The oxygen atom has a partial negative charge and the Hydrogen atoms have a partial positive charge
The O2 atoms have a covalent bonding and are attracted to the electrons more strongly.
The sharing of the electrons gives them water molecules a slightly negative change near the O2 atom. A slight positive change near the H2. Hence the option D is correct.Learn more about the did your answer includes.
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During which stage of the cell cycle dies the cell condense chromosomes and break down the nuclear envelope
Answer:
Prophase
Explanation:
During prophase, the chromosomes condense, the nucleolus disappears, and the nuclear envelope breaks down.
Answer: It should be Prophase I am 100% sure
Because HCl is a strong acid and NaOH is a strong base, the equivalence point of the neutralization reaction occurs at pH ____.
ANSWER: 7
Answer:
yes, 7 is the correct answer.
Answer: 7
Explanation: Just did it.
Describe the two processes of the carbon cycle
The two processes of carbon cycle are rapid carbon exchange and the long-term cycling of carbon.
What are the two process of carbon cycle?The carbon cycle consists of two interconnected processes: rapid carbon exchange among living organisms and the long-term cycling of carbon through geologic processes.
In the first process, photosynthesis consumes carbon dioxide and produces oxygen, while aerobic respiration consumes oxygen and produces carbon dioxide. These two processes play an important role in the carbon cycle.
In the second process, carbon is stored for long periods in carbon reservoirs such as the atmosphere, bodies of liquid water, ocean sediment, soil, land sediments, and the Earth's interior.
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Ammonia and copper(II) oxide react to form solid copper, water and nitrogen gas. What are the coefficients for the balanced chemical equations.
A: 2,2,2,1,1
B: 1,2,1,2,1
C: 1,3,3,3,1
Answer:
a
Explanation:
Answer:
i am also positive it is A
Explanation:
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one mole of an ideal gas
occupies a volume of 22.4
liters at
Answer : One mole of an ideal gas occupies a volume of 22.4 liters at STP.
Explanation :
As we know that 1 mole of substance occupies 22.4 liter volume of gas at STP conditions.
STP stands for standard temperature and pressure condition.
At STP, pressure is 1 atm and temperature is 273 K.
By using STP conditions, we get the volume of 22.47 liter.
Hnece, the one mole of an ideal gas occupies a volume of 22.4 liters at STP.
When 100.g Mg3N2 reacts with 75.0 g H2O, what is the maximum theoretical yield of NH3?
Mg3N2(s) + 6H2O (l) → 3Mg(OH)2(aq) + 2NH3(g)
Answer choices:
1280 g
70.8 g
213 g
23.6 g
25.0 g
Answer : The correct option is, 23.6 g
Explanation : Given,
Mass of [tex]Mg_3N_2[/tex] = 100.0 g
Mass of [tex]H_2O[/tex] = 75.0 g
Molar mass of [tex]Mg_3N_2[/tex] = 101 g/mol
Molar mass of [tex]H_2O[/tex] = 18 g/mol
First we have to calculate the moles of [tex]Mg_3N_2[/tex] and [tex]H_2O[/tex].
[tex]\text{Moles of }Mg_3N_2=\frac{\text{Given mass }Mg_3N_2}{\text{Molar mass }Mg_3N_2}[/tex]
[tex]\text{Moles of }Mg_3N_2=\frac{100.0g}{101g/mol}=0.990mol[/tex]
and,
[tex]\text{Moles of }H_2O=\frac{\text{Given mass }H_2O}{\text{Molar mass }H_2O}[/tex]
[tex]\text{Moles of }H_2O=\frac{75.0g}{18g/mol}=4.17mol[/tex]
Now we have to calculate the limiting and excess reagent.
