Answer:
9.25l
Explanation:
9.25l was correct answer
The ideal gas law is a fundamental equation that describes the behavior of an ideal gas. It relates the pressure (P), volume (V), temperature (T), and number of moles (n) of an ideal gas using the ideal gas constant (R). The volume of the gas is 18.5 L. Hence option D is correct.
We can use the ideal gas law to solve this problem:
PV = nRT
where:
P is the pressure of the gas (in atm)
V is the volume of the gas (in L)
n is the number of moles of the gas
R is the ideal gas constant (0.08206 L·atm/mol·K)
T is the temperature of the gas (in K)
Plugging in the values from the problem, we get:
2 atm * V = 1.5 mol * 0.08206 L·atm/mol·K * 300 K
V = (1.5 mol * 0.08206 L·atm/mol·K * 300 K) / 2 atm
V = 18.5 L
Therefore, the volume of the gas is 18.5 (option D).
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What is the oxidation state of oxygen (O) in the reactant O2(g)?
Answer:0
Explanation:
Since oxygen gas i.e., diatomic oxygen exists in the atmosphere in the free state, hence the oxidation state of each atom will be 0
please answer the question so i can make sure I got them right! thank you :)
pH = pKa + log [conj.base]/[acid]
Let the concentration of the conjugate base = x
=> The concentration of the acid is also x (As the acid concentration is equivalent to that of the conjugate base)
for CH₃COOH=0.50 M and CH₃COO=0,25 M
pH = pKa + log [salt]/[acid]
pKa = -log Ka = -log 1.8x10-5 = 4.74
pH = 4.74 + log (0.50 M/1.0 M) = 4.74 + log 0.5 = 4.74 + (-0.3)
pH = 4.74 - 0.3
pH = 4.44
For0.20 M Na2CO3
pH=−log[H+]
=−log (1.54×10−12)
=11.8
for HNO₂
Kb = 2.17X10^-11 = x^2 / 0.148
x = [OH-] = 1.79X10^-6
pOH = 5.747
pH = 14.000 - pOH = 8.253
for HPO₄³⁻
= [HPO₄³⁻] [PO₄³⁻] [H +]/×10⁻³
=[PO₄³⁻]5.464×10⁻¹⁸
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ClO(4)− Express your answer as a chemical formula.
ClO(4)− is regarded as perchlorate ion and are produced commercially in most situations as salts via industries and in the laboratory.
What is Perchlorate ion?This ion is referred to as a monovalent inorganic anion and is obtained by deprotonation of perchloric acid. It is composed of chlorine and oxygen atoms in the ratio 1 to 4 respectively.
This has 32 valence electrons available in the Lewis structure and is used in the commercial production of solid rocket fuel.This ion has a molar mass of 99.451 g mol−1 and is used in different processes such as an oxidizer and to control static electricity during the process of food preservation in industries.
Therefore ClO₄− is also regarded as perchlorate ion and is the most appropriate choice.
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The following reaction: HF(aq) <--> H+(aq) + F-(aq) has an equilbirum constant (K) value of 7.2 x 10-4. This means that the reaction proceeds essentially to completion.
Group of answer choices
True
False
Given an equilibrium constant value of 7.2 x 10-4 it is false to say that the reaction proceeds essentially to completion.
What is the equilibrium constant?In a reaction, we can judge using the value of the equilibrium constant weather or not the reaction moves on to completion. If the reaction moves up to completion, it the follows that the value of the equilibrium constant ought to be large.
On the other hand, when we have a case that the equilibrium constant is small and is not so large, then the reaction does not proceed essentially to completion.
Given an equilibrium constant value of 7.2 x 10-4 it is false to say that the reaction proceeds essentially to completion.
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In a perfect world, reactions can never go above 100% yield. However in reality you will sometimes get above 100% yield. Why?
Group of answer choices
A. Excess water and Impurities
B. Impurities Only
C. Excess Water Only
D. You can never have above 100% yield under any circumstance.
Answer:
You can never have above 100% yield under any circumstance
To solve such this we must know the concept of chemical reaction. Therefore, the correct option is option D that is you can never have above 100% yield under any circumstance.
