What is the pH of a solution with a H+ ion of 2×10-¹²?​

The vessel's internal pressure is atm, is  \(6.66*10^{-6} atm\)

A vacuum pump is a machine that expels air or gas from a sealed space in order to create a partial vacuum and a difference in pressure. Based on the pressure needs and the application it serves, vacuum pumps are designed using a range of technologies.Fatal accidents have happened in the history of pressure vessel invention and use, proving that pressure vessels can be harmful.A container designed to carry gases or liquids at a pressure much higher than atmospheric pressure is known as a pressure vessel.

The pressure in the vessel in atm is \(6.66 * 10^{-6} atm\).

To calculate this, we first convert \(5.0 * 10^{-3} mmHg\) to atm.

1 mmHg = 0.001315789 atm

Here, \(5.0 * 10^{-3} mmHg = 6.66 * 10^{-6} atm.\)

Therefore, the pressure in the vessel in atm is \(6.66*10^{-6} atm\)

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Answer:

The difference between the two is:

\([Kr]4d^1^05s^25p^2\) is the Orbital Occupancy

\([Kr]5s^24d^1^05p^2\) is the Orbital Filling Order

Both are correct, I don't think your teacher will be so nit-picky to care.

Dalton asserted the indivisible nature of atoms. The mass and chemical characteristics of all atoms of a specific element are the same.

Atoms of two different elements combine to form compounds: Dalton's atomic theory states that atoms of different elements can combine in different proportions to form compounds.

Atoms of an element are identical to atoms of other elements: Dalton's atomic theory states that atoms of the same element have the same properties and composition.

Every element is made of atoms: Dalton's atomic theory states that all elements are made up of atoms, which are the smallest indivisible particles of matter.

In a chemical reaction, some atoms disappear and new atoms appear: Dalton's atomic theory states that in a chemical reaction, atoms are neither created nor destroyed, but simply rearranged into new combinations.

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the possible quantum numbers (ordered n, ℓ, mℓ ) are:Option B.5, 3, -3 and Option C. 4, 3, -2

The quantum numbers n, ℓ, mℓ represent respectively the principal quantum number, the orbital angular momentum quantum number and the magnetic quantum number.

These are the three most important quantum numbers. T

here is another quantum number called the spin quantum number, denoted by ms.

Let's see which of the given quantum number sets is possible.2, 1, 3 is not possible because for ℓ = 1, mℓ can only be -1, 0, or 1. 5, 3, -3 is possible.4, 3, -2 is possible. -4, 3, 1 is not possible.

For any value of ℓ, mℓ must be between -ℓ and +ℓ. e. 2, 1, -2 is not possible because for ℓ = 1, mℓ can only be -1, 0, or 1. f. 3, 2, 2 is not possible because for ℓ = 2, mℓ can only be -2, -1, 0, +1, or +2. g. 3, 3, 1 is not possible because for any value of ℓ, mℓ must be between -ℓ and +ℓ.

Therefore, the possible quantum numbers (ordered n, ℓ, mℓ ) are:5, 3, -34, 3, -2

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Answer:

\(E=2.06\times 10^{-19}\ J\)

Explanation:

Given that,

The wavelength of electromagnetic radiation is 963.5 nm.

We need to find the energy of a photon with this wavelength.

The formula used to find the energy of a photon is given by :

\(E=\dfrac{hc}{\lambda}\\\\E=\dfrac{6.63\times 10^{-34}\times 3\times 10^8}{963.5\times 10^{-9}}\\\\E=2.06\times 10^{-19}\ J\)

So, the energy of a photon is \(2.06\times 10^{-19}\ J\).

The aluminum ground state electron configuration is 1s²2s²2p⁶3s²3p¹.

The electron configuration of aluminum will therefore be  1s²2s²2p⁶3s²3p¹. Scientists can easily write and communicate how electrons are arranged around an atom's nucleus using the configuration notation. It is now simpler to comprehend and predict how atoms will interact to form chemical bonds as a result.

