According to the ideal gas law, a gas's pressure is inversely related to its volume and directly proportionate to its temperature. So, if a gas sample's volume is reduced, the gas sample's pressure must also increase.
As a result, in order to determine the pressure of the gas sample under the specified circumstances, we must first determine the ratio of the two volumes before multiplying the starting pressure of the sample by that ratio.
We may get the ratio of the two volumes using the ideal gas law as follows: V2/V1 = (100.0 mL/0.75 L) x (273 K/25oC) = 8.02 As a result, the gas sample's pressure at 25 oC with a volume of 100.0 mL is 8.02 times higher than the sample's original pressure.
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Which
thermochemical
equation
corresponds to
the graph?
Answer: C
Explanation:
Answer: C
Explanation:
help!!!!!!!!!!!!!!!!!!!!!!!!
Answer:
two
Explanation:
the answer is two
option b
what is the most basic level of organization that can perform functions like converting food into energy
Answer: Cells
Explanation:
A zinc chloride solution is prepared by dissolving 0.316 g of anhydrous zinc chloride in 100.0 mL of H2O.
What mass of zinc chloride is present in 19.97 mL of that solution.
A zinc chloride solution is prepared by dissolving 0.316 g of anhydrous zinc chloride in 100.0 mL of [tex]H_2O[/tex] . The mass of zinc chloride present in 19.97 mL of the solution is 0.316 g.
We can use the formula:
C1V1 = C2V2
where C1 is the concentration of the original solution, V1 is the volume of the original solution, C2 is the concentration of the final solution, and V2 is the volume of the final solution.
First, let's calculate the concentration of the original solution:
concentration = (0.316 g) / (100.0 mL) = 0.00316 g/mL
Now, we can use the formula to find the mass of zinc chloride in 19.97 mL of the solution:
C1V1 = C2V2
0.00316 g/mL x 100.0 mL = C2 x 19.97 mL
C2 = (0.00316 g/mL x 100.0 mL) / 19.97 mL
C2 = 0.01583 g/mL
So the concentration of zinc chloride in the final solution is 0.01583 g/mL.
Now we can use this concentration to calculate the mass of zinc chloride in 19.97 mL of the solution:
mass = concentration x volume
mass = 0.01583 g/mL x 19.97 mL
mass = 0.316 g
Therefore, there are 0.316 g of zinc chloride present in 19.97 mL of the solution.
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What will happen when pressure on a reactant mixture at equilibrium and with fewer moles on the reactant side is increased
when pressure of the reactant mixture at the equilibrium and with the fewer moles in reactant side will be increased and the equilibrium will be shift to the side in the reaction where the fewer moles of the gas.
According to the Le Chartelier, when the reaction is in the equilibrium phase and the one of the constraints which will affect the rate of the reactions, and the equilibrium will be shift to the cancel out this effect that the constraint had.
Therefore, If the pressure of the system or the reaction is in the equilibrium is change, the equilibrium of the reaction will be change that is depending on the side of the reaction with the highest number of the molecules.
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Does anyone have Personal Care services on E2020
Here are some questions on Personal Care services on E2020 are:
A client with a new ileostomy has been home for four days. The HHA is giving the client a bath and notices that the pouch is full. The HHA should say to the client: D. "I'll empty the pouch for you."A client is bedridden at home and has an infected draining sacral wound. The infection control supplies that should be kept in the home is: Gloves.What is infection?An infection is the entrance and growth of dangerous microorganisms in the body that harm the host, such as bacteria, viruses, fungus, or parasites.
Infections can be systemic (affecting the entire body) or localized (affecting a particular area of the body), and they can be moderate to severe.
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draw the lewis structure of ch3br
The Lewis structure of the compound[tex]CH_{3} Br[/tex] is shown in the image attached.
What is the Lewis structure?The Lewis structure of a molecule or ion is produced by arranging the atoms in a manner that lessens the attraction between their valence electron pairs and then distributes the valence electrons among the atoms to form covalent bonds.