The balanced chemical equation is:
[tex]Mg_3N_2(s)+6H_2O(l)\rightarrow 3Mg(OH)_2(aq)+2NH_3(g)[/tex]
From the balanced reaction we conclude that
As, 6 moles of [tex]H_2O[/tex] react with 1 mole of [tex]Mg_3N_2[/tex]
So, 4.17 moles of [tex]H_2O[/tex] react with [tex]\frac{4.17}{6}=0.695[/tex] moles of [tex]Mg_3N_2[/tex]
From this we conclude that, [tex]Mg_3N_2[/tex] is an excess reagent because the given moles are greater than the required moles and [tex]H_2O[/tex] is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of [tex]NH_3[/tex]
From the reaction, we conclude that
As, 6 moles of [tex]H_2O[/tex] react to give 2 moles of [tex]NH_3[/tex]
So, 4.17 moles of [tex]H_2O[/tex] react to give [tex]\frac{2}{6}\times 4.17=1.39[/tex] mole of [tex]NH_3[/tex]
Now we have to calculate the mass of [tex]NH_3[/tex]
[tex]\text{ Mass of }NH_3=\text{ Moles of }NH_3\times \text{ Molar mass of }NH_3[/tex]
Molar mass of [tex]NH_3[/tex] = 17 g/mole
[tex]\text{ Mass of }NH_3=(1.39moles)\times (17g/mole)=23.6g[/tex]
Therefore, the maximum theoretical yield of [tex]NH_3[/tex] is, 23.6 grams.
The maximum theoretical yield of NH3 when 100.g Mg3N2 reacts with 75.0 g H2O is 23.6 g, as H2O is the limiting reactant.
Explanation:To determine the maximum theoretical yield of NH3, start by calculating the number of moles for both reactants. The molar mass of Mg3N2 is 100.93 g/mol, so you have 100 g / 100.93 g/mol = 0.991 moles of Mg3N2. The molar mass of H2O is 18.02 g/mol, so you have 75 g / 18.02 g/mol = 4.16 moles of H2O.
According to the stoichiometry of the reaction, Mg3N2 reacts with 6H2O to produce 2NH3. Thus, the moles of H2O is not enough to react with all the moles of Mg3N2, making H2O the limiting reactant. This means that the reaction will stop once all the H2O is consumed.
From the reaction stoichiometry, 6 moles of H2O produce 2 moles of NH3. So, 4.16 moles of H2O will produce (2/6)*4.16 = 1.39 moles of NH3. The molar mass of NH3 is 17.03 g/mol, so the maximum theoretical yield of NH3 is 1.39 moles * 17.03 g/mol = 23.6 g.
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Which color of the visible spectrum has the shortest wavelength?
1violet
2blue
3yellow
4red
Answer:
violet
Explanation:
Violet has the shortest wavelength at 380 nanometers
The correct option is 1 i.e, Violet light has the shortest wavelength in the visible spectrum at approximately 380-450 nm and carries the most energy. Red light has the longest wavelength, about 620-750 nm, and the least energy.
The visible light spectrum consists of a range of colors that our eyes perceive as different wavelengths. Of these colors, violet light has the shortest wavelength, approximately 380-450 nanometers (nm). Because it has the shortest wavelength, violet light also carries the most energy. On the other end of the spectrum, red light has the longest wavelength, about 620-750 nm, and thus carries the least energy. To remember the order of colors from longest to shortest wavelength, you can use the mnemonic ROY G BIV, which stands for Red, Orange, Yellow, Green, Blue, Indigo, and Violet.
My car has a volume of 2600. L. On a nice spring day, the temperature outside is 20.0 degrees Celsius. If the pressure is 98.5 kPa, how many moles of gas are inside the car?
Answer : The number of moles of gas inside the car is, 105.0 mole.
Explanation :
To calculate the moles of gas we are using ideal gas equation.
[tex]PV=nRT[/tex]
where,
P = Pressure of gas = 98.5 kPa = 0.972 atm (1 atm = 101.3 kPa)
V = Volume of gas = 2600 L
n = number of moles of gas = ?
R = Gas constant = [tex]0.0821L.atm/mol.K[/tex]
T = Temperature of gas = [tex]20^oC=273+20=293K[/tex]
Now put all the given values in above equation, we get:
[tex]0.972atm\times 2600L=n\times (0.0821L.atm/mol.K)\times 293K[/tex]
[tex]n=105.0mol[/tex]
Therefore, the number of moles of gas inside the car is, 105.0 mole.
How any moles of H2O will be produced from 12.3 moles of HCL reacting with Ca(OH)2?
Answer:
\large \boxed{\text{12.3 mol HCl}}
Explanation:
We need a balanced chemical equation with moles.
2HCl +Ca(OH)₂ ⟶ CaCl₂ + 2H₂O
n/mol: 12.3
The molar ratio is 2 mol H₂O:2 mol HCl.