What is chemical reaction?Chemical reaction is a process in which two or more than two molecules collide in right orientation and energy to form a new chemical compound. The mass of the overall reaction should be conserved. There are so many types of chemical reaction reaction like combination reaction, double displacement reaction.
You can never have above 100% yield under any circumstance for any chemical reactions. Option D is the correct options among all the given options.
Therefore, the correct option is option D that is you can never have above 100% yield under any circumstance.
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A chemistry student needs 45.0mL of pentane for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student discovers that the density of pentane is ·0.626gcm−3. Calculate the mass of pentane the student should weigh out. Round your answer to 3 significant digits.
The mass of pentane the student should weigh out is
The density of pentane is 0.626 gcm-3
To calculate the mass of pentane following expression is used,
(Density is defined as the mass divide by volume)
Density = mass / volume
mass of pentane = Density of pentane * Volume of pentane
mass of pentane = 0.626 gcm-3 * 45.0 mL
= 28.17 g
Here the unit of mass of pentane is g,
However the unit of density is gcm-3 and unit of volume is mL i.e. cm3
Hence, Mass = gcm-3 * cm3
Mass = g
The mass of pentane the student should weigh out is 28.17g
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The symbol X in the following equation, 23/11 Na + 1/1H → 23/12 Mg + X, is a/an
Answer:
X = ¹₀n
Explanation:
The mass number is the total amount of neutrons and protons in the element. The atomic number is the total protons in the element. The mass number is the superscript and the atomic number is the subscript. The mass and atomic numbers must be balanced on both sides of the equation. The element can be identified by the atomic number.
In the event that we have an atomic number of zero, there is no element this represents, so the letter "n" should be used.
²³₁₁Na + ¹₁H → ²³₁₂Mg + X
Mass Number:
Reactants = Products
23 + 1 = 23 + ?
24 = 23 + ?
1 = ?
Atomic Number:
Reactants = Products
11 + 1 = 12 + ?
12 = 12 + ?
0 = ?
The complete equation is:
²³₁₁Na + ¹₁H → ²³₁₂Mg + ¹₀n
URGENT
A chemical equilibrium between gaseous reactants and products is shown.
N2(g) + 3H2(g) ⇌ 2NH3(g)
How will the reaction be affected if the pressure on the system is increased?
It will shift toward the reactant side as there is lower pressure on the reactant side.
It will shift toward the product side as there is higher pressure on the product side.
It will shift toward the reactant side as there are a greater number of moles of gas on the reactant side.
It will shift toward the product side as there are a fewer number of moles of gas on the product side.
Answer:
Explanation:
Discussion
When Pressure increases equilibrium shifts to the side with the smallest number of moles. But which side is that?
N2(g) + 3H2(g) ⇌ 2NH3(g)
The left side has 1 mol of nitrogen (N2) and 3 moles of Hydrogen = 4 mols
on the left side.
The right side has 2 mols of NH3 = 2 mols on the right.
Conclusion: You tell the number of mols by the Balance numbers to the left of each chemical in an equation.
Since the left side N2 + 3H2 = 4 mols, the equilibrium does NOT shift left.
2NH3 is only two mols.
The equilibrium shifts Right
Answer
D
Lab Data
Mass of magnesium (g)
Moles of magnesium (mol)
Temperature of water (°C)
Temperature of water (K)
Vapor pressure of water (mmHg)
Barometric pressure (mmHg)
Observations
Volume of hydrogen gas collected (mL)
Volume of hydrogen gas collected (L)
Pressure of hydrogen gas (mmHg)
Pressure of hydrogen gas (atm)
Moles of hydrogen gas produced (mol)
Ideal das constant (L-atm-mol-K)
0.218
-X
ES
V
LAB DATA SH
OLONCE
Answer:
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The compound iron oxide can exist with either iron(II) ions or iron(III) ions. Conduct Internet research to learn about the differences between iron(II) oxide and iron(III) oxide. Give the chemical formula for each compound. Describe their appearance and uses. Based on your findings, are these two forms of the same compound, or are they two completely different compounds?
(What goes in the 6 empty spaces?)
Based on our finding these two compounds are not same they are completely different from each other as Formula of both compounds are different, their appearance is also different from each other.