The octet rule, which states that atoms normally gain or lose electrons to obtain a stable configuration with eight valence electrons, frequently serves as a guidance when arranging electrons in the Lewis structure.
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Iron pyrite (FeS2) is the form in which much of
the sulfur exists in coal. In the combustion of
coal, oxygen reacts with iron pyrite to produce
iron(III) oxide and sulfur dioxide, which is a
major source of air pollution and a substantial
contributor to acid rain. What mass of Fe2O3
is produced from 74 L of oxygen at 2.97 atm
and 161◦C with an excess of iron pyrite?
Answer in units of g
The mass of Fe₂O₃ produced is 101.9 g.
How to calculate mass ?The balanced chemical equation for the combustion of iron pyrite is:
4FeS₂(s) + 11O₂(g) → 2Fe₂O3(s) + 8SO₂(g)
From the equation, 11 moles of oxygen are required to produce 2 moles of Fe₂O₃. Convert the given volume of oxygen to moles:
n(O2) = PV/RT = (2.97 atm)(74 L)/(0.0821 L·atm/mol·K)(161 + 273 K) = 3.51 mol
Since the reaction requires 11 moles of O₂ for every 2 moles of Fe₂O₃, calculate the moles of Fe₂O₃ produced:
n(Fe₂O₃) = (2/11) × n(O₂) = (2/11) × 3.51 mol = 0.638 mol
Finally, use the molar mass of Fe₂O₃ to convert moles to grams:
m(Fe₂O₃) = n(Fe₂O₃) × M(Fe₂O₃) = 0.638 mol × 159.69 g/mol = 101.9 g
Therefore, the mass of Fe₂O₃ produced is 101.9 g.
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A gas sample originally occupies 436 mL at 24 C. When the volume is expanded to 612 mL and the temperature is increased to 97 C, the pressure becomes 526 mm Hg. What was the original pressure?
Initially, there was a 266.8 mm Hg pressure.
solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas sample. The formula is:
(P1 × V1) ÷ (T1) = (P2 × V2) ÷ (T2)
where P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures.
We are given that:
- V1 = 436 mL
- V2 = 612 mL
- T1 = 24 C + 273.15 = 297.15 K (convert from Celsius to Kelvin)
- T2 = 97 C + 273.15 = 370.15 K
- P2 = 526 mm Hg
We want to find P1, the original pressure.
Plugging in the values, we get:
(P1 × 436 mL) ÷ (297.15 K) = (526 mm Hg × 612 mL) ÷ (370.15 K)
Solving for P1, we get:
P1 = (526 mm Hg × 612 mL × 297.15 K) ÷ (436 mL × 370.15 K) = 266.8 mm Hg
Therefore, the original pressure was 266.8 mm Hg.
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You want to have a barbecue this weekend! But you're worried about global warming. You only want to release a maximum of 0.750 kg of carbon dioxide from your propane grill. Using the below equation to answer the following questions.
CH3(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
ΔHrxn = -2220.1 kJ
a. How many kilojoules will you be able to release?
b. If it requires 1900 kJ to cook one hamburger, how many hamburgers can you cook?
a. We will be able to release 37,827 kJ. b. You can cook a maximum of 19 hamburgers without exceeding the limit of 0.750 kg of carbon dioxide.
a. We need to use the balanced chemical equation and the enthalpy change of the reaction.
Therefore, moles [tex]CO_2[/tex] produced are[tex]0.750 kg / 44.01 g/mol = 17.03 mol.[/tex]
The enthalpy change of the reaction is -2220.1 kJ/mol. Thus, the maximum number of kilojoules that can be released is:
[tex]\Delta Hrxn * moles of[/tex] [tex]CO_2[/tex] = [tex]-2220.1 kJ/mol * 17.03 mol = -37,827 kJ[/tex]
We need to reverse the sign of the answer, giving us 37,827 kJ.
b. If it requires 1900 kJ to cook one hamburger, we can divide the maximum number of kilojoules that can be released by the energy required to cook one hamburger:
37,827 kJ / 1900 kJ/hamburger = 19.91 hamburgers
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arrange the following electrons, represented by their quantum numbers, in increasing order of energy (lowest written first)
(1,0,0,-1/2); (3,1,1,1/2); (2,1,0,-1/2); (2,1,0,-1/2); (3,2,0,-1/2)
The electrons can be arranged in increasing order of energy as follows: (1,0,0,-1/2) < (2,1,0,-1/2) < (2,1,0,-1/2) < (3,1,1,1/2) < (3,2,0,-1/2).