The Aufbau Principle, Pauli-exclusion Principle, and Hund's Rule are the three key rules that we adhere to. By removing electrons from the outermost p orbital first, then the s orbital, and finally the d orbitals, the electronic configuration of cations is determined (if any more electrons need to be removed).

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Answer:

3.3 moles of H₂O.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

4NH₃ + 5O₂ —> 6H₂O + 4NO

From the balanced equation above,

4 moles of NH₃ reacted to produce 6 moles of H₂O.

Finally, we shall determine the number of mole of H₂O produced by the reaction of 2.2 moles of NH₃. This can be obtained as follow :

From the balanced equation above,

4 moles of NH₃ reacted to produce 6 moles of H₂O.

Therefore, 2.2 moles of NH₃ will react to produce = (2.2 × 6)/4 = 3.3 moles of H₂O.

Thus, 3.3 moles of H₂O were obtained from the reaction.

The volume of \(N_2O_5\) needed to produce 9.64 L of \(NO_2\) is 4.97 L, calculated using stoichiometry and the ideal gas equation.

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The density of the object weighing 15.50 g  when placed inside the water having initial volume 12.5 mL and the final volume 16.0 mL is 4.42 g/mL.

Density is defined as the mass of a substance per unit of its volume. It is denoted by a Greek symbol ρ. Density is the mass of a substance divided by its volume. It is given by -

                                              ρ = m

                                                      v

where,

ρ = density

m = mass

v = volume

Given data :

Mass (m) = 15.50 g

Volume (v) = (Final volume - initial volume)

               v = 16.0 mL - 12.5 mL = 3.5 mL

Putting the values in above formula,

Density = mass  

                volume

Density = 15.50 = 4.42 g/mL

                  3.5

The density of object is found to be 4.42 g/mL

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Answer:

Explanation:

Endothermic reactions are reactions that absorbs heat energy from the environment or surroundings

They are direct opposites of exothermic reactions in that their reaction vessels might feel cool to the touch

They generally have a reduced amount of heat compared to the environment at that point in time

The metal X has an approximate molar mass of 42.36 g/mol and the metal is most likely calcium.

The molar mass of the metal carbonate XCO₃ and identify the metal X, we need to calculate the number of moles of XCO₃ and CO₂ using the given masses and molar masses.

The molar mass of CO₂ (carbon dioxide) is 12.011 g/mol (for carbon) + 2 * 15.999 g/mol (for oxygen) = 44.01 g/mol.

The number of moles of CO₂ can be calculated using the formula:

moles of CO₂ = mass of CO₂ / molar mass of CO₂

moles of CO₂ = 0.855 g / 44.01 g/mol

moles of CO₂ ≈ 0.01944 mol

Since the reaction stoichiometry is 1:1 between XCO₃ and CO₂, the number of moles of XCO₃ is also approximately 0.01944 mol.

molar mass of XCO₃ = mass of XCO₃ / moles of XCO₃

molar mass of XCO₃ = 2.012 g / 0.01944 mol

molar mass of XCO₃ ≈ 103.38 g/mol

The molar mass of XCO₃ is approximately 103.38 g/mol.

To determine the metal X:

molar mass of X = molar mass of XCO3 - molar mass of CO3

molar mass of X = 103.38 g/mol - (12.011 g/mol + 3 * 15.999 g/mol)

molar mass of X ≈ 42.36 g/mol

Metal X is most likely Calcium that has a molar mass of 40 g/mol

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Answer:

See explanation

Explanation:

Let us look at the reaction again;

Cr2O7 2- (aq) + H2O(l)⇄ 2CrO4 2-(aq) + 2H^+(aq)

When we add sodium hydroxide to the system as shown, the hydroxide ion removes the hydrogen ion thereby leaving a large concentration CrO4^2-(aq) in the system this causes the solution to turn green(equilibrium position shifts to the right).

