What volume, in liters, would 88.9 grams of a substance occupy if it’s density is 2.38 g/mL

Answer:

well just like grass that helps animals eat rocks may give an animal a home

Answer:

Liquid

Explanation:

The molecular formula of hydrate : CaCl₂.6 H₂O

So there are 6 molecules of H₂O

Given

54.7g CaCl₂ and 53.64 g H₂O

Required

The number of molecules H₂O

Solution

mol CaCl₂ :

= mass : MW

= 54.7 : 111 g/mol

= 0.493

mol H₂O :

= 53.64 : 18 g/mol

= 2.98

mol ratio H₂O : CaCl₂ :

= 2.98/0.493 : 0.493/0.493

= 6 : 1

Answer:

I>Sn>Xe

Explanation:

Electron affinity refers to the ability of an atom to accept electron(s) and form a negative ion.

We know that electron affinity is a periodic trend that increases across the period but decreases down the group.

Hence the, electron affinity of iodine is far higher than that of tin. However, xenon is a noble gas and does not accept electrons. Hence, it has an electron affinity of 0 KJ/mol.

Answer:

Explanation:

a )

Average reaction rate between 0 and 1500s

Time duration = 1500 s

moles reacted = .184 - .016 = .168 moles

Moles reacted per second = .168 / 1500

= 112 x 10⁻⁶ moles /s

b )

Average reaction rate between 200 and 1200s

Time duration = 1000 s

moles reacted = .129 - .019 = .11 moles

Moles reacted per second = .11 / 1000

= 110 x 10⁻⁶ moles /s

c )

the instantaneous rate of the reaction at t=800s

We shall assume that between 500 s and 1200 s , rate of reaction is uniform

rate between 500 and 1200

Time duration = 700 s

moles consumed = .069 - .019 = .05 moles

Rate of reaction = .05 / 700

= 71 .4 x 10⁻⁶ moles / s

This will also be instantaneous rate of reaction at t = 800 s .

Answer:

0 for the elemental form, +2 in its compounds.

Answer:

2.5 moles of oxygen are produced.

Explanation:

Given data:

Number of moles of O₂ produced = ?

Number of moles of HgO decomposed = 5 mol

Solution:

Chemical equation:

2HgO      →     2Hg + O₂

now we will compare the moles of HgO and O₂.

           HgO         :          O₂

            2              :          1

            5              :         1/2×5 = 2.5

Thus, from 5 moles of HgO 2.5 moles of oxygen are produced.

Answer:  On Earth, liquid water exists on the surface in the form of oceans, lakes and rivers. It also exists below ground as groundwater, in wells and aquifers. Water vapor is most visible as clouds and fog. The frozen part of Earth's hydrosphere is made of ice: glaciers, ice caps and icebergs.

Answer:

the effluent concentration is 0.06236 mg/L

Explanation:

Given that;

treatment capacity [tex]V_{0}[/tex] = 3,800 m³/d =  ( 3,800 × 86.4) =  43.98 L/sec

reactor's volume V = 45 m³ = (45 × 1000) = 45,000 L

reaction rate constant K =  0.0125 s⁻¹

influent manganese concentration [tex]CA_{0}[/tex] = 0.86 mg/L

-[tex]r_{A}[/tex] = [tex]KC_{A}[/tex]

Now, performance equation for CSTR is expressed as follows;

[tex]\frac{V}{V_{0} }[/tex] = [tex]\frac{CA_{0} -CA _{} }{-r_{A} }[/tex]

[tex]\frac{V}{V_{0} }[/tex] = [tex]\frac{CA_{0} -CA _{} }{KC_{A} }[/tex]

So we substitute

45000L / 43.98 L/sec = ( 0.86 mg/L - CA) / 0.0125 CA

we cross multiply

562.5CA = 37.8228 - 43.98CA

562.5CA + 43.98CA = 37.8228

606.48CA = 37.8228

CA = 37.8228 / 606.48

CA = 0.06236 mg/L

Therefore, the effluent concentration is 0.06236 mg/L

Answer:

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Explanation:

i it true?

Answer:

no way

Explanation:

more free points

Answer:

44

Explanation:

Given that :

Mass of solute = Mass of urea = 16g

Mass of water = 20g

Mass of solution = (mass of solute + mass of solvent) = (mass of urea + mass of water) = (16g + 20g) = 36g

Percentage Mass = (mass of solute / mass of solution) * 100%

Percentage Mass = (16 / 36) * 100%

Percentage Mass = 0.4444444 x 100%

Percentage Mass = 44.44%

Percentage Mass = 44%

Answer:

a. ((100 - 35)/100) times 5.5 grams = 3.575 g

Explanation:

Given that:

The sample of carbon and oxygen = 5.5g

where carbon makes 35% of the mass of the substances.