The energy of an electron is determined by its principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m), and spin quantum number (s). The electrons can be arranged in increasing order of energy by comparing their quantum numbers.
Starting with the lowest energy electron, we have the electron with quantum numbers (1,0,0,-1/2). This electron has the lowest principal quantum number, indicating that it occupies the lowest energy level.
It also has an azimuthal quantum number of zero, which corresponds to the s subshell, and a negative spin quantum number, indicating that its spin is aligned opposite to the magnetic field.
Next, we have the two electrons with quantum numbers (2,1,0,-1/2). These electrons have the same principal quantum number, indicating that they occupy the same energy level.
They both have an azimuthal quantum number of one, which corresponds to the p subshell, and a negative spin quantum number.
Following these electrons, we have the electron with quantum numbers (3,1,1,1/2). This electron has a higher principal quantum number than the previous electrons, indicating that it occupies a higher energy level.
It has an azimuthal quantum number of one, which corresponds to the p subshell, and a positive spin quantum number.
Finally, we have the electron with quantum numbers (3,2,0,-1/2). This electron has the highest azimuthal quantum number of all the electrons, indicating that it occupies the d subshell. It also has a negative spin quantum number.
Therefore, the electrons can be arranged in increasing order of energy as follows: (1,0,0,-1/2) < (2,1,0,-1/2) < (2,1,0,-1/2) < (3,1,1,1/2) < (3,2,0,-1/2).
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The change in enthalpy (AH, ) for a reaction is -25.8 kJ mol.
The equilibrium constant for the reaction is 1.4 × 103 at 298 K.
What is the equilibrium constant for the reaction at 655 K?
The equilibrium constant for the reaction at 655 K is [tex]e^{6.96}[/tex] ≈ 1.05 × 10^3.
The equilibrium constant (K) for a reaction is related to the change in Gibbs free energy (ΔG) through the equation:
ΔG = -RTlnK
where R is the gas constant, T is the temperature in kelvin, and ln is the natural logarithm. Since ΔG and ΔH (the change in enthalpy) are related by the equation:
ΔG = ΔH - TΔS
where ΔS is the change in entropy, we can rearrange the first equation to get:
lnK = -ΔH ÷ RT + ΔS ÷ R
At 298 K, we can use the given values of ΔH and K to solve for ΔS:
lnK = -ΔH ÷ RT + ΔS ÷ R
ln(1.4 × 10³) = (-(-25.8 × 10³ J/mol) ÷ (8.314 J/mol K × 298 K)) + ΔS ÷ 8.314 J/mol K
ΔS = 78.2 J/mol K
Now we can use the equation above to solve for lnK at 655 K, using the same value of ΔH and the newly calculated value of ΔS:
lnK = -ΔH ÷ RT + ΔS ÷ R
lnK = -(-25.8 × 10³ J/mol) ÷ (8.314 J/mol K × 655 K) + (78.2 J/mol K) ÷ 8.314 J/mol K
lnK = 6.96
e ≈ 1.05 × 10³
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report of collage model of photosynthesis process
Photosynthesis is the process by which plants and some microorganisms convert light energy into chemical energy. It is a complex process that occurs in two stages: the light-dependent reactions and the light-independent reactions (also known as the Calvin cycle).
The light-dependent reactions (Photosynthesis)occur in the thylakoid membranes of chloroplasts and involve the absorption of light by pigments such as chlorophyll. This energy is then used to generate ATP and NADPH, which are used in the next stage of the process. The light-independent reactions occur in the stroma of chloroplasts and involve the fixation of carbon dioxide into organic molecules using the energy generated in the previous stage.
