How many oxygen molecules are produced when 3.2×1022 molecules of water decompose?
__H2O à __H2 + __O2
Answer: 1.6x10^22
Explanation: H2O —> H2 + 1/2O2 so half the number of water molecules
What is the volume of 67.1g of ethyl alcohol, which has a density of 0.79 g/mL?
Answer:
[tex]84.94\ \text{mL}[/tex]
Explanation:
[tex]m[/tex] = Mass of ethyl alcohol = [tex]67.1\ \text{g}[/tex]
[tex]\rho[/tex] = Density of ethyl alcohol = [tex]0.79\ \text{g/mL}[/tex]
[tex]V[/tex] = Volume of ethyl alcohol
Density is given by
[tex]\rho=\dfrac{m}{V}\\\Rightarrow V=\dfrac{m}{\rho}\\\Rightarrow V=\dfrac{67.1}{0.79}\\\Rightarrow V=84.94\ \text{mL}[/tex]
The volume of ethyl alcohol is [tex]84.94\ \text{mL}[/tex].
What is POH?
A. pH = log[OH-]
B. POH =[ht][OH-]
C. pOH = -log(OH)
D. pH = -log[H+]
Answer:
The answer is C
Explanation:
2.2.2: The pH Scale
pOH = -log[OH-]
Briefly explain how will you describe which object is moving fast and which one is moving slow?
A 0.0300 mol sample of NO2(g) is placed in a rigid 1.00 L reaction vessel and allowed to reach equilibrium at a certain temperature. What is the value of Kc at this temperature if 0.00500 mol of N2O4(g) is present at equilibrium
Answer:
12.5
Explanation:
Step 1: Write the balanced equation
2 NO₂(g) ⇄ N₂O₄(g)
Since the reaction takes place in a 1.00 L vessel, the initial concentration of NO₂ is 0.0300 M and the concentration at equilibrium of N₂O₄ is 0.00500 M.
Step 2: Make an ICE chart
2 NO₂(g) ⇄ N₂O₄(g)
I 0.0300 0
C -2x +x
E 0.0300-2x x
Step 3: Find the value of x
Since [N₂O₄]eq = 0.00500 M, x = 0.00500
Step 4: Calculate the concentrations at equilibrium
[NO₂] = 0.0300-2(0.00500) = 0.0200 M
[N₂O₄] = 0.00500 M
Step 5: Calculate the concentration equilibrium constant (Kc)
Kc = [N₂O₄]/[NO₂]²
Kc = 0.00500/0.0200²
Kc = 12.5
Sometimes atoms form molecules by sharing two pairs of valence electrons. When this occurs, the atoms are said to be joined by...
Answer:
A double covalent bond
Explanation:
A double covalent bond is a situation where we have two pairs of electrons shared together between the atoms instead of just one pair. Oxygen gas is an example of a simple molecule that contains double bonds.
In other words, it is a type of chemical bond that has 2 electron pairs shared between two atoms.
Type the correct answer in the box. Spell all words correctly.
What forms the backbone of a DNA strand?
A DNA molecule is made up of building blocks known as nucleotides. Each nucleotide consists of deoxyribose, a phosphate group, and one of the chemical bases. The nucleotides join together to form a _______
, which form the backbone of a DNA strand.
7.
How many grams are contained in 3.9 x 1023 sulfur atoms?
atoms → moles
grams
I
Answer: 20.775 g S
Explanation: 3.9x10^23 atoms = 0.648 mol
Atomic mass S = 32.08
S in grams = 20.775
How many grams are in 4.63 x 1024
molecules of CCl4?
Answer:
[tex]m=1,182.8g[/tex]
Explanation:
Hello!
In this case, since the relationship between molecules and mass is first analyzed via the Avogadro's number to compute the moles in the given molecules:
[tex]mol=4.63x10^{24}molec*\frac{1mol}{6.022x10^{23}molec}=7.69mol[/tex]
We now use the molar mass of carbon tetrachloride (153.81 g/mol) to obtain the required grams:
[tex]m=7.69mol*\frac{153.81g}{1mol} \\\\m=1,182.8g[/tex]
Best regards!
4.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 152. gimol, is burned completely in excess oxygen, and the mass of the products carefully measured:
product mass
carbon dioxide 5.79 g
water 2.84 g
Use this information to find the molecular formula of X.