[tex]\text{Moles of H$_{2}$O} = \text{12.3 mol HCl} \times \dfrac{\text{2 mol H$_{2}$O}}{\text{2 mol HCl}} = \textbf{12.3 mol HCl}\\\\\text{The reaction produces $\large \boxed{\textbf{12.3 mol HCl}}$}[/tex]
Assuming a stoichiometric relationship where 2 moles of HCl react with 1 mole of Ca(OH)₂ to produce 2 moles of H₂O, 12.3 moles of HCl would theoretically produce 12.3 moles of H₂O.
The question is about determining how many moles of H₂O will be produced from 12.3 moles of HCl reacting with Ca(OH)₂. To solve this, it's essential to know the chemical reaction involved. Unfortunately, the reaction between HCl and Ca(OH)₂, which typically forms CaCl₂ and H₂O, is not provided in full detail in the question. However, knowing that HCl reacts with base like Ca(OH)₂ to produce water and a salt, and typically in stoichiometric reactions involving a strong acid like HCl and a strong base like Ca(OH)₂, the ratio often is 2 moles of HCl react with 1 mole of Ca(OH)₂ to produce 2 moles of water (as a simplified approximation). While an exact reaction equation is necessary for a precise answer, if we assume the reaction follows a simple stoichiometry of 2HCl + Ca(OH)₂ → 2H₂O + CaCl₂, then for every 2 moles of HCl, 2 moles of H₂O are produced. Therefore, if 12.3 moles of HCl react completely with an adequate amount of Ca(OH)₂, they would produce 12.3 moles of H₂O, assuming the reaction goes to completion and all the HCl is used.
Calculate the number of moles of sodium chloride (NaCl) formed if 0.345
moles of calcium chloride (CaCl2) react.
1 Na2CO3 (aq) + 1 CaCl2 (aq) – 1 CaCO3 (s) + 2 NaCl (aq)
= ________ Moles ?
Answer : The number of moles of [tex]NaCl[/tex] formed are, 0.69 moles.
Explanation : Given,
Moles of [tex]CaCl_2[/tex] = 0.345 mol
Now we have to calculate the moles of [tex]NaCl[/tex]
The balanced chemical equation is:
[tex]1Na_2CO_2(aq)+1CaCl_2(aq)\rightarrow 1CaCO_3(s)+2NaCl(aq)[/tex]
From the balanced reaction, we conclude that
As, 1 mole of [tex]CaCl_2[/tex] react to give 2 moles of [tex]NaCl[/tex]
So, 0.345 mole of [tex]CaCl_2[/tex] react to give [tex]2\times 0.345=0.69[/tex] mole of [tex]NaCl[/tex]
Therefore, the number of moles of [tex]NaCl[/tex] formed are, 0.69 moles.
1 Na₂CO₃(aq) + 1 CaCl₂(aq) → 1 CaCO₃(s) + 2 NaCl(aq) = 0.690 moles.
If 0.345 moles of calcium chloride (CaCl₂) react, it will produce 0.690 moles of sodium chloride (NaCl) based on the balanced chemical equation provided.
This is derived from the 1:2 molar ratio between CaCl₂ and NaCl.To calculate the number of moles of sodium chloride (NaCl) formed from the reaction between calcium chloride (CaCl₂) and sodium carbonate (Na₂CO₃)we can use the balanced chemical equation: 1 Na₂CO₃(aq) + 1 CaCl₂(aq) → 1 CaCO₃(s) + 2 NaCl(aq)We start with the given number of moles of CaCl₂: 0.345 moles.From the balanced equation, we see that 1 mole of CaCl₂ produces 2 moles of NaCl.Therefore, if we have 0.345 moles of CaCl₂, we multiply by 2 to find the moles of NaCl:0.345 moles CaCl₂ × 2 moles NaCl / 1 mole CaCl₂ = 0.690 moles NaCl
So, 0.345 moles of calcium chloride will produce 0.690 moles of sodium chloride.
Correct question is: Calculate the number of moles of sodium chloride (NaCl) formed if 0.345 moles of calcium chloride (CaCl2) react.
1 Na2CO3 (aq) + 1 CaCl2 (aq) – 1 CaCO3 (s) + 2 NaCl (aq) = ________ Moles ?
Hydrogen peroxide also called
Answer:
dihydrogen dioxide, hydrogen dioxide, hydrogen oxide, oxydol, peroxide, H2O
what is an energy sublevel
Answer:
A sublevel is an energy level defined by quantum theory.
Explanation:
In chemistry, sublevels refer to energies associated with electrons. In physics, sublevels may also refer to energies associated with the nucleus.