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How many grams of KOH are needed to make 185.5 ml with a concentration of 5 M?
Type your answer...
To calculate the mass of KOH needed to make a 5 M solution in 185.5 mL, we need to use the formula:
mass = moles × molar mass
where moles is the amount of KOH in moles and molar mass is the mass of one mole of KOH.
We can calculate the moles of KOH as follows:
moles = Molarity × Volume (in liters)
First, we need to convert the volume from milliliters to liters:
185.5 mL = 0.1855 L
Now we can calculate the moles of KOH:
moles = 5 M × 0.1855 L = 0.9275 moles
The molar mass of KOH is 56.11 g/mol. Therefore, the mass of KOH needed is:
mass = 0.9275 moles × 56.11 g/mol = 52.05 g
Therefore, 52.05 grams of KOH are needed to make a 5 M solution in 185.5 mL.
Question: Why is the liquid oxygen machine producing less liquid oxygen than normal?
Claim1: there is frozen water in tank 2, which is blocking some of the oxygen from coming into tank 3.
Claim2: some of the liquid oxygen evaporated in tank 3.
Claim3: some of the oxygen didn’t condense in tank 2.
The nuclear reaction entails the breakdown of an element and the subsequent release of radioactive particles. This process can occur naturally or be produced purposefully. As a result, the reaction equation is balanced. The radon element is transmuted into polonium and an alpha particle in the provided question. Since an alpha particle was emitted, the equation is balanced.
The alpha decay of radon is shown by;
222/86Rn ----> 218/84Po + 4/2He
What is the alpha decay of radon?Radon undergoes alpha decay by emitting an alpha particle, which consists of two protons and two neutrons.
Let us note that when there is an alpha decay, the parent nucleus would loose a helium nucleus and the daughter nucleus would less than than the parent in mass by four units and less than the parent in charge by 2 units and this would satisfy the mass and charge balance of the equation. The decay equation is; 222/86Rn ----> 218/84Po + 4/2He
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Missing parts;
Use the equation to complete the activity.
219 86Rn → 215 84Po + a
The nuclear equation shows the transmutation of a form of radon into polonium and an alpha particle. In one to two sentences, explain whether or not the reaction is balanced.
Pleas help!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
_______________________________
2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g)
Moles of NA = Given Mass (g) ÷ Molecular Mass (g/mol)
= 27.5 ÷ 22.9897
= 1.196 mol
Moles of H2 Produced = Mol of NA × 1 mol H2 ÷ 2 Mol NA
= 1.196 × 1 ÷ 2
= 0.60 mol
Number of Molecules = Moles × Avogadro's Number
= 0.60 × 6.023 × 10²³ mol - 1
= 3.61 × 10²³
The Number of Molecules of Hydrogen Gas Produced When Added To Water Is 3.61 × 10²³
_________________________________
6. A 90.0 gram sample of an unknown solid is heated to 80 °C and placed into a calorimeter containing 120 grams of water at 24 °C. If the final temperature of the solid sample and the water is 32 °C, what is the specific heat of solid?
PLEASE SHOW WORK
Answer:
1.02 J/g°C.
Explanation:
We can use the equation:
q = m * c * ΔT
where q is the heat absorbed or released, m is the mass of the substance (in grams), c is the specific heat, and ΔT is the change in temperature (in Celsius).
First, we can calculate the heat gained by the water:
q_water = m_water * c_water * ΔT_water
where m_water is the mass of the water (in grams), c_water is the specific heat of water (4.184 J/g°C), and ΔT_water is the change in temperature of the water.
m_water = 120 g
c_water = 4.184 J/g°C
ΔT_water = (32°C - 24°C) = 8°C
q_water = (120 g) * (4.184 J/g°C) * (8°C) = 4009 J
This means that the heat lost by the unknown solid is equal to the heat gained by the water:
q_solid = -q_water
q_solid = -4009 J
Next, we can calculate the change in temperature of the solid:
ΔT_solid = (32°C - 80°C) = -48°C
Now, we can solve for the specific heat of the solid:
q_solid = m_solid * c_solid * ΔT_solid
-4009 J = (90.0 g) * c_solid * (-48°C)
c_solid = -4009 J / (90.0 g * -48°C)
c_solid = 1.02 J/g°C
Therefore, the specific heat of the unknown solid is 1.02 J/g°C.
