2(g) --> NO(g) + H2O(g)
To see the number of atoms of any element in a molecule multiply the stoichiometry of that molecule to the number that is written on the foot of that element in that molecule the balanced equation are
[tex]2KCL+3O_{2} \rightarrow 2KClO_{3}[/tex]
[tex]2NH_{3} +\frac{5}{2} O_{2} \rightarrow 2NO+3H_{2} O[/tex]
What is Balanced equation?Balanced equation is the one in which the total number of atoms of a species on reactant side is equal to the total number of atoms on product side
In first , The skeletal reaction is
[tex]KCl+O_{2} \rightarrow KClO_{3}[/tex]
The number of oxygen atoms on left side is 2 while on product side it is 3 so to balance multiply by 3 to [tex]O_{2}[/tex] and by 2 to product side
[tex]KCl+3O_{2} \rightarrow 2KClO_{3}[/tex]
The number of atoms of Potassium and chlorine on left and right are 1 and 1 while on right side it is 2,2 so multiply [tex]KCl[/tex] by 2
The balanced equation is
[tex]2KCl+3O_{2} \rightarrow 2KClO_{3}[/tex]
In second the skeltal equation is
[tex]NH_{3} +O_{2} \rightarrow NO+H_{2} O[/tex]
The number of hydrogen atom is 3 while on produt side it is 2 so multiply [tex]NH_{3}[/tex] by 2 and [tex]H_{2} O[/tex] by 3
[tex]2NH_{3} +O_{2} \rightarrow NO+3H_{2} O[/tex]
now balance nitrogen
[tex]2NH_{3} +O_{2} \rightarrow 2NO+3H_{2} O[/tex]
Now balance oxygen and the balanced equation is
[tex]2NH_{3} +\frac{5}{2} O_{2} \rightarrow 2NO+3H_{2} O[/tex]
Thus the two balanced equation are
[tex]2KCL+3O_{2} \rightarrow 2KClO_{3}[/tex] and
[tex]2NH_{3} +\frac{5}{2} O_{2} \rightarrow 2NO+3H_{2} O[/tex]
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(a) Explain the process by which these dark lines are generated by the elements in the sun's atmosphere.
Specifically, why are they black and not colored, and why do they match the colored line spectra of
those elements?
These substances absorb black body radiation energy at a very particular wavelength of light that is particular to them. The black (absorption) line is the result of energy being absorbed from the spectrum when an electron jumps from an orbit with low energy to an orbit with high energy.
Why dark lines appear in the absorption spectra?A substance's light transmission spectrum that displays black bands or lines where light has been absorbed by atoms, generating a dip in the spectrum, is called an absorption spectrum. By descending the energy ladder, electrons produce an emission spectrum.Some of the light at specific wavelengths is scattered when it travels through the atmosphere's gas, producing darker bands. The wavelengths of light released when common materials were heated to form lines that became known as "spectral lines" were recorded.To learn more about : Absorption spectra
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Answer the following question: Ethanol, C2H5OH, is considered clean fuel because it burns in oxygen to produce carbon dioxide and water with few trace pollutants. If 500.0 g of H2O are produced during the combustion of ethanol, how many grams of ethanol were present at the beginning of the reaction? When answering this question include the following:
Have both the unbalanced and balanced chemical equations.
Explain how to find the molar mass of the compounds.
Explain how the balanced chemical equation is used to find the ratio of moles (hint: step 3 in the video).
Explain how many significant figures your answer needs to have.
The numerical answer
The amount, in grams, of ethanol that was present at the beginning of the reaction, would be 430 grams.
Stoichiometric problemEthanol burns in oxygen according to the following equation:
[tex]C_2H_5OH + O_2 -- > CO_2 + H_2O[/tex]
The balanced equation of the reaction will be:
[tex]C_2H_5OH + 3O_2 -- > 2CO_2 + 3H_2O[/tex]
The mole ratio of ethanol to water is 1:3.
The molar weight of H = 1 g/mol.