Answer:
C₄H₁₀O₄
Explanation:
From the question given above, the following data were obtained:
Mass of compound = 4 g
Molar mass of compound = 152 g/mol
Mass of CO₂ = 5.79 g
Mass of H₂O = 2.84 g
Molecular formula of compound X =?
Next, we shall determine the mass of Carbon, Hydrogen and Oxygen in the compound. This can be obtained as follow:
For Carbon (C):
Mass of CO₂ = 5.79 g
Molar mass of CO₂ = 12 + (2×16) = 44 g/mol
Mass of C = 12/44 × 5.79
Mass of C = 1.58 g
For Hydrogen (H):
Mass of H₂O = 2.84 g
Molar mass of H₂O = (2×1) + 16 = 18 g/mol
Mass of H = 2/18 × 2.84
Mass of H = 0.32 g
For Oxygen (O):
Mass of C = 1.58 g
Mass of H = 0.32 g
Mass of compound = 4 g
Mass of O =?
Mass of O = (Mass of compound) – (Mass of C + Mass of H)
Mass of O = 4 – (1.58 + 0.32)
Mass of O = 4 – 1.9
Mass of O = 2.1 g
Next, we shall determine the empirical for compound X. This can be obtained as follow:
C = 1.58 g
H = 0.32 g
O = 2.1 g
Divide by their molar mass
C = 1.58 / 12 = 0.13
H = 0.32 / 1 = 0.32
O = 2.1 / 16 = 0.13
Divide by the smallest
C = 0.13 / 0.13 = 1
H = 0.32 / 0.13 = 2.46
O = 0.131 / 0.13 = 1
Multiply by 2 to express in whole number
C = 1 × 2 = 2
H = 2.46 × 2 = 5
O = 1 × 2 = 2
Thus, the empirical formula for the compound is C₂H₅O₂
Finally, we shall determine the molecular formula for the compound. This can be obtained as follow:
Molar mass of compound = 152 g/mol
Empirical formula => C₂H₅O₂
Molecular formula =?
Molecular formula => [C₂H₅O₂]ₙ
[C₂H₅O₂]ₙ = 152
[(2×12) + (5×1) + (2×16)]n = 152
[24 + 5 + 32]n = 152
61n = 152
Divide both side by 61
n = 152 / 61
n = 2
Molecular formula => [C₂H₅O₂]₂
Molecular formula => C₄H₁₀O₄
which formula represents a molecule solid
Dry ice are the molecule which represent molecular solid. Hence option c is correct.
What are molecule?Molecules are defined as the lowest identifiable unit into which a pure material can be divided while maintaining its chemical makeup and attributes is made up of two or more atoms. When two or more atoms come together and form bonds with one another, a molecule is created. Each atom shares an electron when a bond is formed between them. A molecule is created as a result of a covalent bond.
Molecular solid are defined as composed of atoms or molecules joined by hydrogen bonds, London dispersion forces, and dipole-dipole forces. Solids made of molecules and held together by van der Waals forces are referred to as molecular solids. Examples include carbon dioxide, hydrogen, etc. Crystalline solids include ZnS. The ionic solid MgO is. Diamond is organized in a network.
Thus, dry ice are the molecule which represent molecular solid. Hence option c is correct.
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Your question is incomplete, but probably your complete question was
Which of the following is an example of molecular solid?
a. Zinc sulphide
b. Magnesium oxide
c. Dry ice
d. Diamond
If I use warm water on my plants then they will grow faster as hot water increases metabolism this is an example of
Answer:
The options are
A. a hypothesis
B. a theory
C. a research question
D. a scientific explanation
The answer is A. a hypothesis
Explanation:
A hypothesis is referred to as a brief explanation on the occurrence of an event.
In the example above using of warm water on plants was inferred to make it grow faster as hot water increases the metabolism.
How many hydrogen atoms in the
molecule (NH4)2C8H402?
Answer:
12 hydrogen atoms
Explanation:
Let's consider the chemical formula of the compound (NH₄)₂C₈H₄O₂.
We can see the ammonium ion, NH₄⁺, which contains 4 hydrogen atoms. However, this ion is enclosed in parenthesis with a subindex 2. That means that we have to multiply the whole ion by 2, therefore resulting in 8 atoms of hydrogen. Then, in C₈H₄O₂, we can see another 4 hydrogen atoms. The total number of hydrogen atoms in 1 molecule of (NH₄)₂C₈H₄O₂ is 8 + 4 = 12 hydrogen atoms.
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 200. mL flask with 3.9 atm of sulfur dioxide gas and 3.2 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.6 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits.