7. What is the reason that methemoglobinemia was isolated to Troublesome Creek area of KY? (In other
words why was the disorder only prevalent in KY; why didn't other states see cases like this?)
Methemoglobinemia was caused by contaminated well water and a genetic predisposition in the population of Troublesome Creek, KY.
Methemoglobinemia was detached to the Problematic Rivulet area of KY in view of the novel blend of ecological variables and hereditary inclination in the populace. The issue was brought about by the utilization of well water polluted with elevated degrees of nitrate and nitrite, which can cause the arrangement of methemoglobin in the blood. The populace in this space was to a great extent slipped from a little gathering of trailblazers who settled there during the 1800s, which might have added to a higher pervasiveness of the hereditary characteristic that inclines people toward the issue. The particular mix of hereditary defenselessness and ecological openness in this populace probably prompted the secluded flare-up of methemoglobinemia around here.
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How many grams of O are in 615g of N2O?
There are approximately 223.2 grams of oxygen in 615 grams of N2O.
To find the number of grams of O in 615g of N2O, we first need to understand the chemical formula of N2O. N2O is a compound made up of two nitrogen atoms (N) and one oxygen atom (O). Therefore, the molecular weight of N2O would be:
(2 x atomic weight of N) + (1 x atomic weight of O)
= (2 x 14.01 g/mol) + (1 x 16.00 g/mol)
= 44.01 g/mol
Now, to calculate the number of grams of O in 615g of N2O, we need to know the proportion of O in the compound. Since there is only one oxygen atom in each molecule of N2O, we can find the proportion of O by dividing the atomic weight of O by the molecular weight of N2O:
Atomic weight of O / Molecular weight of N2O
= 16.00 g/mol / 44.01 g/mol
= 0.363
This means that oxygen makes up 36.3% of the total weight of N2O. To find the number of grams of O in 615g of N2O, we can multiply the total weight by the proportion of O:
615g x 0.363
= 223.2g
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ASAP!! BRAINLIEST! Please help and show work
Quantifying chemical reactions
Quantifying chemical reactions is essential in understanding the stoichiometry of a reaction, predicting product formation, and optimizing product yield in industrial applications. Stoichiometric coefficients and limiting reactants are two important tools used in this process.
Quantifying chemical reactions involves measuring the amount of reactants and products involved in a chemical reaction. This is important in determining the stoichiometry of the reaction, which refers to the relative amounts of reactants and products involved. Stoichiometry is a crucial concept in chemistry because it allows scientists to predict the amount of product that will be formed from a given amount of reactant, or vice versa.
One way to quantify chemical reactions is through the use of stoichiometric coefficients. These coefficients represent the number of moles of each reactant and product involved in the reaction. For example, the balanced chemical equation for the reaction between hydrogen gas and oxygen gas to form water is:
[tex]2H2 + O2 → 2H2O[/tex]
This equation tells us that two moles of hydrogen gas react with one mole of oxygen gas to form two moles of water. The stoichiometric coefficients can be used to determine the mass of each reactant and product involved in the reaction, using the molar masses of each substance.
Another way to quantify chemical reactions is through the use of limiting reactants. A limiting reactant is the reactant that is completely consumed in a reaction, limiting the amount of product that can be formed. The amount of product formed will be determined by the amount of limiting reactant present. This concept is important in industrial chemistry, where maximizing product yield is often the goal.
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What is the pH of a solution that has a H+ concentration of 1.9x10-6?
The pH of the solution is 5.72, which is slightly acidic.
pH is a measure of the acidity or basicity of a solution. It is defined as the negative logarithm of the hydrogen ion concentration (H+) in a solution. The pH scale ranges from 0 to 14, where a pH of 7 is neutral, pH below 7 is acidic, and pH above 7 is basic. The formula to calculate pH is pH = -log[H+], where [H+] represents the concentration of hydrogen ions in moles per liter.