The net ionic equation is;

OH^-(aq) + H^+(aq) ----> H2O(l)

The reaction;

OH^-(aq) + H^+(aq) ----> H2O(l) is exothermic hence, if the temperature of the system is increased, the equilibrium position will shift towards the left hand side and the solution turns orange.

Tables are more suitable than a graph to show data because they present data in as close to raw form as possible.

Data can be represented in Tables, charts and graphs. These data representation are used for two broad purposes.

Unlike the case of graphs that use abstraction to focus on trends and numerical relationships, tables present data in as close to raw form as possible.

Tables are usually meant to be read, so they are ideal when the data that is present are those type of data that cannot easily be presented visually, or when the data requires more specific attention.

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Both Example A and Example B are correct, but they refer to different processes. Example A refers to the physical action of chopping vegetables into smaller pieces, which can make them easier to cook and eat.

This process does not change the fundamental nature of the vegetable, but simply alters its physical properties.

Example B, on the other hand, refers to the process of digestion in the human body. During digestion, food is broken down into simpler forms, such as sugars, amino acids, and fatty acids, which can be absorbed and used by the body for energy and other functions. This process involves both physical and chemical changes, as enzymes in the digestive system break down complex molecules into simpler ones.

In summary, Example A describes a physical process that alters the size and shape of a vegetable, while Example B describes a physiological process that breaks down complex food molecules into simpler forms for use by the body. Both processes are important for preparing and consuming nutritious food.

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169.2K is the equilibrium temperature of the system after the insulating wall is removed.

Generally speaking, a condition of equilibrium is one in which nothing is changing. A body in equilibrium won't undergo any energy exchanges, either positive or negative. Equilibrium is defined significantly differently in biology, physics, and chemistry.

Yet the underlying idea is the same. A body in balance will be least affected by outside influences. Even when external pressures are present, the opposing forces often have a balanced impact on the item under consideration.

for gas, n1=1mol

               T1= 148K

for solid,n2=2mol

            T2=178K

for conservation of energy, ΔQ= Qgas+ Qsolid=0

Q= CvΔT

0=Cvgas(Teql-148) + Cvsolid(Teq-178)

0= 5/2×1×R(Teql-148) + 3×2×R(Teq-178)

Tequi= 169.2K

Therefore, 169.2K is the equilibrium temperature of the system after the insulating wall is removed.

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Answer:

b. the heating of 10 g of liquid water from 0°C to 100°C.

Explanation:

Hello,

In this case, we must notice a., c. and d. processes are not actually absorbing heat but releasing it since cooling, freezing and condensation are processes with negative heat sign since matter changes from a state of more energy to a state of less energy. We can prove this by realizing that freezing enthalpy of water is -6.00 kJ/mol, condensation enthalpy of eater is -40.8 kJ/mol and a change of temperature from 100 °C to 0 °C is negative.

In such a way, the only process absorbing heat is b. the heating of 10 g of liquid water from 0°C to 100°C since energy must be added to the system, or absorbed by it in order to attain the heating.

Regards.

The process having the greatest amount of heat is:

b. the heating of 10 g of liquid water from 0°C to 100°C.

The options a., c. and d. processes are not actually absorbing heat but releasing it since cooling, freezing and condensation are processes with negative heat sign since matter changes from a state of more energy to a state of less energy.

The freezing enthalpy of water is -6.00 kJ/mol, condensation enthalpy of eater is -40.8 kJ/mol and a change of temperature from 100 °C to 0 °C is negative.

So out of all the options, only process at b is a heating process thus it will absorb greatest amount of heat.

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Answer:

As of right now (4-7-2021), the physical science requirement for the SLP certificate must be met by completing coursework in the areas of either chemistry or physics.

The balanced chemical equation is, Mg(s)+ SnSO4 (aq.) → MgSO4(aq.)+ Sn(s) .