Answer:
0.20
Explanation:
Step 1: Write the balanced equation
2 SO₂(g) + O₂(g) ⇄ 2 SO₃(g)
Step 2: Make an ICE chart
2 SO₂(g) + O₂(g) ⇄ 2 SO₃(g)
I 3.9 3.2 0
C -2x -x +2x
E 3.9-2x 3.2-x 2x
Step 3: Find the value of x
The partial pressure at equilbrium of SO₃ is 1.6 atm. Then,
2x = 1.6 atm
x = 0.80 atm
Step 4: Calculate the partial pressures at equilibrium
pSO₂ = 3.9-2(0.80) = 2.3 atm
pO₂ = 3.2-0.80 = 2.4 atm
pSO₃ = 1.6 atm
Step 5: Calculate the pressure equilibrium constant
Kp = pSO₃² / pSO₂² × pO₂
Kp = 1.6² / 2.3² × 2.4
Kp = 0.20
Which body system or systems are affected by asthma?
Answer:
The lungs
Explanation:
Asthma is a disease that affects the airways of your lungs. With asthma, your airways' lining tends to always be in a hypersensitive state characterized by redness and swelling. Causing the airways to swell and, in severe cases, close completely off.
hope this helps, this should also probably be in biology:)
if you are provided with 34.5 g iron (iii) chloride and 25.3 g sodium carbonate what is the limiting ractant
Answer:
Sodium carbonate, Na₂CO₃ is the limiting
Explanation:
We'll begin by writing the balanced equation for the reaction between iron (iii) chloride, FeCl₃ and sodium carbonate, Na₂CO₃.
This is illustrated below:
2FeCl₃ + 3Na₂CO₃ → Fe₂(CO₃)₃ + 6NaCl
Next, we shall determine the masses of FeCl₃ and Na₂CO₃ that reacted from the balanced equation. This can be obtained as follow:
Molar mass of FeCl₃ = 56 + (3×35.5)
= 56 + 106.5
= 162.5 g/mol
Mass of FeCl₃ from the balanced equation = 2 × 162.5 = 325 g
Molar mass of Na₂CO₃ = (2×23) + 12 + (3×16)
= 46 + 12 + 48
= 106 g/mol
Mass of Na₂CO₃ from the balanced equation = 3 × 106 = 318 g
SUMMARY:
From the balanced equation above,
325 g of FeCl₃ reacted with 318 g of Na₂CO₃.
Finally, we shall determine the limiting reactant. This can be obtained as follow:
From the balanced equation above,
325 g of FeCl₃ reacted with 318 g of Na₂CO₃.
Therefore, 34.5 g of FeCl₃ will react with = (34.5 × 318)/325 = 33.76 g of Na₂CO₃.
From the calculations made above, we can see clearly that it will take a higher amount (i.e 33.76 g) of Na₂CO₃ than what was given (i.e 25.3 g) to react completely with 34.5 g of FeCl₃. Therefore, Na₂CO₃ is the limiting reactant and FeCl₃ is the excess reactant.
How would you make 5mls of a solution that is 2.0% lactose and 0.1M SPG buffer from separate stock solutions that are 6% lactose and 1M SPG in concentration
Answer:
Check the explanation section.
Explanation:
The following steps should be followed orderly.
STEP ONE:
Use the dilution equation in the calculation of the volume for the stock solution. That is, C1 × V1 = C2 × V2.
Where C1 and C2 are the concentration of the stock solution and the diluted solution.
STEP TWO:
Put 6% of lactose and make sure to dilute it in order to make 2.0% lactose
and put it in Beaker A. Also, make sure to dilute the 1M to 0.1M SPG buffer in Beaker B.
STEP TWO:
Now, from beaker A containing 2% lactose, measure and remove 5.0 mL from it. Also, measure and remove 5.0 mL from beaker B containing 0.1M SPG.
So, in STEP TWO above we won't know how much water we need to use for dilution, thus, there is the need to make use of STEP ONE.
Therefore, from STEP ONE ABOVE, we have the dilution equation given as;
C1 × V1 = C2 × V2.
Hence, 6 × V1 = 2 × 5. Therefore, the volume needed from the stock solution, V1 = (2 × 5)/ 6 = 1.6 mL.
STEP THREE:
Now measure out 1.6 mL from the stock solution, that is 6% lactose and add it to 5mL of the diluted solution of 2% in beaker A into another container, say beaker C and add H2O to form SOLUTION X.