Given the H+ concentration of 1.9x10-6, we can calculate the pH of the solution as follows:
pH = -log(1.9x10-6) = 5.72
It is important to note that pH is an important factor in various chemical and biological processes. It can affect the solubility of certain substances, enzymatic activity, and the growth and survival of living organisms. Maintaining the appropriate pH is crucial for the proper functioning of these processes.
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What mass of CO2 can be produced from 25.0 g CaCO3 given the decomposition reaction CaCO3 => CaO + CO2
25.0 g of CaCO3 will produce 11.0 g of CO2. Mass is an intrinsic property of an object, meaning it does not depend on the object's location or the presence of other objects.
What is Mass?
Mass is a measure of the amount of matter in an object. It is a scalar quantity and is typically measured in units such as grams (g) or kilograms (kg). Mass is not the same as weight, which is a measure of the force exerted on an object due to gravity.
The balanced chemical equation for the decomposition of calcium carbonate (CaCO3) is:
CaCO3 → CaO + CO2
According to the equation, 1 mole of CaCO3 produces 1 mole of CO2. The molar mass of CaCO3 is 100.09 g/mol, which means that 1 mole of CaCO3 has a mass of 100.09 g.
To calculate the mass of CO2 produced from 25.0 g of CaCO3, we first need to convert the mass of CaCO3 to moles:
25.0 g CaCO3 x (1 mol CaCO3/100.09 g CaCO3) = 0.2498 mol CaCO3
Since 1 mole of CaCO3 produces 1 mole of CO2, we know that 0.2498 mol of CaCO3 will produce 0.2498 mol of CO2.
To convert the moles of CO2 to mass, we can use the molar mass of CO2, which is 44.01 g/mol:
0.2498 mol CO2 x 44.01 g/mol = 11.0 g CO2
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1. Which of the following stars has a temperature of approximately 9000 K and luminosity about to
20 times greater than the Surfs luminos
a Sirius
b. Procyon
c. Figel
d. Polaris
2. Which of the following types of stars is considered part of the main sequera
a Supergants
b. Red giants
c. Red dwarts
d. White dwarfs
3. Which of the following stars is cooler than the
Surf
a. Procyon B
b. Pigel
C. Barnard's Star
d. Sirius
4. The Sun is classified with which of the following types of stars?
a. Supergiants
b. Red giants
c. Main sequence
d. White dwars
5. Which of the forces listed below is most responsible for the formation of start?
a. Gravity
b. Magnetism
c. Bectromagnetism
d. Light
6. Which star has a higher luminosity and a lower temperature than the Sun?
a. Pigel
b. Barnard's Star
c. Alpha Centauri
d. Aldebaran
7. Compared to the temperature and luminosity of the star Polars, the star Srus is
a. hotter and more luminous
b. hotter and less luminous
c. cooler and more luminous cooler and less luminous
1. The star that has a temperature of approximately 9000 K and luminosity about 20 times greater than the Sun’s luminosity is Vega.
2. The type of star that is considered part of the main sequence is red dwarfs.
3. The star that is cooler than the Sun is Barnard’s Star.
4. The Sun is classified as a main sequence star.
5. The force most responsible for the formation of stars is gravity.
6. The star that has a higher luminosity and a lower temperature than the Sun is Aldebaran.
7. Compared to the temperature and luminosity of the star Polaris, the star Sirius is hotter and more luminous.
A gas‑filled weather balloon has a volume of 56.0 L
at ground level, where the pressure is 761 mmHg
and the temperature is 23.1 ∘C.
After being released, the balloon rises to an altitude where the temperature is −6.97 ∘C
and the pressure is 0.0772 atm.
What is the weather balloon's volume at the higher altitude?
What is the electron configuration for magnesium (Mg)?
O A. 1s²2s²2p²356
B. 15²25²3s23p6
C. 3s²3p 3d
D. 1s²2s²2p63s²
Answer:
D is correct.(1s22s22p63s2)
Can someone please help me with chemistry?