The half cell reactions are, Sn2+(aq.)  + 2e-    ----->   Sn(s) and Mg(s)  ---->  Mg2+(aq.)   +  2e-  

A Half cell reaction is expressed either as an oxidation reaction in which electrons are lost or a reduction reaction where electronic are gained. The reactions occur in an electrochemical cell in which the electrons are lost at the anode through oxidation and consumed at the cathode where the reduction occurs. Half-cell reactions are useful in galvanic and voltaic cells in which the electrons flow from the anode to the cathode through an electrolyte to produce an electromotive force (EMF).

Half cell Reaction at cathode : Reduction 

Sn2+(aq.)  + 2e-    ----->   Sn(s)

Half- cell reaction at anode  : Oxidation 

Mg(s)  ---->  Mg2+(aq.)   +  2e-  

E1  is made of   Mg

E2 is made of  Sn 

Chemical species in solution S1 are  Mg2+  and SO42-  .

Chemical species in solution S2 are   Sn2+  and SO42-  

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Answer:

233.3 times

Explanation:

The diameter of a carbon atom is 1.5 x 10^-10 meters, so the circumference of a carbon atom is pi x diameter = 3.14 x 1.5 x 10^-10 m = 4.71 x 10^-10 m

If you have 2 x 10^19 atoms in a small speck of carbon and all the atoms laid side by side, the total circumference of all the atoms would be 2 x 10^19 x 4.71 x 10^-10 = 9.42 x 10^9 meters.

The circumference of the earth at the equator is 40,075 km, so that is 40,075 x 1000 = 40,075,000 meters.

Divide the total circumference of all the atoms by the circumference of the Earth:

9.42 x 10^9 m / 40,075,000 m = 233.3 times

Therefore, the atoms from this speck of carbon would extend around the Earth 233.3 times if they laid side by side.

Answer:

The balanced chemical equation for the reaction is:

5CaF2 · 3Ca3(PO4)2 + 24H2SO4 → 20H3PO4 + 10HF + 15CaSO4 · 2H2O

This equation shows that when fluorapatite is reacted with sulfuric acid, it produces phosphoric acid, hydrogen fluoride, and gypsum. The balanced equation indicates that 5 moles of CaF2·3Ca3(PO4)2 react with 24 moles of H2SO4 to produce 20 moles of H3PO4, 10 moles of HF, and 15 moles of CaSO4·2H2O.

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HAZMAT Class 6 Toxic and infectious substances.

Answer:

CLASS 2 Gases

Explanation:

Hope this helps

Answer:

Its D

Explanation:

I took the quiz

Answer:

D

Explanation:

IT IS REACTING

Answer: A

Explanation:

Answer:

By definition:

Example:

If I study hard in school, I will get good grades.

Answer:

The answer is "12.06"

Explanation:

Given:

\(M(HBrO) = 0.3\ M\\\\V(HBrO) = 20 \ mL\\\\M(KOH) = 0.15 \ M\\\\V(KOH) = 64 \ mL\)

\(\to mol(HBrO) = M(HBrO) \times V(HBrO) = 0.3 M \times 20 mL = 6 \ mmol\\\\\to mol(KOH) = M(KOH) \times V(KOH)= 0.15 M \times 64 mL = 9.6 mmol\)

  6 mmol of both will react

excess KOH remaining\(= 3.15 \ mmol\)

Volume\(= 20 + 64 = 84 \ mL\)

\([OH^{-}] = \frac{ 9.6 \ mmol}{84\ mL} = 0.01142\ M\)

use:

\(pOH = -\log [OH^-]\)

        \(= -\log (1.142\times 10^{-2})\\\\= 1.94\)

use:

\(PH = 14 - pOH\)

       \(= 14 - 1.94\\\\= 12.06\)

The pH of the resulting  solution is  12.63.