STEP FOUR:
Using the dilution equation again, Determine the the volume that is needed from 1M SPG.
C1 × V1 = C2 × V2.
V1 = ( 0.1 × 5)/ 1 = 0.5mL.
STEP FIVE:
measure 0.5mL out from the 1M SPG and 5 mL out of 0.1M SPG buffer and add water to it to form SOLUTION Y.
STEP SIX:
Now, mix solution X and solution Y together and take the required 5ml
A chemist determines by measurements that moles of nitrogen gas participate in a chemical reaction. Calculate the mass of nitrogen gas that participates.
Answer:
0.56 g
Explanation:
A chemist determines by measurements that 0.020 moles of nitrogen gas participate in a chemical reaction. Calculate the mass of nitrogen gas that participates.
Step 1: Given data
Moles of nitrogen gas (n): 0.020 mol
Step 2: Calculate the molar mass (M) of nitrogen gas
Molecular nitrogen is a gas formed by diatomic molecules, whose chemical formula is N₂. Its molar mass is:
M(N₂) = 2 × M(N) = 2 × 14.01 g/mol = 28.02 g/mol
Step 3: Calculate the mass (m) corresponding to 0 0.020 moles of nitrogen gas
We will use the following expression.
m = n × M
m = 0.020 mol × 28.02 g/mol
m = 0.56 g
Mercury, also known as quicksilver, is a metallic element and a liquid at room temperature. Calculate mercury's density if a sample of mercury is found to have a mass of 685.0685.0 g and a volume of 51.3951.39 mL. density: g/mL
Answer:
13.33g/mL is mercury's density
Explanation:
The density of a substance is defined as the ratio between the mass of the substance and the space that occupy. We can express the density of mercury in g/mL:
Grams mercury: 685.0g
Volume = 51.39mL
That means the density of the mercury is:
685.0g / 51.39mL
13.33g/mL is mercury's densityContainer A holds 717 mL of an ideal gas at 2.80 atm. Container B holds 174 mL of a different ideal gas at 4.30 atm. Container A and container B are glass spheres connnected by a tube with a stopcock. Container A is larger than container B. If the gases are allowed to mix together, what is the resulting pressure
Answer:
3.09 atm
Explanation:
Given that:
Volume of container A = 717 mL
Pressure of container A = 2.80 atm
Volume of container B = 174 mL
Pressure of container B = 4.30 atm
Now, if the valve are being removed and the gases are allowed to mix together; then
The total final pressure can be calculated by using the formula:
[tex]P_f = \dfrac{P_AVA+P_BV_B}{V_A+V_B}[/tex]
[tex]P_f = \dfrac{2.80*717+4.30*174}{717+174}[/tex]
[tex]P_f = \dfrac{2007.6+748.2}{891}[/tex]
[tex]P_f = \dfrac{2755.8}{891}[/tex]
[tex]\mathbf{P_f =3.09 \ atm}[/tex]
The absence of the intermolecular attraction between the atoms or molecules is called an ideal gas. The pressure of the resultant mixture is 3.09 atm.
What is the relation between pressure and volume?The relationship between the pressure and the volume of the gas is given by Boyle's law which states the inverse proportionality relation with the volume.
Given,
The volume of container A = 717 mL
The volume of container B = 174 mL
The pressure of container A = 2.80 atm
The pressure of container B = 4.30 atm
The total final pressure of the ideal gas of the mixture is calculated by:
[tex]\begin{aligned} \rm P_{f} &= \rm \dfrac{P_{A}V_{A}+ P_{B}V_{B}}{V_{A}+V_{B}}\\\\&= \dfrac{2007.6 +748.2}{891}\\\\&= 3.09 \;\rm atm\end{aligned}[/tex]
Therefore, the total pressure of the mixture is 3.09 atm.
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What is the density of lead (in g/cm^3 3 ) if a rectangular bar measuring 0.500 cm in height, 1.55 cm in width, and 25.00 cm in length has a mass of 220.9 g? Report the answer with the units of g/cm^3 3 and the proper number of significant figures. Numbers in bold count towards significant figures. Type your answer here with correct significant figures and units:
Answer:
Density = 11.4 g/cm³
Explanation:
Given data:
Density of lead = ?