The molar weight of O = 16 g/mol
Molar weight of C = 12
Molar mass of water, [tex]H_2O[/tex] = (1 x 2) + 16 = 18 g/mol
Molar mass of ethanol, [tex]C_2H_5OH[/tex] = (12x2) + (1x5) + 16 + 1 = 46 g/mol
If, mole = mass/molar mass; mole of 500.0 g water will be:
500/18 = 27.778 moles
Then, the equivalent mole of ethanol that burned, from the stoichiometric mole ratio, would be:
27.778/3 = 9.259 moles
If, mass = mole x molar mass,
Then, 9.259 moles ethanol = 9.259 x 46 = 425.914
Since the molar mass has the least significant figures (two significant figures), the final answer will also have two significant figures.
Thus, the amount of ethanol that was present at the beginning of the reaction is 430 grams.
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Determine the molarity of NaOH to three decimal places if 21.77 mL of this NaOH were used to titrate 0.305 g of KHP (MM 204.22 g/mol)
Answer
The molarity of NaOH to three decimal places is 0.069 mol/L
Explanation
Given:
Volume of NaOH used = 21.77 mL
Reacting mass of KHP = 0.305 g
Molecular Mass of KHP = 204.22 g/mol
What to find:
The molarity of NaOH to three decimal places.
Step-by-step solution:
The first step is to write the balanced stoichiometric chemical equation of the reaction:
[tex]HKC_8H_4O_4+NaOH\rightarrow NaKC_8H_4O_4+H_2O[/tex]From the balanced chemical equation;
1 mol KHP reacts with 1 mol NaOH
Thus, moles of KHP is:
[tex]\text{Moles of KHP }=\frac{Reacting\text{ mass}}{MM\text{ of KHP}}=\frac{0.305\text{ g}}{204.22\text{ g/mol}}=1.493\times10^{-3}\text{ mol}[/tex]Since, 1 mol KHP reacts with 1 mol NaOH from the balanced equation,
Therefore, 1.493 x 10⁻³ mol KHP will react with:
[tex]\frac{1\text{ mol NaOH }\times1.493\times10^{-3}mol\text{ KHP}}{1\text{ mol KHP}}=1.493\times10^{-3}mol\text{ NaOH}[/tex]The last step is to calculate the molarity of NaOH:
Conversion factor:
1 mL = 10⁻³ L
21.77 mL = 2.177 x 10⁻³ L
Molarity of NaOH is:
[tex]\begin{gathered} \text{Molarity of NaOH }=\frac{Moles\text{ of NaOH}}{Volume\text{ of NaOH in L}}=\frac{1.493\times10^{-3}\text{ mol}}{2.177\times10^{-3}\text{ L}} \\ \text{Molarity of NaOH }=0.069\text{ mol/L} \end{gathered}[/tex]
I need help with this question please
The 0.2 moles of glucose are present in the 0.400 M solution.
What is molarity?
The amount of a substance in a specific volume of solution is known as its molarity (M).
As given in the solution
Volume = 0.500 L
Molarity = 0.400
By using the molarity formula
M = moles of glucose/Volume in liters
Let's say moles of glucose = X
X= 0.400 * 0.500 = 0.2 moles
Hence, the answer is 0.2 moles of glucose .
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An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L.Initially, the temperature of the gas was 732.°C and had a pressure of 294. kPa. Determine the pressure of the gas when the temperature decreased to 156°C.
125.49kPa
Explanations:
According to the Gay's Lussac law, the pressure of the given mass of a gas is directly proportional to its absolute temperature provided that the volume is constant. Mathematically;
[tex]\begin{gathered} P\alpha T \\ P=kT \\ T=\frac{P_1}{T_1}=\frac{P_2}{T_2} \end{gathered}[/tex]Given the following parameters
Iinitial pressure P1 = 294kPa
Initial temperature = 732.°C = 732+273 = 1005K
Final temperature = 156°C + 273 = 429K
Required
New pressure P2
Substitute the given parameters
[tex]\begin{gathered} P_2=\frac{P_1T_2}{T_1} \\ P_2=\frac{294\times429}{1005} \\ P_2=125.49kPa \end{gathered}[/tex]Therefore the pressure of the gas when the temperature decreased to 156°C is 125.49kPa
The rate constant for a reaction at 40.0°C is exactly 4 times that at 20 0°C Calculate the energy of activation for the reaction.
