whats the question?
PLSSS HELP!! In the demonstration, Iron reacted with the oxygen in the air. Which one ran out
first? How do you know?
is water vapor only found in hot water?
HELP PLEASE
Instantaneous speed is the rate of motion at an instant in time. Based on this statement, a reasonable conclusion is that if and object's instantaneous speed does not chang over time then,________.
•the object is quickly speeding up
•the object is very gradually slowing down
•the object is moving at a constant speed
•the object has returned to its beginning position
Answer:
The object is moving at a constant speed.
Classify each of the compounds as an ionic compound, a covalent compound or an acid.a. BaCl2______________________d. CH4______________________b. MnO2______________________e. H2S*______________________c. H3AsO4______________________f. CH3OH
Answer:
a. BaCl2 is ionic compound.
b. CH4 is covalent compound.
b. MnO2 is ionic compound.
e. H2S is covalent compound.
c. H3AsO4 is ionic compound.
f. CH3OH is covalent compound.
Explanation:
BaCl2, MnO2 and H3AsO4 are ionic compounds due to the presence of ionic bond between the atoms while on the other hand, CH4, H2S and CH3OH are covalent compounds due to the presence of covalent bond between their atoms. In covalent bonds, sharing of electrons occur whereas in ionic bonds, complete transfer of electrons occur from one atom to another atom.
11. A 4.175 gram sample of a certain hydrate of copper (II) sulfate, CuSO,• xH,O, is heated until all
the water is driven off. The resulting anhydrous compound weighs 3.120 grams. What is the
formula of the hydrate?
The formula of the hydrate = CuSO₄• 3H₂O
Further explanationGiven
4.175 grams sample CuSO₄• xH₂O
3.120 grams anhydrous compound CuSO₄
Required
The formula
Solution
mass of H₂O driven off :
= 4.175 - 3.12
= 1.055 g
MW CuSO₄ = 159.5 g/mol
MW H₂O = 18 g/mol
mol ratio of CuSO₄ : H₂O :
= 3.12/159.5 : 1.055/18
= 0.01956 : 0.05861
= 1 : 3
Based on the data provided, the formula of the hydrated salt is CuSO4.3H20
What is the formula of the hydrate?The formula of the hydrate is determined from the mole ratio of the anhydrous saltand water.
Mass of water = 4.175 - 3.120
mass of water = 1.055 g
Mole ratio= mass/molar mass
molar mass of CuSO4 = 160 g/mol
molar mass of H2O = 18 g/mol
CuSO4 = 3.120/160 = 0.0195
H2O = 1.055/18 = 0.0586
CuSO4 = 0.0195/0.0195 = 1
H2O = 0.0586/0.0195 = 3
Therefore, the formula of the hydrated salt is CuSO4.3H20
Learn more about hydrated salts at: https://brainly.com/question/24920157
what is the molarity of a solutoin which contains 38.5 g of sodium chloride disolved in 325 ml solution ?
Answer:
Molarity = 2.02 M
Explanation:
Given data:
Molarity of solution = ?
Mass of sodium chloride = 38.5 g
Volume of solution = 325 mL (0.325 L)
Solution:
Number of moles = mass/molar mass
Number of moles = 38.5 g/ 58.44 g/mol
Number of moles = 0.658 mol
Molarity:
Molarity = number of moles / volume of solution in L
Molarity = 0.658 mol /0.325 L
Molarity = 2.02 M
Which two elements have similar characteristics?
Answer:
The two elements are FLUORINE AND CHLORINE. These two elements have similar characteristics because they belong to the same group in the periodic table. On the periodic table, elements with similar properties are grouped together in the same group. Both chlorine and fluorine belongs to the halogen group.
Explanation:
Hope it helps, some how.
When C2H4(g) reacts with H2O(g) to form CH3CH2OH(g) according to the following equation, energy is released into the surroundings. C2H4(g) H2O(g) CH3CH2OH(g) Is this reaction endothermic or exothermic
Answer:
Exothermic
General Formulas and Concepts:
Chemistry
Thermodynamics
Exothermic - releases heat as a productEndothermic - absorbs heat as a reactantExplanation:
We are given that the reaction takes place between C₂H₄ (g) and H₂O (g) to form CH₃CH₂OH (g) and is releasing heat.