What is Iron (II) Oxide ?The formula of the Iron II oxide is FeO. Common name of Iron (II) Oxide is Ferrous Oxide. Iron (II) Oxide is a black colored powder. The mineral form of Iron (II) oxide is known as Wustite. Iron (II) Oxide is used as a pigment. It is also used to make dyes.
What is Iron (III) Oxide ?The formula of the Iron (III) Oxide is Fe₂O₃. Common name of Iron (III) Oxide is Ferric oxide. Iron (III) Oxide appears as Red-Brown solid. It is also known as Hematite. Iron (III) oxide is used as pigments. It is used in dental composites , cosmetics. It is also used to apply the final polish on metallic jewellery.
Thus from the above conclusion we can say that Based on our finding these two compounds are not same they are completely different from each other as Formula of both compounds are different, their appearance is also different from each other.
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In the chemical reaction:
Cu + 2AgNO3 → 2Ag + Cu(NO3)2
What is the limiting reactant if you start with 1.8 moles of copper and 2.0 moles of silver nitrate?
Group of answer choices
A. copper (II) nitrate
B. copper
C. silver
D. silver nitrate
Taking into account the reaction stoichiometry and definition of limiting reactant, AgNO₃ will be the limiting reagent.
Reaction stoichiometryIn first place, the balanced reaction is:
Cu + 2 AgNO₃ → 2 Ag + Cu(NO₃)₂
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:
Cu: 1 moleAgNO₃: 2 molesAg: 2 molesCu(NO₃)₂: 1 moleLimiting reagentThe limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
Limiting reagent in this caseTo determine the limiting reagent, it is possible to use a simple rule of three as follows: if by stoichiometry 1 mole of Cu reacts with 2 moles of AgNO₃, 1.8 moles of Cu reacts with how many moles of AgNO₃?
[tex]amount of moles of AgNO_{3} =\frac{1.8 moles of Cux2 moles of AgNO_{3} }{1 mole of Cu}[/tex]
amount of moles of AgNO₃= 3.6 moles
But 3.6 moles of AgNO₃ are not available, 2 moles are available. Since you have less moles than you need to react with 1.8 moles of Cu, AgNO₃ will be the limiting reagent.
SummaryIn summary, AgNO₃ will be the limiting reagent.
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Hydrogen gas has a density of 0.090/gL, and at normal pressure and 0.214°C one mole of it takes up 22.4L. How would you calculate the moles in 370.g of hydrogen gas?
Set the math up. But don't do any of it. Just leave your answer as a math expression.
Also, be sure your answer includes all the correct unit symbols.
how to set up this equation?
moles= ???
Answer:
See below
Explanation:
370 g / .090 g/l = _____?___ liters
take that answer then :
? liters / 22.4 liters / mole = # moles done!
There are approximately 183.50 moles of hydrogen gas in 370.g of hydrogen gas.
The number of moles in 370.g of hydrogen gas using the given information.
In the given example,
Density of hydrogen gas = 0.090 g/L
Molar volume at normal pressure and 0.214°C = 22.4 L/mol
So, we calculate the volume of hydrogen gas (in L) using the given mass and density:
Volume (in L) = mass (in g) / density (in g/L)
Volume (in L) = 370.g / 0.090 g/L
Volume (in L) ≈ 4111.11 L
By using the molar volume, calculate the number of moles:
moles = Volume (in L) / Molar volume (in L/mol)
moles = 4111.11 L / 22.4 L/mol
moles ≈ 183.50 moles (rounded to two decimal places)
Hence, there are approximately 183.50 moles of hydrogen gas in 370.g of hydrogen gas.
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How many mL of a 0.193 M aqueous solution of ammonium bromide, , must be taken to obtain 8.42 grams of the salt?
Answer:
445 mL NH₄Br
Explanation:
(Step 1)
Convert grams ammonium bromide (NH₄Br) to moles using its molar mass.
Molar Mass (NH₄Br): 14.007 g/mol + 4(1.008 g/mol) + 79.904 g/mol
Molar Mass (NH₄Br): 97.943 g/mol
8.42 grams NH₄Br 1 mole
----------------------------- x ------------------------ = 0.0860 moles NH₄Br
97.943 grams
(Step 2)
Calculate the volume of NH₄Br using the molarity equation. Then, convert liters (L) to milliliters (mL).