Explanation:
Data provided:
T2 = 40.0 °C
(absolute temperature = T2 = 40.0 °C + 273 = 313 K)
------
T1 (absolute) = 20.0 °C + 273 = 293 K
------
The rate constant for a reaction at 40.0 °C is exactly 4 times that at 20.0 °C, mathematically:
k2/k1 = 4
------------------------
Here is used the Arrhenius expression as follows:
[tex]ln\text{ }\frac{k2}{k1}=\text{ }\frac{Ea}{R}x\lbrack\frac{1}{T1}-\frac{1}{T2}\rbrack[/tex]R = universal gas constant = 8.314 J/mol K
Ea = activation energy
------------------------
Procedure:
[tex]\begin{gathered} ln\text{ 4 = }\frac{Ea}{8.314\text{ J/mol K}}x\lbrack\frac{1}{293\text{ K}}-\frac{1}{313\text{ K}}\rbrack \\ 1.386\text{ = }\frac{Ea}{8.314}x(2.18x10^{-4}) \\ Ea\text{ = 52858.73 J/mol} \\ \end{gathered}[/tex]Answer: Ea = 52858.73 J/mol
a gas mixture at 20.0 C and 2.0 atm contains 0.40 mol of H2, 0.15 mol of O2, and 0.50 mol of N2. Assuming ideal behavior, what is the partial pressure of hydrogen gar [H2] in the mixture?
The partial pressure of hydrogen gas in the mixture is:0.53334 atm.
What is partial pressure?
partial pressure. noun. the pressure that a gas would have if it took up the entire volume that the mixture of gases currently occupies.
P total,and the total number of moles in the mixture would be,
n total=nH2+nO2+nN2
This means that you could write
P total.V=ntotal.RT
p total=n total.RT/V
This is equivalent to
p total=[nH2+nO2+nN2].RT/V
therefore,
P total =PH2+PO2+pN2
now, to get the partial pressure of,let's Hydrogen gas
RT/V=Ptotal/nH2+nO2+nN2
therefore
PN2=XN2.p total
similarly,
PO2=XO2.p total
PN2=XN.p total
The total number of moles will be
[tex]ntotal[/tex] = 0.40+0.15+0.50=1.50 moles.
[tex]PH2[/tex]=0.40/1.50*2.0 atm =0.5334 atm.
[tex]PO2[/tex]=0.15/1.50*2.0 atm =0.2 atm.
[tex]PN2[/tex]=0.50/1.50*2.0 atm =0.66 atm.
Hence, the partial pressure of hydrogen gas in the mixture is:0.53334 atm.
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I need help with this chem equation
The percentage yield is 81.08.
calculation:-
The percentage yield = actual yield/ theoretical yield × 100
= 150 grams / 185 grams ×100
= 81.08
The percentage yield method is calculated to be the experimental yield divided by way of theoretical yield improved through a hundred. If the actual and theoretical yield is the same, the percentage yield is a hundred%. generally, the percentage yield is lower than 100% due to the fact the real yield is regularly much less than the theoretical value.
In chemistry, yield also referred to as reaction yield, is a degree of the number of moles of a product shaped in relation to the reactant consumed, and received in a chemical reaction, typically expressed as a percent.
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A covalent compound is formed by
a. metal atoms losing valence electrons to non-metal atoms
b. non-metal atoms losing valence electrons to non-metal atoms
c. metal atoms sharing valence electrons
d. non-metal atoms sharing valence electrons
Complete and balance the following half reaction. Assume the reaction occurs in basic media.
Cl−⟶ClO3−
Balance the following half reaction occurs in basic media then Cl → ClO₃⁻
6OH⁻ + Cl⁻¹ → ClO₃⁻¹ + 3H₂O + 6e⁻
The concentration of OH⁻ is more than the solution called as basic medium
Here given reaction is
Cl → ClO₃⁻
Then the steps we have to follow are:
Balancing in basic solution then
First get the acidic answer means in acidic answer, Break into half reaction Balance all element except H and OBalance O by adding H₂OBalance H by adding H⁺Then add electron to the more positive sideBalance electronCancel the likes substances on opposite sideThen rewrite the correct equationAdd as many OH⁻ as you have H⁺ to both sideThen simplify and cancel out like H₂OThen 2H⁺ + 2OH⁻ → 2H₂OAnd then 1 H = 1H⁺2Oxygen = 2H₂OThen rewrite the correct equationAnd the equation is 6OH⁻ + Cl⁻¹ → ClO₃⁻¹ + 3H₂O + 6e⁻ in basic media
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3. Given the names of the following compounds, determine their correct chemical formula
e. Pentanitrogen tribromide
Answer:
N5Br3
Explanation:
I need to fill in the blanks if you can only do one question can you please do the first one
Answer
34.40 grams of H₂O are made.
Explanation
The first step is to balance the chemical equation for the reaction:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
From the balanced equation;
1 mole of C₃H₈ produced 4 moles of H₂O
1 mole of C₃H₈ = 44.1 g/mol
1 mole of H₂O = 18.015 g/mol
This implies;
(1 mol x 44.1 g/mol) = 44.1 g of C₃H₈ produced (4 mol x 18.015 g/mol) = 72.06 of H₂O
Therefore, 23.5 g of C₃H₈ will produce
[tex]\frac{23.5g\text{ }C₃H₈}{44.1g\text{ }C₃H₈}\times72.06g\text{ }H₂O=38.40\text{ }gram\text{ }H₂O[/tex]Hence, 34.40 grams of H₂O are made
The ammonia (NH3)molecule is the conjugate base of the NH4+ (called "ammonium") ion. a weak acid. An aqueous solution of NH3 has a pH of 1 1.6. Write the net ionic equation for the reaction that makes an aqueous solution of NH3 basic. (The answer looks very similar to Eq. 5 in the introduction to this experiment.)
NH3 is a weak base. In solution we write NH3(aq).
The question says NH3 because ammonia is a weak base and does not ionize strongly in water. To write the net ion equation, we need to remove the spectator ion. Removing the spectator ion leaves the net ion equation. This process can be repeated for each reaction to obtain the net ionic equation.
The net ionic equation describes only the species participating in the reaction while the full ionic equation also includes the spectator ion. A net ionic equation is a chemical equation of a reaction that lists only the species involved in the reaction. The net ionic equation is commonly used in acid-base neutralization reactions double displacement reactions, and redox reactions.
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URGENT HELP PLEASE. Identity the element represented by the orbital diagram below.
Answer: 4.023938398328392932838398293892839839829382938928938298928392839239829389329808091808208210808208018820801808208093829898081080282
Explanation:
What is the pressure exerted by 2.10 g Ar gas at 18.0 °C in a 660-ml flask?
1.91*10^-3 atm
4.71 atm
1.91 atm
0.118 atm
76.1 atm
Answer:
1.91 atm
Explanation:
To start this question I would first look at what the question is giving us:
M= 2.10g Argon
T= 18.0°C
V= 660-mL
P= ?atm
We now would recognize that from the things given, the formula that suits it would be PV=nRT because it would have the given data present were we can solve for P.
R is a constant that is 0.082 L*atm/K*mol. This constant lets us know what units we need to convert in order move forward.
We would need our volume to be in Liters, our pressure in atm, our temperature in K and our mass in mols.
So then in order to convert the mass given, we would need to go from grams to mols. We do this by starting off with our given mass (2.10g) and then dividing it by the molar mass of the element Argon (39.948g). This would make a total of 0.052mols.
To convert the Celsius to Kelvin, we just need to add 273 to the temperature given. 18.0°C + 273 = 291K.
To convert our volume, 1000mL=1L, so we would divide our given mL by 1000. 600/1000= 0.660L.
Now we can go ahead and use our formula and plug in the numbers to solve for P.
PV=nRT
(x atm)(0.660 L)=(0.0526 mol)(0.082 L*atm/K*mol)(291 K)
When solved, we would get a final answer of 1.90173 atm. Our closest answer being 1.91 atm.
What is the "percent
abundance" of the black eyed
peas in this sample?
Sample Number Abundance Mass
of Beans
(%)
(g)
187
[?]
1.3
Black
Eyed Peas
Cannellini
Beans
113
2.9
Weighted
Average (g)
1.9
The percentage abundance of the blacked-eyed peas in the sample is 39.6%.