This means that heat would be product as it is being released during the reaction.
Therefore, we have an exothermic reaction.
If you have a gas sample with a pressure of 2 atm, a volume of 40 L and a temperature of 300 K, what will be the number of moles of gas in that sample?
Answer:
n = 3.25 mol
Explanation:
Given data:
Pressure of sample = 2 atm
Volume of sample = 40 L
Temperature = 300 K
Number of moles = ?
Solution:
PV = nRT
R = general gas constant = 0.0821 atm.L/mol.K
2 atm ×40 L = n × 0.0821 atm.L/mol.K × 300 K
80 atm.L = n × 24.63 atm.L/mol
n = 80 atm.L /24.63 atm.L/mol
n = 3.25 mol
An irregularly-shaped piece of aluminum (Al) has a mass of 66.0 grams. What is the volume in cm³ of this piece of aluminum if its density is 2.70 g/cm³?
Answer:
[tex]V=24.45\ \text{cm}^3[/tex]
Explanation:
Given that,
Mass of a piece of Aluminium, m = 66 grams
The density of Aluminium, d = 2.70 g/cm³
We need to find the volume of this piece in cm³.
We know that,
Density = mass per unit volume
[tex]d=\dfrac{m}{V}\\\\V=\dfrac{m}{d}\\\\V=\dfrac{66\ g}{2.7\ g/cm^3}\\\\V=24.45\ \text{cm}^3[/tex]
So, the volume of the piece is [tex]24.45\ \text{cm}^3[/tex].
WHICH ONE IS TRUE WHICH ONE IS FALSE?
The number of valence electrons decreases from left to right across each period.
The number of valence electrons increases from top to bottom within each group.
All of the elements in group 9 have nine valence electrons.
Elements with the most valence electrons are in group 18.
Answer:
The number of valence electrons increases from top to bottom within each group.
Explanation:
The valence electrons are the outermost shell electrons.
Therefore, the number of valence electrons does not increase from top to bottom within each of the group.
Down a group, the number of valence electrons remains the same.
For group I elements, the number of electrons is 1.
The group is the vertical arrangement of elements.
From left to right across a period, the number of valence electrons increases because you move from group to group.
Can anybody answer this question of chemistry?
Answer:
Answer:A
Answer:AExplanation:
Answer:AExplanation:Molar Mass of glucose = (6×12)+(1×12)+(16×6)= 180g/mol
= 180g/molNumber of moles of Glucose = Mass/Molar Mass
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778moles
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556moles
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556molesMass of ethanol= Molar Mass of ethanol × Number of moles
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556molesMass of ethanol= Molar Mass of ethanol × Number of moles={(12×2)+(1×6)+16} × 55.5556
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556molesMass of ethanol= Molar Mass of ethanol × Number of moles={(12×2)+(1×6)+16} × 55.5556= 46.5×55.5556
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556molesMass of ethanol= Molar Mass of ethanol × Number of moles={(12×2)+(1×6)+16} × 55.5556= 46.5×55.5556= 2555.55
Answer:
Answer:A
Answer:AExplanation:
Answer:AExplanation:Molar Mass of glucose = (6×12)+(1×12)+(16×6)= 180g/mol
= 180g/molNumber of moles of Glucose = Mass/Molar Mass
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778moles
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556moles
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556molesMass of ethanol= Molar Mass of ethanol × Number of moles
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556molesMass of ethanol= Molar Mass of ethanol × Number of moles={(12×2)+(1×6)+16} × 55.5556
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556molesMass of ethanol= Molar Mass of ethanol × Number of moles={(12×2)+(1×6)+16} × 55.5556= 46.5×55.5556
= 180g/molNumber of moles of Glucose = Mass/Molar Mass= 5000/180= 27.7778molesIn the balanced equation of fermentation, the ratio of glucose to ethanol is 2:1Therefore the number of moles of ethanol is 2×27.7778=55.5556molesMass of ethanol= Molar Mass of ethanol × Number of moles={(12×2)+(1×6)+16} × 55.5556= 46.5×55.5556= 2555.55
Assign oxidation numbers to the element in each of the following compounds. Remember an oxidation number is for one atom of the element.
a. HgO
b. Al4C3
c. CrF2
d. Fe2S3
Answer:
a. x = + 2
b. x = + 3
c. x = + 2
d. x = + 3
Explanation:
The oxidation number is a formal charge assigned to an atom present in a molecule or formula unit or ion based on some arbitrary rules.
a.