The equation of the reaction is;

HBrO(aq) + KOH(aq) ------> KOBr(aq) + H2O(l)

Number of moles of KOH= 64/1000 × 0.150 M = 0.0096 moles

Number of moles of HBrO = 20/1000 × 0.300 M = 0.0060 moles

Number of moles of excess base = 0.0096 moles -  0.0060 moles = 0.0036 moles

Total volume of solution = 64.0 mL +  20.0 mL = 84 mL = 0.084 L

Molarity of excess base =  0.0036 moles/0.084 L = 0.043 M

pOH = -log[OH-]

pOH = -log[ 0.043 M]

pOH = 1.37

pH + pOH = 14

pH = 14 -pOH

pH = 14 - 1.37

pH = 12.63

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Answer:

T₂  = 203.4 K

Explanation:

Given data:

Initial volume = 350.0 mL

Initial temperature = 22.7 °C

Initial pressure = 0.914 atm

Final temperature = ?

Final volume = 220.0 mL

Final pressure = standard =  1 atm

Solution:

First of all we will convert the temperature into kelvin.

22.7 °C + 273 = 295.7 K

Formula:  

P₁V₁/T₁ = P₂V₂/T₂

T₂  =  P₂V₂T₁  /P₁V₁

T₂  = 1 atm × 220.0 mL × 295.7 K /  0.914 atm  × 350.0 mL

T₂ = 65054 atm.mL.k /319.9 atm.mL

T₂  = 203.4 K

The equilibrium constant at this temperature is Kc= 4.17 x 10⁻⁶.

Since the equilibrium constant depends on the equilibrium concentration of both the reactants and the products of the chemical reaction.

Balanced reaction equation

2CH₄(g)⇌C₂H₂(g)+3H₂(g)

The initial concentration of the CH₄ = 0.093 M

The equilibrium concentration of the H = 0.017 M

Equilibrium constant = ?

Let's make the ice table

2CH₄(g) ⇌ C₂H₂(g) + 3H₂(g)

0.093 M 0 0

-2x +x +3x

0.093-2x x 0.017 M

3x = 0.017 M

Therefore, x =0.017 M /3 = 0.00567 M

Therefore, the equilibrium concentration of CH₄ =

0.093 M – 2x = 0.093 M – (2 x 0.00567 M) = 0.0817 M

Equilibrium concentration of the C₂H₄ = x = 0.00567 M

Let's write the equilibrium constant expression

Kc= [C₂H₄[H2]³/[CH₄]²

Let's put the values in the formula

Kc= [0.00567][0.017]³/[0.0817]²

Kc= 4.17 x 10⁻⁶

Therefore, the equilibrium constant is 4.17 x 10⁻⁶.

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Answer:

B) Pressure and Temperature

Explanation:

Just did it

To titrate 30.00 ml of a 0.1000 M \(NaOH\) solution, one needs about 0.6126 g of monoprotic \(KHP\).

1. To calculate the amount of \(NaOH\) needed to make a 0.1 M solution, we first need to calculate the number of moles of \(NaOH\) needed.

Molarity = moles of solute / liters of solution
0.1 M = x moles / 0.5 L
x = 0.05 moles

Now we can calculate the mass of \(NaOH\) needed:
Mass = moles x molecular weight

Mass = 0.05 moles x 40.3 g/mol
Mass = 2.015 g

Therefore, approximately 2.015 g of \(NaOH\) should be dissolved in 500 ml of distilled water to produce a solution with a molarity near 0.1 M.

2. We can use the equation:
Moles of \(NaOH\) = moles of \(KHP\)

Molarity x volume (in liters) of \(NaOH\) = moles of \(KHP\)
0.1000 M x 0.03000 L = moles of \(KHP\)

moles of \(KHP\) = 0.003
Now we can calculate the mass of \(KHP\) needed:

Mass = moles x molecular weight
Mass = 0.003 moles x 204.2 g/mol

Mass = 0.6126 g
Therefore, approximately 0.6126 g of monoprotic \(KHP\) is needed to titrate 30.00 ml of a 0.1000 M \(NaOH\) solution.

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