What is the percentage abundance ?
It is the ratio in which a particular substance occurs to the total occurrence of similar substances of the same kind.
Percentage abundance = (occurrence of substance/total occurrence of substance of similar kind) × 100
Thus the percent abundance of the black eyed peas in this sample can be calculated as:
total number of beans = 187
number of blacked-eyed peas = 187 - 113 = 74
Percentage abundance = 74/187 × 100 %
= 39.6%
Thus we can conclude, the percentage abundance of the blacked-eyed peas in the sample is 39.6%.
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A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 16.83g PbCl2(s) is obtained from 200.0mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.
0.25 Molarity of lead nitrate aqueous solution is there when a solution of nacl is added slowly to a solution of lead nitrate.
What is molarity and how it is calculated out to be so?Molarity is the number of moles of substance present in one litre of solution and is measured in g/litres.Here in this question is given 16.83 g of lead nitrate is obtained from 200 ml of original solution.To calculate the molarity first we will have to calculate the number of moles of lead nitrate for which the formula is given mass/ molar mass.The mass that is given is 16.83 g and the molar mass is 331.2 g dividing we will get 5.02.Then dividing the number of moles by 0.2 L of solution we will get the answer as 0.25 g/litre molarity as the answer.To know more about molarity visit:
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Determine the mass of sodium metal that contains the same number of moles as 81.7 g of copper
metal.
The mass of sodium metal that contains the same number of moles as 81.7 g of copper metal is 2.3 grams.
What is Sodium Metal?
Since sodium is a soft metal, it tarnishes quickly when exposed to air. Water also causes a strong reaction. In some nuclear reactors, sodium is employed as a heat exchanger. It is also used as a reagent in the chemical sector. In contrast, sodium salts are more useful than sodium itself.
Mass of copper = 81.7 g
1 Mole of Cu = 8.17 g
Now, 1 mole of Copper contains 6.022×10^23 atoms
So 0.1 moles of Copper contains 6.022 × 10^22 atoms.
So we need to find the weight of 6.022× 10^22 Sodium atoms.
We know that 6.022 ×10^22 Na atoms is 0.1 mole of Na.
So we need to find the weight of 0.1 mole of Na.
1 mole of Na = 23 g
So 0.1 mole of Na = 2.3 grams
So, answer is 2.3 grams.
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How many liters of oxygen are required to completely react with 2.0 liters of CH4 at30 °C and 3.0 atm?CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
1) Write the chemical equation.
[tex]CH_4+2O_2\rightarrow CO_2+2H_2O[/tex]2) List the known and unknown quantities.
Sample: CH4.
Volume: 2.0 L.
Temperature: 30 ºC = 303.15 K.
Pressure: 3.0 atm.
Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1).
Moles: unknown.
3) Moles of CH4.
3.1- Set the equation.
[tex]PV=nRT[/tex]3.2- Plug in the known values and solve for n (moles).
[tex](3.0\text{ }atm)(2.0\text{ }L)=n*(0.082057\text{ }L*atm*K^{-1}mol^{-1})(303.15\text{ }K)[/tex][tex]n=\frac{(3.0\text{ }atm)(2.0\text{ }L)}{(0.082057\text{ }L*atm*K^{-1}*mol^{-1})}=[/tex][tex]n=0.24\text{ }mol\text{ }CH_4[/tex]4) Moles of oxygen that reacted.
The molar ratio between CH4 and O2 is 1 mol CH4: 2 mol O2.
[tex]mol\text{ }O_2=0.24\text{ }CH_4*\frac{2\text{ }mol\text{ }O_2}{1\text{ }mol\text{ }CH_4}=0.48\text{ }mol\text{ }O_2[/tex]5) Volume of oxygen required.
Sample: O2.
Moles: 0.48 mol.
Temperature: 30 ºC = 303.15 K.
Pressure: 3.0 atm.
Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1).
Volume: unknown.
5.1- Set the equation.
[tex]PV=nRT[/tex]5.2- Plug in the known values and solve for V (liters).