HgO
The oxidation number of Hg in HgO is:
x + (-2) = 0
x = +2
b.
Al₄C₃
The oxidation number of Al in Al₄C₃ is:
4x +(3 × -4) = 0
4x - 12 = 0
4x = +12
x = 12/4
x = +3
c. CrF₂
x + ( 2 × - 1) = 0
x - 2 = 0
x = + 2
d. Fe₂S₃
2x + ( 3 × - 2) = 0
2x + (-6) = 0
2x = 6
x = 6/2
x = +3
Decide whether the compound is ionic or molecular, if you can.
Compound is a soft waxy white solid that can be easily shaped and molded by hand. When the flame of an ordinary laboratory burner is held about away from the solid, it rapidly and extensively melts into a clear liquid.
Answer:
Molecular solid
Explanation:
Molecular solids have a very low melting point. This is because, they are composed of weak intermolecular forces hence the layers of the solid easily fall apart as the solid melts.
We can see here that the solid being considered melts easily. Hence we can conclude that it is actually a molecular solid.
all organisms begins life as a ________ cell.
Answer:
All organisms begin life as a single cell
Explanation:
Single cell also did you know 15 minutes can save you 15% more on car insurance
the number that go before symbols and formulas in a chemicql equation are
A.SuperScripts
B.Subscripts
C.Catalysts
D.Coefficients
12. Which gas has the greatest kinetic energy at STP?
a. He
b. Ne
c. Ar
d. none of the above (all have the same kinetic energy)
Answer:
d. none of the above (all have the same kinetic energy)
Explanation:
The kinetic theory of gases states that the molecules of an ideal gas experience a constant random motion.
At standard temperature and pressure (STP), the kinetic energy of an ideal gas such as hydrogen, argon, neon, sodium, oxygen, helium, magnesium, beryllium, nitrogen, carbon, fluorine, chlorine etc are all the same.
The standard temperature and pressure (STP) of an ideal gas is 273K and 100 kPa.
Hence, all of the gases have the same kinetic energy at standard temperature and pressure (STP).
Kinetic energy can be defined as an energy possessed by an object or body due to its motion.
Mathematically, kinetic energy is given by the formula;
[tex] K.E = \frac{1}{2}MV^{2}[/tex]
Where, K.E represents kinetic energy measured in Joules.
M represents mass measured in kilograms.
V represents velocity measured in metres per seconds square.
Which constants would most likely be filled in the first row of the table?
O temperature and moles of gas
O volume and temperature
O
pressure and volume
pressure and moles of gas
Answer:
A
Explanation:
Correct on edge
The temperature and moles of gas constants would most likely be filled in the first row of the table. Therefore, option A is correct.
What is gas constant ?The gas constant, denoted by R, is a physical constant that is expressed in terms of units of energy per temperature increment per mole. It's also referred to as the ideal gas constant, the molar gas constant, or the universal gas constant.
A general constant in the equation of state of gases that is equal to the product of the pressure and volume of one mole divided by the absolute temperature in the case of an ideal gas see gas law sense c.
All gases adapt an equation of state known as the ideal gas law: PV = nRT, where n is the number of moles of the gas and R is the universal gas constant.
Thus, option A is correct.
To learn more about the gas constant, follow the link;
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Your question is incomplete, most probably your question was
The incomplete table below shows selected characteristics of gas laws.
Name
Variables
Constants
Equation
?
?
?
PV = k
Charles's law
?
?
V = kT
?
Temperature, pressure
?
P = kT
Combined gas law
Pressure, temperature, volume
?
?
Which constants would most likely be filled in the first row of the table?
temperature and moles of gas
volume and temperature
pressure and volume
pressure and moles of gas