Molarity (M) = moles / volume (L)
0.193 M = 0.0860 moles / volume
(0.193 M) x volume = 0.0860 moles
volume = 0.445 L
1,000 mL = 1 L
0.445 L NH₄Br 1,000 mL
------------------------ x ------------------ = 445 mL NH₄Br
1 L
Quick explanation please i'm having trouble
Two different atoms have nine protons each and the same mass. However, one is neutral while the other has a negative charge. Describe what each atomic structure could be, listing the possible number and location of all subatomic particles.
what is s for silicon tetrachloride Sicl4?
S denotes the ''number of shared electron pairs by an atom'', Hence, Silicon transmits its 4 electrons with 4 Cl-atoms. Thus the Value of S is 4 in SiCl₄ .It is also known as covalency
What is silicon tetrachloride used for?
Silicon Tetrachloride is a transparent, colorless, fuming liquid with an irritating odor. It is used to create Silicon-containing chemicals and in chemical analysis. determine potentially hazardous frontages.
How is silicon tetrachloride produced?Silicon tetrachloride is designed by the chlorination of various silicon compounds such as ferrosilicon, silicon carbide, or mixtures of silicon dioxide and carbon. The ferrosilicon route is most familiar. In the laboratory, SiCl 4 can be prepared by dining silicon with chlorine on 600 °C (1,112 °F): Si + 2 Cl 2 → SiCl.
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Suppose you need to prepare 136.9 mL of a 0.315 M aqueous solution of NaCl.
What mass, in grams, of NaCl do you need to use to make the solution?
Answer:
2.52 g NaCl
Explanation:
(Step 1)
To find the mass, you first need to find the moles NaCl. This value can be found using the molarity ratio:
Molarity = moles / volume (L)
After you convert mL to L, you can plug the given values into the equation and simplify to find moles.
136.9 mL / 1,000 = 0.1369 L
Molarity = moles / volume
0.315 M = moles / 0.1369 L
0.0431 = moles
(Step 2)
Now, you can use the molar mass to convert moles to grams.
Molar Mass (NaCl): 22.990 g/mol + 35.453 g/mol
Molar Mass (NaCl): 58.443 g/mol
0.0431 moles NaCl 58.443 g
------------------------------ x ------------------- = 2.52 g NaCl
1 mole
28. What mass
0.120M HCI?
of Na₂CO3 (Molar Mass = 106.0 g/mol) is required to react completely with 21.6 mL of.
Mass of [tex]$\mathrm{Na}{2} \mathrm{CO} 3$[/tex] required [tex]$=0.55 \mathrm{~g}$[/tex]
What is meant by molar mass?The mass of one mole of a sample is its molar mass. Add the atomic masses (atomic weights) of all the atoms in the molecule to obtain the molar mass. Using the mass listed in the Periodic Table or atomic weights table, determine the atomic mass for each element.The total mass of all the atoms that make up a mole of a specific molecule, measured in grams, is known as the molar mass or molecular weight. The measurement is made in grams per mole.Molar mass is a crucial factor to consider while planning an experiment. The molar mass enables you to calculate the quantity you should weigh on your scale if you are testing theories involving precise amounts of a substance. Take a look at an experiment that needs 2 moles of pure carbon as an illustration.The mass 0.120M HCI:
Moles of [tex]$\mathrm{HCl}$[/tex]reacted [tex]$=0.120 \times 21.6 / 1000=0.00260$[/tex]
according to balanced reaction, [tex]$\mathrm{HCl}$ and $\mathrm{Na} 2 \mathrm{CO} 3$[/tex] reacts in [tex]$2: 1$[/tex] the ratio
moles of [tex]$\mathrm{Na} 2 \mathrm{CO} 3$[/tex]required [tex]$=0.00260 \times 2=0.00520$[/tex]
convert moles to mass
mass [tex]$=$[/tex]moles [tex]$\times$[/tex]molar mass
mass [tex]$=0.00520 \times 106.0$[/tex]
mass [tex]$=0.55 \mathrm{~g}$[/tex]
mass of [tex]$\mathrm{Na} 2 \mathrm{CO} 3$[/tex]required [tex]$=0.55 \mathrm{~g}$[/tex]
Mass 0.120M HC is [tex]$=0.55 \mathrm{~g}$[/tex]
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A sample of a gas (15.0 mol) at 2.0 atm is expanded at constant temperature from 5 L to 19.5 L. calculate the final pressure.