Answer:e
The level of energy possessed by all of the electrons in one type of orbital.
Explanation:
I took the test.
Prove to me that 0.85% NaCl (basic solution of an IV) is isosmotic. That is, that it is approximately 300 mosmo/L in concentration. You must show ALL your work, cancelling out all units. You must show units on each step. As a starter, the above concentration is equal to 0.85g Nacl/ 100 ml.
Answer:
the osmolarity of the 0.85% NaCl solution is approximately equal to 300 mosmol/L.
Explanation:
Molarity= number of moles/volume of the solution in liters
volume of the solution= 100 mL
1 L= 1000 mL
100 mL= 100/1000=0.1 L
molar mass of NaCl= 58.44 g/mol
number of moles= mass in gram/gram molecular mass
= 0.85/58.44
= 0.01455
molarity= number of moles/volume of the solution in liters
= 0.01455 / 0.1
= 0.1455 M
1 M= 1000 mM
so 0.1455 M = 0.1455 × 1000
= 145.5 mM
Osmolarity is the concentration of solutes in the solution.
NaCl dissociates to Na+ and Cl-
so osmolarity of 145.5 mM NaCl= 2 × 145.5
= 291 mosmol/L
Therefore, we conclude that the osmolarity of the 0.85% NaCl solution is approximately equal to 300 mosmol/L.
How many moles of lead, Pb, are in 1.50 x 1012 atoms of lead?
Answer:
2.49*10⁻¹² mol
Explanation:
Use Avogadro's Number for this equation (6.022*10²³). Divide Avogrado's by the number of atoms you have to find moles. You are answer should be 2.49*10⁻¹² mol.
Answer:
2.49*10⁻¹² mol
Explanation:
Use Avogadro's Number for this equation (6.022*10²³). Divide Avogrado's by the number of atoms you have to find moles. You are answer should be 2.49*10⁻¹² mol.
Plz let me know if it is correct.
At what temperature will 41.6 grams N, exert a pressure of 815 mmHg in a
20.0L cylinder?
Hint: You must convert 41.6 g into moles FIRST, then use Ideal gas law to solve
for temperature.
134K
O 238 K
O 337 K.
O 176K
None of the given options are correct, and the correct answer is 174 K.
Explanation:
Mass of N = 41.6 g
Moles = [tex]$\frac{given mass}{molar mass}[/tex]
= [tex]$\frac{41.6 g}{28 g/ mol}[/tex] = 1.5 moles
Pressure, P = 815 mm Hg = 1.07 atm
Volume, V = 20 L
R = gas constant = 0.08205 L atm mol⁻¹ K⁻¹
Temperature, T = ? K
We have to use the ideal gas equation,
PV = nRT
by rearranging the equation, so that the equation becomes,
T = [tex]$\frac{PV}{nR}[/tex]
Plugin the above values, we will get,
T = [tex]$\frac{1.07 \times 20}{1.5 \times 0.08205}[/tex]
= 174 K
So the temperature of the nitrogen gas is 174 K.
Final answer:
The temperature at which 41.6 grams of nitrogen exert a pressure of 815 mmHg in a 20.0L cylinder is calculated using the ideal gas law and is approximately 177 Kelvin.
Explanation:
To find the temperature at which 41.6 grams of nitrogen (N₂) will exert a pressure of 815 mmHg in a 20.0L cylinder, we need to use the ideal gas law, which is PV = nRT.
First, we convert the mass of nitrogen to moles. The molar mass of N₂ is 28.02 g/mol, so:
moles of N₂ = 41.6 g ÷ 28.02 g/mol = 1.484 moles of N₂
Using the ideal gas law:
R = 62.36 L mmHg / (mol·K)
We have:
PV = nRT
(815 mmHg)(20.0 L) = (1.484 mol)(62.36 L mmHg / mol·K)T
T = (815 mmHg × 20.0 L) / (1.484 mol × 62.36 L mmHg / mol·K)
T = 16370 mmHg·L / (92.48104 mol·L mmHg / mol·K)
T = 177 K (rounded to 3 significant figures)
The temperature at which 41.6 grams of nitrogen will exert a pressure of 815 mmHg in a 20.0L cylinder is approximately 177 Kelvin.
Ammonium hydroxide is a weak base according to the Arrhenius definition. This means that ammonium hydroxide-
A.receives most of its H+ in solution.
B.gives up some of its Ht in solution.
C.receives most of its OH in solution.
D.gives up some of its OH in solution.
Answer:
D
Explanation:
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Ammonium hydroxide, a weak base, according to the Arrhenius definition, gives up some of its OH- ions in solution.
Explanation:Ammonium hydroxide is considered a weak base according to the Arrhenius definition beacause it dissociates in water to some extent and produces hydroxide ions (OH-). So, the correct choice in this case is (D) 'gives up some of its OH in solution'. It doesn't receive most of its H+ in solution, which makes options A and B incorrect, and it does not receive most of its OH- ions instead it donates them in the solution, making option C incorrect as well.
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What do acid compounds contain? molecules ions hydrogen oxygen
Answer:
most acids contain something called hydrogen atoms
Explanation:
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What is the pH when the poH value is 2?
Answer:
i hate my life PERIODT
Explanation:
WHY AM I HERE :/
Identify the 2 numbers given for each element
Each element in the periodic table has two numbers. The first is the atomic number that represents the number of protons in the nucleus. The second is the atomic weight that accounts for the average mass of the isotopes of the element.
Explanation:In the periodic table, each element is represented with two numbers. The larger number, usually found on top, is the atomic number, which signifies the number of protons present in the nucleus of the atom. The second number is the atomic weight or atomic mass, which is usually found at the bottom of the element symbol. It represents the average mass of the isotopes of that element, considering their abundance. For instance, for Carbon (C), the atomic number is 6 (protons) and the atomic weight is about 12.01 (protons + neutrons).
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how to make a milkshake?
Answer:
Strawberry? Peppermint fudge? Bananarama? Any flavor you like! Learn how to make milkshakes from scratch with our step-by-step guide (plus pretty pictures).
Milkshakes are one of the most iconic American desserts. They’re refreshingly cool, slurp-ably sweet and come in pretty much any flavor you can imagine. But you don’t need to belly up to a vinyl booth to enjoy one. Making a milkshake from scratch is simple. If you’ve got a tub of ice cream on hand, you’re halfway there. Follow along as our test kitchen shows how to make the most flavorful milkshake.
In the mood for more classic sweets? These vintage dessert recipes are making a comeback.
How to Make the Best Milkshake Ever
Ingredients
1/3 cup milk.
You can use 2%, whole milk, or a blend of milk and half-and-half.
1-1/2 cups ice cream
Vanilla makes a good base for most shakes, or you can use a flavor like chocolate.
Delicious mix-ins!
Think a swirl of chocolate syrup, peanut butter, a chopped banana or other fruit, a handful of chocolate or butterscotch chips (we could go on and on…)
A blender, of course.
You can use a classic stand blender-or an immersion blender if you want to make it right in your glass.
Instructions
Step 1: Add the Milk, Ice Cream and Mix-Ins
Learn how to make a milkshake
TASTE OF HOME
Send your ingredients straight to the blender. For best results, put in your milk first. That will get the blender mixing quickly. Be sure to let your ice cream soften before scooping. If it’s too hard, you might end up having to add more milk, which thins the shake.
Test Kitchen tip: For an ultra-rich shake, use whole milk or milk with a little half-and-half cream. But never use heavy cream. If you send that through the blender, it’ll create little bits of butter.
We’re going to make a strawberry shake, so we’ll add 1/2 cup frozen unsweetened strawberries and 1 tablespoon strawberry preserves.
Editor’s tip: Remember that any ingredients you add will soon be pulverized in the blender. If you want to keep the size and shape of mix-ins like sprinkles, cherries or chocolate chips, it’s best to reserve as a garnish.
Step 2: Blend ’til smooth
Ice cream, milk and strawberries in a blender
It’s time to blend away. You’ll want to keep an eye on the consistency. This recipe creates a Goldilocks-style shake: not too firm and not too soft (runny). Of course, you can always customize it either way. Use less milk for a thicker, spoonable shake; more for a thinner, sippable one.
Be sure to check our our Test Kitchen’s recommendation for the best blender for your milkshake.
Step 3: Pour and Enjoy!
Strawberry milkshake in a glass with a green striped straw sticking out
Pour your milkshake into a chilled glass to serve. It tastes great straight-up or topped with a tower of whipped cream. Feeling fancy? Layer on toppings like chocolate syrup, sugary cereal or rainbow sprinkles. Once you’ve mastered the classic garnishes, try these crazy takes!
Answer:
Explanation:
4 large scoops of whatever flavor icecream you want
1/4 cup of milk
in the blender blend all together
pour into a glass
add whip cream sprinkles and a cherry
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2 Points
Which of the following is described by the equation H2O(l) + heat → H2O(g)?
Consider this reaction:
Which is the base in this reaction?
What is the total charge of an ionic compound
Answer:
Zero
Explanation:a ionic compound consists of an equal number or positive and negative ions
Which of the following might not have DNA in double-helix form?
A)A human
B)A bacterium
C)A bird
D)A tree
Answer:
B
Explanation:
Answer:
D.A tree
Explanation:
What is the ability to do work defined as?
pressure
energy
force
temperature
Answer:
Your answer is Energy
How many moles of H2SO4 do you have if there are 1.64x10^22 molecules of H2SO4
0.027 moles of [tex]H_{2} S_{} 0_{4}[/tex] if there are 1.64x[tex]10^{22}[/tex] molecules of [tex]H_{2} S_{} O_{4}[/tex]
Explanation:
Data given:
number of molecules of [tex]H_{2} S_{} 0_{4}[/tex] = 1.64 X [tex]10^{22}[/tex]
Atomic weight of the sulphuric acid = 98.07 grams/mole
We know that 1 mole of sulphuric acid has 6.022 x [tex]10^{23}[/tex] (Avagadro number) molecules.
so number of moles present in 1.64 X [tex]10^{22}[/tex] molecules is given by:
so to get moles we will use
number of moles = [tex]\frac{number of molecules given}{avagadro number}[/tex]
number of moles = [tex]\frac{1.64 X 10^{22} }{6.022 X 10^{23} }[/tex]
number of moles = 0.027 moles
So, 1.64 X [tex]10^{22}[/tex] molecules will be there in 0.027 moles of sulphuric acid.
A student weighed 0.2440 grams of sample of a recently synthesized cobalt amine bromide compound. After dissolving in 120mL of acidified water, she added 2.55 grams of AgNO3 to precipitate any free Br-. The precipitate was found to weigh 0.3700 grams. Calculate the %Br- in the sample. MW Cl- 35.45 g/mol; MW Br- 79.91 g/mol; MW Ag 107.87 g/mol
The bromine percentage is 49.42 %
Explanation:
Mass of AgBr precipitated = 0.31 g
Molecular weight of AgBr = 187.77 g mol - 1
moles of AgBr = 0.31 g by 187.77 g mol - 1 = 0.0016509 moles
moles of Br ion = 0.0016509 moles
Mass of Br ion = 0.0016509 moles into 79.904 g mol - 1 = 0.1319 g
The Total mass of compound = 0.2669 g
Percentage of bromine = 0.1319 by 0.2669 = 49.42 percent
Hence the bromine percentage is 49.42 %
Kinetic molecular theory explains changes in _ ?
A) states of matter
B) polarity
C) electronegativity
D) potential energy
Answer:
A) States of matter
Explanation:
Hope this answer helps you
Final answer:
The kinetic molecular theory explains changes in states of matter, as it relates to the balance between particle motion (kinetic energy) and intermolecular forces influenced by temperature and pressure. Correct option is A.
Explanation:
The kinetic molecular theory explains changes in states of matter. It posits that matter is composed of tiny particles that are always in motion. The balance between the kinetic energy, which is related to the particle motion, and the intermolecular forces, which are attractive forces between particles, determines a substance's state. Temperature changes can alter the kinetic energy of particles, leading to state changes. Similarly, increasing pressure compacts molecules closer together, enhancing the intermolecular forces, and potentially causing a phase change.
What pressure will be exerted by 0.60 mol of CO2 when its temperature is 25 OC and it is in a 500 mL container?
Answer:
29.3 atm
Explanation:
We need to use the Ideal Gas Law to solve this problem: PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, and T is the temperature in Kelvin.
Here, volume is V = 500 mL = 0.500 L; moles is n = 0.60 mol; R is 0.08206 atm/(mol * K); and temperature is T = 25 + 273 = 298 K. Plug these into the equation to solve for P:
P * (0.500 L) = (0.60 mol) * (0.08206 atm/mol * K) * (298 K)
P ≈ 29.3 atm
Hope this helps!
What is one limitation of descriptive investigations?
They cannot show cause and effect.
They produce lots of data.
They can be done at a lower cost.
They follow procedures.
Answer:the answer is A. They cannot show cause and effect
Answer:
A
Explanation: I just did this on edgenuiity and got it right