Show steps! Thank you
a. The mass of Cr2O3 is 0.559 g Cr2O3 is the maximum amount of Cr2O3 produced.
b.The limiting reactant is Cr(NO3)3 because it produces less moles of Cr2O3 than Na2O.
c. The percent yield is 84%.
How do we calculate?The balanced equation is shown below:
2 Cr(NO3)3 + 3 Na2O → Cr2O3 + 6 NaNO3
moles of Cr(NO3)3 = 1.75 g / 238.01 g/mol = 0.00735 mol
moles of Na2O = 1.75 g / 61.98 g/mol = 0.0282 mol
moles of Cr2O3 = (0.00735 mol Cr(NO3)3) × (1 mol Cr2O3 / 2 mol Cr(NO3)3) = 0.00368 mol Cr2O3 (theoretical yield)
mass of Cr2O3 = (0.00368 mol Cr2O3) × (151.99 g/mol) = 0.559 g Cr2O3
The percent yield can be calculated by dividing the actual yield by the theoretical yield and multiplying by 100%:
percent yield = (actual yield / theoretical yield) × 100%
percent yield = (0.455 g / 0.559 g) × 100% = 81.4%
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which one have least PH
a. CH3CH2COOH
b. CH2CLCH2COOH
c. CH3CHCL2COOH
d. CH3CH2CH2COOH
CH₃CHCl₂COOH is 2,2-dichloropropanoic acid, with the least pH, option (c) is correct.
pH is a measure of the acidity or basicity of a solution. A lower pH indicates a higher acidity. Acidity is due to the presence of hydrogen ions (H⁺) in a solution. The more the concentration of H⁺, the lower the pH. CH₃CH₂COOH is propanoic acid, which has a pH of around 4.9.
CH₂ClCH₂COOH is 2-chloropropanoic acid, which has a pH of around 2.8 due to the electron-withdrawing effect of the chlorine atom. CH₃CH₂CH₂COOH is butanoic acid, which has a pH of around 4.8. Thus, CH₃CHCl₂COOH is 2,2-dichloropropanoic acid, which has the least pH among the given options, around 1.5 due to the presence of two electron-withdrawing chlorine atoms, option (c) is correct.
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Answer:
5. 0.566 g
6. A. 100 times more
Explanation:
5. The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration. For a solution with pH=2, the concentration of hydrogen ions is 10^-2 mol/L. Since HBr is a strong acid, it dissociates completely in water to produce H+ and Br- ions. Therefore, the concentration of HBr in the solution is also 10^-2 mol/L.
The molar mass of HBr is 80.91194 g/mol
So, in a 700 mL solution (0.7 L), there are
0.7 L * 10^-2 mol/L = 0.007 mol of HBr.
This corresponds to 0.007 mol * 80.91194 g/mol = 0.566 g of HBr dissolved in the solution.
6. The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration. This means that for each decrease in pH by 1 unit, the hydrogen ion concentration increases by a factor of 10. Since the difference in pH between the two solutions is 3 units (6-3=3), the hydrogen ion concentration in the solution with pH=3 is 10^3 = 100 times more than in the solution with pH=6.
The characteristics of two different types of reactions are shown below:
Reaction A: An atom loses electrons during the reaction.
Reaction B: An atom loses protons and neutrons during the reaction.
Which statement is true about the two reactions?
Both reactions retain the identity of the elements.
Both reactions change the identity of the elements.
Reaction A produces more energy than Reaction B.
Reaction B produces more energy than Reaction A.
The statement that is true about the reactions is
Both reactions retain the identity of the elements.How to identify the true statementIn Reactions A and B, the participating atoms preserve their elemental identity despite losing electrons (in Reaction A) or protons and neutrons (in Reaction B). This can give rise to distinct isotopes or ions of the same element while preserving its fundamental attributes.
The statements concerning energy production aren't necessarily accurate or linked with the reaction's traits. Energy output depends on many variables, such as specific reactants involved and their conditions during reactions.
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