Answer:
.512 ATM
Explanation:
P1V1 = P2V2
2 * 5 = P2 * 19.5
P2 = .512 ATM
In the reaction:
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
How does the equilibrium shift if the HCl concentration is increased?
Group of answer choices
A. To the reactants
B. No change will occur
C. To the products
D. The equilibrium will initially shift but eventually be uneffected.
The equilibrium shift if the HCl concentration is increased to the product.
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
What is effect of concentration on equilibrium?If the concentration of a substance is changed, then the equilibrium will shift in such a way that it minimise the effect of change which occur. If we increase the concentration of a reactant, then the equilibrium will shift to minimize the changes in the direction of the reaction which uses the reactants, so that the reactant concentration decreases.
Factor affecting concentration of reactionThe temperature: As we increasing the temperature, the average speed of the reactant molecules also increases. As many molecules move faster, the large number of molecules moving fast enough to react increases, make the faster formation of products.pressure and concentration of the system are the factors which affect equilibrium.Thus, we concluded that with increase in the concentration of reactant equilibrium shift forward.
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How to calculate the exact molarity of phosphoric acid using the first equivalence point with the use of Diprotic and Triprotic Ka's?
As we know that the equivalency point of moles of added base will be equal to the moles of original acid, this allows to determine the number of moles of original acid.
How do you find the concentration at the first equivalence point?At the equivalency point the moles of added base will be equal to the moles of original acid, this allows the determination of the number of moles of original acid. This can be combined with the original volume of the analyte solution in order to determine its concentration.
So we can conclude that at the equivalence point the moles of added base will be equal to the moles of original acid, this allows the determination of the number of moles of original acid.
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4 Fe(s) + 3 02(g)
--> 2 Fe₂O3(s)
1. What is the oxidation state of iron (Fe) in the reactant Fe(s)?
2. What is the oxidation state of oxygen (O) in the reactant O2(g)?
3. What is the oxidation state of iron (Fe) in the product Fe2O3(s)?
4. What is the oxidation state of oxygen (O) in the product Fe2O3(s)?
5. In this reaction, iron is... (oxidized or reduced?)
6. In this reaction, oxygen is... (oxidized or reduced?)
7. What was the oxidizing agent in this reaction: Fe(s) or O2(g)?
The oxidation number of reactant Fe is 0 while the oxidation number of iron in the product is +3
What s a redox reaction?The term redox reaction implies a reaction in which there is an increase in the oxidation number of a specie and the decrease in the oxidation number of another specie.
Now we have the answers as follows;
1) The oxidation number of reactant Fe is 0
2) The oxidation number of reactant oxygen is 0
3) The oxidation number of iron in the product is +3
4) The oxidation number of oxygen in the product is -2
5). Iron is oxidized in the reaction
6) Oxygen is reduced in the reaction
7) The oxidizing agent in this case is the oxygen atom
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Perform the following mathematical operation and report the answer to the appropriate number of significant figures. 5.4-4.21
Answer:
1.2 ( two significant digits)
Explanation:
5.4 - 4.21 answer should only have the the number of significant digits as the number in the equation with the least number of significant digits... in this case 5.4 is only two significant digits....so the answer should only have two significant digits
5.4 - 4.21 = 1.19 round to two digits = 1.2
Need the answer pretttty pleaseeeeee
Answer:
The answer would be D.
Explanation:
Whenever one has many of the same correlating numbers within in a pattern, the rest tend to follow. With the information I was given and not the actual plotting, that would be my answer.
us
Let's say that you were asked to find the
molecular formula for a compound given its
empirical formula, CH₂O, and the compound's
molar mass.