Height of lead bar = 0.500 cm
Width of lead bar = 1.55 cm
Length of lead bar = 25.00 cm
Mass of lead bar = 220.9 g
Solution:
Density = mass/ volume
Volume of bar = length × width × height
Volume of bar = 25.00 cm × 1.55 cm × 0.500 cm
Volume of bar = 19.4 cm³
Density of bar:
Density = 220.9 g/ 19.4 cm³
Density = 11.4 g/cm³
Which change happens during evaporation?
A. A gas turns into a liquid.
B. A liquid turns into a gas.
C. A solid turns into a liquid.
D. A liquid turns into a solid.
Answer:
B.) A Liquid turns into Gas.
Which number should go in the blank?
- H₂ + O2 -> 2H₂O
O
2
3
1
PLEASE HELP ITS DUE IN 1 HOUR!!!!!!
Answer: Sorry I try to download it but it not showing anything, if you take a picture of the work maybe I would do it....
Explanation:
A 2.912 g sample of a compounds containing only C, H, and O was completely oxidized in a reaction that yielded 3.123 g of water and 7.691 g of carbon dioxide. Determine the empirical formula and molecular formula of the compound if it has a molar mass of 100.1 g/mol.
Answer:
Explanation:
18 gram of water contains 2 g of hydrogen
3.123 gram of water will contain 2 x 3.123 / 18 = .347 g of hydrogen .
44 gram of carbon dioxide contains 12 g of carbon
7.691 gram of carbon dioxide will contain 12 x 7.691 / 44 = 2.1 g of carbon .
So the sample will contain 2.912 - ( .347 + 2.1 ) g of oxygen .
= .465 g of oxygen .
moles of Carbon = 2.1 / 12 = .175
moles of hydrogen = .347 / 1 = .347
moles of oxygen = .465 / 16 = .029
Ratio of moles of carbon , oxygen and hydrogen ( C,O,H )
= 0.175 : 0.029 : 0.347
= .175/ .029 : 1 : .347 / .029
= 6 : 1 : 12
So empirical formula = C₆H₁₂O
Let the molecular formula be [tex](C_6H_{12}O)_n[/tex]
molecular weight = n ( 6 x 12 + 12x 1 + 16)
= 100 n
Given 100 n = 100.1
n = 1
Molecular formula = C₆H₁₂O.
How can you make an item that is made of magnetic material become a permanent magnet instead of a temporary magnet? *.
Answer:
You can heat it and then let it cool it in a very strong magnetic field.
It can be heated and then allowed to cool in a very powerful magnetic field. To make an item that is made of magnetic material become a permanent magnet instead of a temporary magnet.
What is magnetic field ?The magnetic influence on moving electric charges, electric currents, and magnetic materials is described by a magnetic field, which is a vector field. A force perpendicular to the charge's own velocity and the magnetic field acts on it when the charge is travelling through a magnetic field.
Heating a ferromagnetic material to a crucially high temperature is the primary method for producing permanent magnets. Although the temperature varies depending on the type of metal, it has the effect of aligning and "fixing" the magnet's domains in place over time.
Electric charges in motion are what generate magnetism. The smallest building blocks of matter are called atoms. Each atom contains electrons, which are tiny particles with electric charges.
Thus, It can be heated and then allowed to cool in a very powerful magnetic field.
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Smallest particle of a substance that can retain its properties & is
composed of one or more atoms *
O A. Atom
O B. Molecules
O C. Matter
O D. Everything
Answer:
Molecules
Explanation:
Find the atomic mass unit of Silicon-28, Silicon-29, Silicon-30 with masses of 27.977, 28.976, 29.974, respectively.
Answer:
28.085
Explanation:
The formular to obtain average atomic mass unit from isotopes is given as;
sum of (Percentage abundance * Atomic mass) of all isotopes = Average atomic mass unit
Silicon 28 = 92.23%
Silicon 29 = 4.67%
Silicon 30 = 3.1%
(92.23 / 100 * 27.977) + (4.67 / 100 * 28.976) + (3.1 / 100 * 29.974) = Average atomic mass
Average atomic mass = 25.803 + 1.353 + 0.929 = 28.085
Draw a Lewis structure for H3O+ . Include all hydrogen atoms and show all unshared electrons and the formal charges, if any. Assume that bonding follows the octet rule.
Answer:
In this Lewis equation it can be seen how oxygen and hydrogen have a dative union, that is, there is a proton that is temporarily "borrowed"
Explanation:
This molecule is the same as water but with one more hydrogen, that is why the general charge of the molecule is positive
What is the Scientific notation for 0.10050
Answer:
1.005 x [tex]10^{1}[/tex]
Explanation: