Answer:
decrease in temperature , decreases the kinetic movements of the gase molecules as a result decreases the frequency of collisions between gas molecules A and B consequently decreases the rate of reactions of gases A and BHow many molecules does 85.0 g HCl contain?
A. 2.04 x 10^24 molecules
B. 1.98 x 10^24 molecules
C. 1.40 x 10^24 molecules
D. 2.54 x 10^24 molecules
Answer: C. 1.40×10^24
Explanation:
To do this, we must convert this from grams to moles, then from moles to molecules. For the first step, you will need to find the molar mass of HCl on the periodic table, which is 36.461gHCl.
[tex]85.0gHCl*\frac{1molHCl}{36.461gHCl} =2.33molHCl[/tex]
Now that we have the moles, we must convert that to molecules by using Avogadro's number.
[tex]2.33molHCl*\frac{6.022*10^{24} }{1molHCl} =1.40*10^{24}[/tex]
Now we have our answer. The best answer choice here is C. 1.40×10²⁴.
I hope this helps! Pls mark brainliest!! :)
How many faradays are transferred in an electrolytic cell when a current of 2.0 A flows for 12 hours
The Faradays transferred during the process is 86400 C.
An electric current in a circuit is calculated by dividing the total charge that runs in the circuit with the total time taken.
I = Q/t
Rearrange the formula to express it in terms of charge.
Q = I x t
Calculations:
Convert 12 h to s.
12 h = (12 x 60 x 60) s = 43200 s
Substitute the values in the above formula.
Q = 2.0 C/s x 43200 s
= 86400 C
Therefore, the charge (Faradays) transferred in an electrolytic cell is 86400 C.
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What is one property of salts?
OA. They have a low pH.
O B. They are neutral.
O C. They have a high pH.
OD. They are very reactive.
Mercury (Hg) is present in trace amounts in coal, ranging from 50.0 to 200.0 ppb. A typical power plant burns 1.49 million tons of coal per year. Calculate tons of mercury in the coal based on the lower (50.0 ppb) and higher (200.0 ppb) concentrations.
Answer and Explanation:
To calculate this, simply use an equality of proportions:
50 particles : 1 billion particles = x tons : 1.49 million tons
The value of x can be solved for by multiplying the ratio on the left by the value 1.49 million / 1 billion:
So, x = (50)(0.00149) tons = 0.0745 tons
Then, do the same thing for the larger concentration:
x = (200)(0.00149) tons = 0.298 tons
state two properties of sulphur that makes it possible to extract using the frasch process
Explanation:
sulphur has a low melting point.
sulphur has a low boiling point thus it can be extracted by pumping hot water which turns it ito solution form
A piece of iron has a mass of 35,342 grams. Iron has a density of 7.9 grams per cubic centimeter. Find the volume of the piece of iron to the nearest cubic centimeter.
The volume of the piece of iron to the nearest cubic centimeter is 4473.6 cubic centimeter.
Calculation of volume:-density = mass / volume
volume = mass/ density
=35342/ 7.9
=4473.6 cubic centimeter
Describe density.The density of a substance indicates how dense it is in a given area. Mass per unit volume is the definition of a material's density. In essence, density is a measurement of how closely stuff is packed. It is a particular physical characteristic of a specific thing. The Greek scientist Archimedes made the discovery of the density principle. If you are familiar with the formula and the relevant units, calculating density is simple. The letter D can also be used to signify density instead of the symbol.
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If a naturally occurring sample of an unidentified element is found to contain three isotopes (A, B, and C) and consists of 90.5% isotope A (mass number 20), 0.3% isotope B (mass number 21), and 9.2% isotope C (mass number 22), the atomic weight of the element measured from the sample will be:
If a naturally occurring sample of an unidentified element is found to contain three isotopes (A, B, and C) and consists of 90.5% isotope A (mass number 20), 0.3% isotope B (mass number 21), and 9.3% isotope C (mass number 22), the atomic weight of the element measured from the sample will be greater than 21 amu.
To calculate the average atomic mass, multiply the fraction through the mass number for every isotope, then add them together. Whenever we do mass calculations concerning elements or compounds (combos of elements), we usually use average atomic loads.
For instance, carbon-14 is a radioactive isotope of carbon that has six protons and 8 neutrons in its nucleus. We name it carbon-14 because the overall range of protons and neutrons within the nucleus also called the mass number, provides up to fourteen (6+8=14).
Together, the quantity of protons and the range of neutrons determine an detail's mass variety. Due to the fact, that an element's isotopes have barely unique mass numbers, the atomic mass is calculated by obtaining the suggested mass numbers for its isotopes.
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How is a compound different than a
mixture?
a. A compound can be separated by physical
means.
b. A mixture can be separated by physical
means.
c. A mixture is made of only one type of
atom.
d. A compound is made of only one type of
atom
B
A mixture can be separated by a physical means because there is no chemical bond between the constituents
Use the periodic table to identify the element indicated by each electron configuration by typing in the
chemical symbol for the element.
1s22s22p6:
1s22s22p63s23p3:
1s22s22p53s23p54s1:
1s22s22p53s23p64s2308:
1s?2s?2p53s23p54s23d104p65s24d3:
Answer:
1s22s22p6: Neon (Ne)
1s22s22p63s23p3: Phosphorous (P)
1s22s22p63s23p64s1: Potassium (K)
1s22s22p63s23p64s2(im not sure what 308 is supposed to be): Calcium (Ca)
1s22s22p63s23p64s23d104p65s24d3: there is no pure element that ends 4d3 that I know of so this can either be Zirconium(Zr) if it ends in 4d2 or Niobium (Nb) if it ends in 4d4
Explanation:
you can look at the periodic table and the trends to find the rough idea of where the electron configuration ends, there are helpful articles and images on these, i attached an image that may help. After that you can look at the atomic number to find the number of electrons for a pure element and use the electron subshell pattern thing to find the exact number
What is the symbol of the species with 23 protons and 21 electrons?
Answers
V^2-
V^2+
Na^2+
Sc^2+
Na^2-
Sc^2-
[tex]V^{2+}[/tex]is the symbol of the species with 23 protons and 21 electrons.
Hence, option F is correct.
What is a proton?Electrons are a type of subatomic particle with a negative charge. Protons are a type of subatomic particle with a positive charge.
If it has 23 protons, then its proton number (also know as its atomic number) is 23. You can look that symbol up in your periodic table.
If it has 21 electrons then it has a net charge of 23(+) - 21. So we know the ionisation state of the species, and we can record that as a superscript after the symbol for the species.
Hence, [tex]V^{2+}[/tex] is the symbol of the species with 23 protons and 21 electrons.
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A sample of ethanol (C2H6O) has a mass of 0.2301 g. Complete combustion of this sample causes the temperature of a bomb calorimeter to increase by 1.33°C. The calorimeter has a mass of 2.000 kg and a specific heat of 2.45 J/g•°C.
The number of mole of ethanol present in the sample is 0.005 mole
Description of moleThe mole of a substance is related to it's mass and molar mass according to the following equation
Mole = mass / molar mass
With the above formula, we can obtain the mole of ethanol
How to determine the mole of ethanolMass of ethanol = 0.2301 gMolar mass of ethanol = 46 g/molMole of ethanol = ?Mole = mass / molar mass
Mole of ethanol = 0.2301 / 46
Mole of ethanol = 0.005 mole
Complete question
A sample of ethanol (C2H6O) has a mass of 0.2301 g. Complete combustion of this sample causes the temperature of a bomb calorimeter to increase by 1.33°C. The calorimeter has a mass of 2.000 kg and a specific heat of 2.45 J/g•°C. How many moles of ethanol are present in the sample?
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When butane burns completely, only water and carbon dioxide gas are produced. If 11.6 g of butane and 40.0 L of oxygen at 22.0o C and 102 kPa react, what volume of carbon dioxide gas also at 22.0o C and 102 kPa can be collected over water. The vapour pressure of water at 22.0o C is 2.24 kPa.
2C4H10(g) + 13O2(g) --> 10H2O(g) + 8CO2(g)
19.7 litre volume of carbon dioxide gas at 22.0o C and 102 kPa can be collected over water.
What is vapour pressure?Vapour pressure is a measure of the tendency of a material to change into the gaseous or vapour state, and it increases with temperature.
Moles of Butane = mass in grams / molar mass = 11.6 / 58.12 = 0.2
Volume of [tex]O_2[/tex] (V) = 40 liter
Temperature (T) = 22°C = 22 + 273 = 295 K
Pressure (P) = 102 kPa = 102 / 101.325 = 1.007 atm
Moles of [tex]O_2[/tex] (n) can be calculated by ideal gas equation.
PV = nRT
n = 1.007 40 ÷ 0.0821 295 = 1.663
Balanced chemical reaction;
2[tex]C_4H_10[/tex] + 13[tex]O_2[/tex] ---> 8[tex]CO_2[/tex] + 10[tex]H_2O[/tex]
From reaction;
13 moles [tex]O_2[/tex] require 2 moles [tex]C_4H_10[/tex]
So, 1.663 moles [tex]O_2[/tex] will require = 2 x 1.663 ÷13 = 0.256 moles of [tex]C_4H_10[/tex]
Thus [tex]C_4H_10[/tex] is a limiting reagent. So it will drive the yield of [tex]CO_2[/tex].
Moles of [tex]CO_2[/tex] produced = (8/2) 0.2 = 0.8 moles
Pressure of [tex]CO_2[/tex] (P) = 102 - 2.24 = 99.76 kPa = 99.76 ÷ 101.325 = 0.985 atm
Applying the ideal gas equation for [tex]CO_2[/tex],
PV = nRT
0.985 V = 0.8 0.0821 x 295
V = 19.7 liter
The volume of [tex]CO_2[/tex] produced = 19.7 liter.
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If you mix 200.0 mL of a 0.150 M solution of silver acetate with 2.500 g of copper metal you will get a single replacement reaction. What mass of Silver metal will you produce if the reaction has a 45.0% efficiency?
Answer: 2.11 g
Explanation:
[tex]$$Equation: $2 \mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{Cu}(s) \longrightarrow \mathrm{Cu}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+2 \mathrm{Ag}(s)$[/tex]
[tex]$$No of moles of $\mathrm{Ag}$ produced from $\mathrm{Cu}=2.500 \mathrm{~g} \times \frac{1 \mathrm{~mol} \mathrm{Cu}}{63.55 \mathrm{~g}} \times \frac{2 \mathrm{~mol} \mathrm{Ag}}{1 \mathrm{~mol} \mathrm{Cu}}$ $=0.07868 \mathrm{~mol} \mathrm{Ag}$[/tex]
[tex]$$No of moles of $\mathrm{Ag}$ produced from $\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}=200.0 \mathrm{~mL} \times \frac{1 \mathrm{~L}}{1000 \mathrm{~mL}} \times \frac{0.150 \mathrm{~mol} \mathrm{AgC_{2 } \mathrm { H } _ { 3 } \mathrm { O } _ { 2 }}}{1 \mathrm{~L}}$ $=0.0300 \mathrm{~mol} \mathrm{Ag}$[/tex]
[tex]Since $\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$ limits the production of $\mathrm{Ag}, \mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$ acts as the limiting reactant \\\\No of moles of Ag formed $=0.0300 \mathrm{~mol}$\\Theoretical yield of $\mathrm{Ag}=0.0300 \mathrm{~mol} \mathrm{Ag} \times \frac{108 \mathrm{~g}}{1 \mathrm{~mol} \mathrm{Ag}}=3.24 \mathrm{~g}$\\Actual yield of silver $=65.0 \%(3.24 \mathrm{~g})$$$=\frac{65.0}{100}(3.24 \mathrm{~g})=2.106 \mathrm{~g} \approx 2.11 \mathrm{~g}$$[/tex]
PLEASE HELP ASAP! very much appreciated
Answer:
-Unknown
Explanation:
Questions is not seen properly bro
If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its
volume at a pressure of 2.50 atm?
Answer:
the volume of the gas at 2.50 atm pressure is equal to 1.44 Litres.
Explanation:
Which of the following is an example of a change of state?
OA. A white wall is painted red.
B. Drops of water form on the outside of a cold glass.
O C. Corn is ground into flour.
D. A piece of paper turns into ash when it burns.
Answer:
Option B
Explanation:
For Option A the state is not changing but just has different look now. For Option B the state is changing from gas to liquid drops due to cold glass For Option C it hasn't changed state as both corn and flower is solidFor Option D paper and ash are both solidsTherefore our answer must be Option B
arrangement of element by atomic weights provided mendeleev with some elements that didn't fit the patterns such as argon. explain how this problem was eventually overcome
Answer:
this problem was eventually overcome by arranging elements by increasing atomic number instead of atomic weight.
This problem was eventually overcome by arranging elements by increasing atomic number instead of atomic weight.
What is an atomic weight?The total weight of an atom is called the atomic weight. It is approximately equal to the number of protons and neutrons, with a little extra added by the electrons.
Mendeleev arranged the elements in order of increasing weight and broke them into rows such that elements in each column shared valence, the number of other atoms they combined with, as well as other properties.
In his 1869 Periodic Table, Mendeleev left blanks with suggested atomic weights for elements he thought would be discovered someday. William Ramsay's discovery of argon initially posed a threat to the Periodic Table. At first, Mendeleev believed argon was not an element, because it didn't react with anything.
Hence, this problem was eventually overcome by arranging elements by increasing atomic number instead of atomic weight.
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In a __________ elimination, the base extracts a proton and the leaving group leaves simultaneously. In a __________ process, the leaving group leaves ___________ the base abstracts a proton. g
In a Base catalyst elimination, the base extracts a proton and the leaving group leaves simultaneously. In a Concentrated process, the leaving group leaves the base abstracts a proton.
Just as there are two mechanisms of substitution (SN2 and S N1), there are two
mechanisms of elimination (E2 and E1).
E2 mechanism — bimolecular elimination
E1 mechanism — unimolecular elimination
The E2 and E1 mechanisms differ in the timing of bond cleavage and bond formation, analogous to the SN2 and S N1 mechanisms.
E2 and S N2 reactions have some features in common, as do E1 and SN1 reactions.
Base removes a proton from the β-carbon atom,
while the halogen atom leaves from the α-carbon resulting in the formation of a π-bond. Such eliminations are also called β-eliminatione liminations are also called β elimination reactions
In a base-catalyzed elimination reaction, the base takes away a proton from the β position of the leaving group (the group that goes away with the bonding pair of electrons) and a double bond is formed. When the base is bulky it prefers to take away the proton from the less hindered position.
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BRAINLIST ASAP!!! Acid catalyzed dehydration-condensation reactions of carboxylic acids and alcohols produce chemicals called esters.
i. Using carbon skeletal notation, write the dehydration-condensation reaction that occurs between ethanol and butanoic acid
ii. What is the name of this ester?
The dehydration-condensation reaction occurs between 'ethanol' and 'butanoic acid' giving an ester called as "ethyl butanoate".
What is an ester and how it is formed?Esters are produced when carboxylic acids are heated with alcohols in the presence of an acid catalyst.
The catalyst is usually concentrated sulphuric acid.
Dry hydrogen chloride gas is used in some cases, but these tend to involve aromatic esters (ones containing a benzene ring).
Esters are represented by the formula RCOOR', where R and R' are hydrocarbon groups.
The chemical reaction occurring in the formation of the ester is known as an esterification reaction.
The reaction that occurs between ethanol and butanoic acid:
Ethanol reacts with butanoic acid in the presence of an acid-catalyst and gives ethyl butanoate as ester and water as products. If an acid reacts with a base, salt and water are the products. But ester is not a salt.
i) The carbon skeletal notation for the given reaction is shown below.
ii) The ester is named "ethyl butanoate".
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A key element to successful response to a chemical, biological, or radiological incident is the rapid identification of the hazard and immediate:
A key element to a successful response to a chemical, biological, or radiological incident is the rapid identification of the hazard and immediate control over all responding units.
Rapid techniques commonly used for species identification consist of species-precise primer pairs and probes, randomly amplified polymorphic DNA (RAPD), amplified fragment period polymorphisms (AFLP), restriction fragment length polymorphisms (RFLP), and karyotyping.
Elements favoring fast identity kits are reduced time in getting ready, inoculating, incubating, and cleaning up; also a convenience, decreased area for trying out and garage, ease of operation, and saving of cloth and cash are many motives for the food industry to use rapid identification structures for ordinary.
A urine lifestyle test can discover micro organism or yeast causing urinary tract contamination (UTI). If microorganisms multiply, an antibiotic sensitivity take look at can discover the antibiotic most in all likelihood to kill those specific bacteria. Your healthcare issuer may additionally order a urine tradition if you get persistent or difficult-to-deal with UTIs.
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Complete each row of the table below by filling in the missing prefix or missing exponent.
The given question is based on the concept of conversion factor
1 KL = 10³ L, 1cL = 10⁻³ L, 1dL = 10⁻² L, 1 nL = 10⁻⁹ L
What is Conversion factor ?A conversion factor is an expression for the relationship between units that is used to change the units of a measured quantity without changing the value.
A conversion ratio (or unit factor) always equals one (1), where the numerator and the denominator have the same value expressed in different units.
Hence, The complete filled table is given as follows ;
1 KL = 10³ L,
1cL = 10⁻³ L,
1dL = 10⁻² L,
1 nL = 10⁻⁹ L
Where,
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Identify the reactant, reagent, and solvent to synthesize the Grignard reagent. An unknown reactant is treated with an unknown reagent in an unknown solvent to give a grignard reagent. The product is a carbon bonded to two methyls, a hydrogen and magnesium chloride. The best reactant is: The best reagent is: The best solvent is:
The best reactant is: iPrCl
The best reagent is: Mg
The best solvent is: CH3CH2OCH2CH3
Grignard reagent or Grignard compoundA chemical molecule with the general formula RMgX, where X is a halogen and R is typically an alkyl or aryl group, is known as a Grignard reagent or Grignard compound. Methylmagnesium chloride (ClMgCH3) and phenylmagnesium bromide (C6H5)-Mg-Br, respectively, are two prominent examples. They fall within the category of organomagnesium compounds.
Why does the Grignard reagent include mg?Typically, magnesium ribbon is needed for the reaction that results in the synthesis of Grignard reagents. A magnesium oxide passivating coating protects the whole magnesium, preventing interactions with organic halides. As an initiator, Grignard's prepared reagent can also be applied.
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Determine physiological temperature, 98.6 F in degree C
Answer:
37
Explanation:
( 98.6 - 32 ) × 5(100c) ÷ 9(180f) = 37
How many individual oxygen atoms are contained in a sample of P2O5 that also
contains 0.620 moles of P? (Input your answer with scientific notation using "e-
notation and report your answer to two places past the decimal point. Moodle is
looking for a number only, no units.)
Answer:
Explanation:
Equation with given
P2O5 ====> 2P^5 + 5O-2
0.620 x
Solution
What you are going to do first is find the molar amount of oxygen. Use a proportion to do this
2/0.620 = 5/x Cross Multiply
2x = 0.620 * 5 Divide both sides by 2
2x/2 = 0.620 *5/2
x = 0.310 * 5 Combine
x = 1.55 moles of oxygen.
Now comes the answer. How many atoms are there in 1.55 moles of oxygen?
1 mole of anything contains 6.02 * 10^23 items of that mole
1.55 moles of oxygen contains x atoms of oxygen
1/1.55 = 6.02 * 10^23 / x Cross multiply
1*x = 1.55 * 6.02*10^23 Combine
x = 9.331 e 23
Answer
9.33e23
PLEASE HELP ASAP!! How many grams of AgNO3 would react with 24 grams of Mg?
Answer: [tex]340gAgNO_{3}[/tex].
Explanation:
You will need to create a stoichiometric equation with the information given. The formula is in the problem and so are the molar masses. I will add and plug in the data for you below.
[tex]24gMg*\frac{1molMg}{24gMg} *\frac{2molAgNO_{3} }{1molMg} *\frac{170gAgNO_{3}}{1molAgNO_{3}} =340gAgNO_{3}[/tex]
I plugged the numbers into my scientific calculator, which is how I got the answer. I also added the letters in the formula above because you have to be able to cancel them out so you can find your missing data.
Therefore, [tex]340gAgNO_{3}[/tex] would react with 24gMg.
I hope this helps! Pls give brainliest!! :)
[tex]340g AgNO_3[/tex] would react with 24 grams of Mg.
What are moles?A mole is defined as 6.02214076 × [tex]10^{23}[/tex] of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.
Create a stoichiometric equation with the information given.
[tex]24g Mg X \frac{1 mol of Mg}{24g Mg} X \frac{2 mol of AgNO_3}{1 mol of Mg} X \frac{170g AgNO_3 }{1 mol AgNO_3} = 340g AgNO_3[/tex]
[tex]340g AgNO_3[/tex]
Hence, [tex]340g AgNO_3[/tex] would react with 24 grams of Mg.
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Calculate the work (KJ) done during a reaction in which the internal volume contracts from 83 L to 13 L against an outside pressure of 4.4 atm.
-31.2 kJ is the work done during a reaction in which the internal volume contracts from 83 L to 13 L against an outside pressure of 4.4 atm.
How to calculate the work done on or by a gas ?It is represented by the equation
W = PΔV
where,
W = Work done
P = Pressure
ΔV = Change in volume (V₂ - V₁)
Now put the values in above formula we get
W = PΔV
= 4.4 atm × (13 L - 83 L)
= 4.4 atm × (-70 L)
= -308 atm L
Now change L atm into J
= -308 × 101.3 J [L × atm = 101.3 J]
= -31200.4 J
= -31200.4 × 10⁻³ kJ
= -31.2 kJ
Thus from the above conclusion we can say that -31.2 kJ is the work done during a reaction in which the internal volume contracts from 83 L to 13 L against an outside pressure of 4.4 atm.
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7. If you start with 3.20 mol of Li3N and 9.0 mol water, how many moles of NH3 will be formed?
Li3N + 3H2O ----> NH3 + 3LiOH
Taking into account the reaction stoichiometry, 3 moles of NH₃ will be formed.
Reaction stoichiometryIn first place, the balanced reaction is:
Li₃N + 3 H₂O → NH₃ + 3 LiOH
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:
Li₃N: 1 moleH₂O: 3 molesNH₃: 1 mole LiOH: 3 molesLimiting 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 Li₃N reacts with 3 moles of H₂O, 3.20 moles of Li₃N reacts with how many moles of H₂O?
[tex]moles of H_{2} O=\frac{3.2 moles of Li_{3}Nx 3 moles of H_{2} O}{1 mole of Li_{3}N}[/tex]
moles of H₂O= 9.6 moles
But 9.6 moles of H₂O are not available, 9 moles are available. Since you have less moles than you need to react with 3.20 moles of Li₃N, H₂O will be the limiting reagent.
Mass of NH₃ formedConsidering the limiting reagent, the following rule of three can be applied: if by reaction stoichiometry 3 moles of H₂O form 1 mole of NH₃, 9 moles of H₂O form how many moles of NH₃?
[tex]molesof NH_{3} =\frac{9 moles H_{2} Ox1 mole of NH_{3}}{3 moles H_{2} O}[/tex]
moles of NH₃= 3 moles
Finally, 3 moles of NH₃ will be formed.
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0.546 g sample of pure oxalic acid (H2C2O4) crystals is dissolved in water and titrated with 22.40 mL of a potassium hydroxide solution. What is the molarity of the KOH(aq)
The molarity of KOH is 0.2678 moles/L.
What is the molarity(M)?The number of moles of solute per liter of solution is known as Molarity.The formula to find the molarity is;
Molarity(M) = number of moles/ volume of solutions in liter.
Define mole?The amount of a substance that contains exactly [tex]6.02214076\times10^{23}[/tex]elementary entities of the given substance can be defined as a mole.The formula to find the number of moles of a substance is;Number of moles(n) = mass of the substance/Molar mass
The mass of Oxalic acid is 0.546g.
The molar mass of Oxalic acid [tex]H_{2}C_{2}O_{4}[/tex] is 90g (1*2+12*2+16*4=90)
The number of moles of Oxalic acid is,
n = 0.546/90
n = 0.006 moles
So, the number of moles of Oxalic acid is 0.006 moles.
The volume of KOH is 22.40mL = 22.40*1000 = 0.0224L
Therefore the molarity of KOH is,
M = number of moles/ volume of solutions in liter
M = 0.006/0.0224
M = 0.2678 moles/L
Therefore, the molarity of KOH is 0.2678 moles/L
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4. An industrial gas storage tank with adjustable pressure has volume of 100.0 L when the
gas temperature is 55.0°C. Calculate the temperature of the gas if the volume drops to
75.0 L with no loss in pressure.
Taking into account the Charles' law, the temperature of the gas if the volume drops to 75.0 L is 246 K or -27 C.
Charles' lawCharles' law establishes the relationship between the temperature and the volume of a gas when the pressure is constant. This law says that for a given sum of gas at constant pressure, as the temperature increases, the volume of the gas increases and as the temperature decreases, the volume of the gas decreases. That is, the volume is directly proportional to the temperature of the gas.
Mathematically, Charles' law is a law that says that when the amount of gas and pressure remain constant, the ratio between volume and temperature will always have the same value:
[tex]\frac{V}{T}=k[/tex]
Considering an initial state 1 and a final state 2, it is fulfilled:
[tex]\frac{V1}{T1}=\frac{V2}{T2}[/tex]
Final temperatureIn this case, you know:
V1= 100 LT1= 55 C= 328 K (being 0 C= 273 K)V2= 75 LT2= ?Replacing in Charles's law:
[tex]\frac{100 L}{328 K}=\frac{75 L}{T2}[/tex]
Solving:
[tex]T2x\frac{100 L}{328 K}=75 L[/tex]
[tex]T2=\frac{75 L}{\frac{100 L}{328 K}}[/tex]
T2= 246 K= -27 C
Finally, the temperature of the gas if the volume drops to 75.0 L is 246 K or -27 C.
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Give three examples of environmental, industrial and bio-chemistry.
Three examples of environmental, industrial and bio-chemistry are listed below:
Environmental chemistry: Contamination, Atmospheric Deposition, and Soil Pollution.industrial chemistry: industrial inorganic chemicals, industrial organic chemicals, and agricultural chemicalsbio-chemistry: genetic, immunology, and enzymologyMeaning of ChemistryChemistry can be defined as a branch of science which is concerned with the substances matter is composed of, their properties and reactions,
Chemistry also deals with the use of such reactions to form new substances.
In conclusion, Three examples of environmental, industrial and bio-chemistry are listed anove
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