[tex](3.0\text{ }atm)(V)=0.48\text{ }O_2*(0.082057\text{ }L*atm*K^{-1}mol^{-1})(303.15\text{ }K)[/tex][tex]V=\frac{(0.48\text{ }mol\text{ }O_2)(0.082057\text{ }L*atm*K^{-1}*mol^{-1})(303.15\text{ }K)}{3.0\text{ }atm}[/tex][tex]V=3.98\text{ }L[/tex]3.98 L of O2 is required to react with 2.0 L CH4.
.
Convert 5.25 moles of Ne to particles of Ne
Answer
Explanation
Given:
Moles of Ne = 5.25 mol
What to find:
The number of particles of Ne in 5.25 moles of Ne.
Step-by-step solution:
Conversion factor: 1 mole of any substance = 6.022 x 10²³ particles
Therefore, 5.25 moles of Ne will be equal
[tex]undefined[/tex]How many moles of Al2O3 are produced if we use 5.7 moles of Al?
4 Al + 3 O2 --> 2 Al2O3
Moles of Al₂O₃ are produced if we use 5.7 moles of Al is 2.85 moles .
The balanced equation is :
4Al + 3O₂ -----> 2Al₂O₃
here given that :
moles of Al = 5.7 moles
from the equation it is clear that
four mole of Al produced 2 moles of Al₂O₃
so we can calculated the moles of Al₂O₃ produce by 5.7 moles of Al
5.7 moles of Al produced = (5.7 × 2 ) / 4 moles of Al₂O₃
= 2.85 moles of Al₂O₃
Thus, Moles of Al₂O₃ are produced if we use 5.7 moles of Al is 2.85 moles .
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At what temperature does sulfur hexafluoride have a density of 0.4450 g/L at 0.8210 atm
The temperature at which sulfur hexafluoride have a density of 0.4450 g/L at 0.8210 atm is 32.40K.
We know that density is the mass of the substance divided by the volume of the substance.
so mass of SF6 = 146.05 g
Density = 0.4450g/L
D = M/V
0.4450 = 146.05 /V
V= 146.05/ 0.4450
V= 328.20L
Now we know that ideal gas equation,
PV = nRT
Where P = Pressure of the gas = 0.8210 atm
T=?
R = 8.314
V = 328.20L
thus, putting values inthe formula,
0.8210 × 328.20 = 1 × 8.314 × T
T = 269.45 / 8.314
T =32.40K
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The volume of a given mass of gas is 410. mL at 380. mm Hg. What will its volume in mL be ifthe pressure changes to 2.00 atm?
Answer:
[tex]102.5\text{ mL}[/tex]Explanation:
Here, we want to get the final volume of the gas
According to Boyles' law, the volume is inversely proportional to the pressure
Mathematically:
[tex]P_1V_1\text{ = P}_2V_2[/tex]where:
P1 is the initial pressure of the gas which is 410 ml
V1 is the initial volume of the gas which is 380 mmHg
P2 is the final pressure of the gas which is 2 atm (we convert this to mmHg by multiplying by 760 mmHg: we have that as 2 * 760 mmHg = 1520 mmHg)
V2 is the final volume of the gas which is what we want to calculate
Substituting the values:
[tex]\begin{gathered} V_2\text{ = }\frac{P_1V_1}{P_2} \\ \\ V_2\text{ = }\frac{410\times380}{1520}\text{ = 102.5 mL} \end{gathered}[/tex]Seven 5.0 mL aliquots of a dilute solution of HCl were titrated with 0.1245 M sodiumhydroxide. The following volumes were needed to neutralize the acid solution:
In this question, we have to determine the molar concentration of the acid HCl, we have the following information:
5.0 mL of HCl
0.1245 M of NaOH
7 different volumes of NaOH, if we take the average value, we will have 58.8 mL of average
Now we can use the titration formula, which is:
MaVa = MbVb
Ma = molar concentration of acid
Va = volume of acid
Mb = molar concentration of base
Vb = volume of base
Now we add the values into the formula:
Ma * 5.0 = 0.1245 * 58.8
5Ma = 7.32
Ma = 7.32/5.0
Ma = 1.46 M
The molar concentration of HCl, based on the information provided and using the average value of volume for the base is 1.46 M