The first step in solving such a problem is to
calculate the molar mass for the empirical
formula. What is the molar mass of CH₂O?
(C=12.01 amu, H=1.008 amu, O=16.00 amu)
[?] g/mol CH₂0
1
Answer:
Molar mass = 30.026 g/mol
Explanation:
Let Molar mass be mm
mm of CH2O = 12.01 + 2(1.008) + 16.00
= 12.01 + 2.016 + 16.00 = 30.026 g/mol
select the common word on the outside of a shipping container that will alert you to the fact that the material inside is hazardous
The common word on the outside of a shipping container that will alert you to the fact that the material inside is hazardous is caution.
What are hazardous statements?Hazardous statements are those words or phrases that are labelled against chemicals which shows the degree of how dangerous the chemical are.
The common words that are used as hazardous statements which shows that a chemical is dangerous include the following:
Danger,Caution andWarning.Therefore, the common word on the outside of a shipping container that will alert you to the fact that the material inside is hazardous is caution.
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What is the mass of a 5.00cm3 piece of copper having a density of 8.96g/cm3
Answer:
44.8 grams
Explanation:
The density exists as a ratio comparing the mass of a piece of copper per 1 cm³. Since you have been given a new volume, you can set up a proportion to find the new mass.
[tex]\frac{8.96 grams}{1.00 cm^3} =\frac{?grams}{5.00cm^3}[/tex] <----- Proportion
[tex]44.8 = (1.00cm^3)(?grams)[/tex] <----- Cross-multiply
[tex]44.8= ?grams[/tex] <----- Divide both sides by 1.00
How many molecules in 5.68 g of ozone (O3)
Answer:
[tex]\boxed{\sf no.\ of \ molecules = 7.13 \times 10^{22} \ molecules}[/tex]
Explanation:
Given data::Mass in g = m = 5.68 g
Molar mass = M = (16)3 = 48 g/mol
Avogadro's number = [tex]N_A[/tex] = 6.023 × 10²³
Required:No. of molecules = ?
Formula:[tex]\displaystyle no.\ of \ molecules = \frac{m}{M} \times N_A[/tex]
Solution:Put the givens in the above formula
[tex]\displaystyle no. \ of \ molecules =\frac{5.68}{48} \times 6.023 \times 10^{23}\\\\no. \ of\ molecules = 0.12 \times 6.023 \times 10^{23}\\\\no. \ of \ molecules = 0.713\times 10^{23}\\\\no.\ of \ molecules = 7.13 \times 10^{22} \ molecules\\\\\rule[225]{225}{2}[/tex]
Please help thank you so much
The two compounds that are the correct enol tautomers of 2-butnone are the structures shown in Option B.
What is Keto Enol Tautomerism?Isomerism is a situation in which two compounds have the same molecular formula but do not have the same structural formula. This occurs because the atoms in the molecule are arranged differently in space. One of the types of isomerism that we have is the Keto Enol Tautomerism. The Keto Enol Tautomerism occurs between the Keto and the enol forms of a compound via the movement of electrons. It is common in ketone compounds.
In this case, we can see that the compound 2-butanone can give rise to two enol compounds that have the same molecular formula as the 2-butanone.
The two compounds that are the correct enol tautomers of 2-butnone are the structures shown in Option B.
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What is the oxidation number of chlorine in KClO3?
Group of answer choices
A. +5
B. +1
C. -5
D. -1
The oxidation number of chlorine in KClO3 is +5 (option A).
How to calculate oxidation number?The oxidation number of an element is the hypothetical charge of an atom within a molecule.
The oxidation number of an element like chlorine in a compound like Pottasium chlorate can be calculated as follows:
The oxidation number of the elements in KClO3 is as follows:
K = +1Cl = xO = -21 + x - 2(3) = 0
x - 5 = 0
x = +5
Therefore, the oxidation number of chlorine in KClO3 is +5.
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How to recover ballpoint ink washed off from a paper?
The first step in clearing a clogged ballpoint pen is to exert additional pressure when scrawling and drawing vertical lines on paper. If this approach doesn't work, dip the pen's tiny tip in rubbing alcohol. [Only the tidbit] Any dried-up or hardened ink on the tip will dissolve with this.