It implies that oxygen will make: (100 - 35)% = 65%

Suppose y be the mass of the oxygen;

Then:

[tex]y = \dfrac{(100-35)}{100} \times 5.5 \ g[/tex]

[tex]y = \dfrac{(65)} {100} \times 5.5 \ g[/tex]

[tex]y = 3.575 \ g[/tex]

The mass of carbon [tex]= \dfrac{35}{100} \times 5.5 \ g[/tex]

= 1.925 g

Answer:

Average atomic mass  = 3.9 amu

Explanation:

Given data:

Percent abundance of He-2 = 0.420%

Percent abundance of He-3 = 2.75%

Percent abundance of He-4 = 96.83%

Average atomic mass = ?

Solution:

Average atomic mass = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass) + (abundance of 3rd isotope × its atomic mass)  / 100

Average atomic mass = (0.420×2)+(2.75×3) +(96.83×4)/100

Average atomic mass =  0.84 + 8.25 +387.32 / 100

Average atomic mass = 396.41 / 100

Average atomic mass  = 3.9 amu.

Explanation:

first we have to find molar mass of ca(H2c3o2)2

40+(1*2)2+(12*3)2+(16*2)2

40+4+72+64=180g/mole

m=n*Mm

m=1.75mole*180g/mole

m=315g

Test tubes heat small amounts of liquids while boiling tube boils liquids

Answer: 49 joules

Explanation: gravitational potential energy = mgh

m= mass kg,  g= acceleration due to gravity 9.8 m/sec/sec, h= height m

=5*9.8.1 joules = 49 joules

Answer:

See explanation

Explanation:

Here we are trying to see how a binary covalent compound is named. A binary covalent compound comprises of only two elements held together by covalent bonds.

The first element retains its normal name whereas the second element has the suffix -ide added to it.

For instance, CO2 is named as carbon dioxide, HBr is named as hydrogen bromide etc.

Answer: it's ide

Explanation:

Got it right in the quiz

Answer:

37.4 mol.

Explanation:

Hello!

In this case, since the Avogadro's number help us to realize that one mole of any substance contains 6.022x10²³ formula units, in this case atoms of zinc, the following dimensional analysis provides the correct answer:

[tex]=2.25x10^{25} atoms*\frac{1mol}{6.022x10^{23}atoms}\\\\= 37.4mol[/tex]

Best regards!

Answer:

Vibrational energies of atoms

Explanation:

Planck applied quantization to Vibrational energies of atoms because in Black body spectrum prediction a blackbody at equilibrium is expected to radiate energies at various Frequencies ( i.e. increase in radiated energy ∝ increase in frequency ) but towards the ultraviolet region of the spectrum the energy radiated begins to drop as frequency increases. The phenomenon of drop in energy with increase in frequency is termed Ultraviolet catastrophe. hence to solve this phenomenon Planck applied quantization to Vibrational energies of atoms

The percent composition of the compound.

A O-18.18%, N-21.21%, H-60.60%

Given

6.00 grams of oxygen,

7.00 grams of nitrogen,

20.00 grams of hydrogen.

Required

The percent composition

Solution

Total mass :

= mass of O + mass of N + mass of H

= 6 + 7 + 20

= 33 g

% O = 6/33 x 100%= 18.18%

% N = 7/33 x 100%=21.21%

% H = 20/33 x 100% = 60.6 %

Answer:

[tex]\Delta H_{f,C_3H_4}=276.8kJ/mol[/tex]

Explanation:

Hello!

In this case, since the equation we use to model the heat exchange into the calorimeter and compute the heat of reaction is:

[tex]\Delta H_{rxn} =- m_wC_w\Delta T[/tex]

We plug in the mass of water, temperature change and specific heat to obtain:

[tex]\Delta H_{rxn} =- (35000g)(4.184\frac{J}{g\°C} )(2.316\°C)\\\\\Delta H_{rxn}=-339.16kJ[/tex]

Now, this enthalpy of reaction corresponds to the combustion of propyne:

[tex]C_3H_4+4O_2\rightarrow 3CO_2+2H_2O[/tex]

Whose enthalpy change involves the enthalpies of formation of propyne, carbon dioxide and water, considering that of propyne is the target:

[tex]\Delta H_{rxn}=3\Delta H_{f,CO_2}+2\Delta H_{f,H_2O}-\Delta H_{f,C_3H_4}[/tex]

However, the enthalpy of reaction should be expressed in kJ per moles of C3H4, so we divide by the appropriate moles in 7.00 g of this compound:

[tex]\Delta H_{rxn} =-339.16kJ*\frac{1}{7.00g}*\frac{40.06g}{1mol}=-1940.9kJ/mol[/tex]

Now, we solve for the enthalpy of formation of C3H4 as shown below:

[tex]\Delta H_{f,C_3H_4}=3\Delta H_{f,CO_2}+2\Delta H_{f,H_2O}-\Delta H_{rxn}[/tex]

So we plug in to obtain (enthalpies of formation of CO2 and H2O are found on NIST data base):

[tex]\Delta H_{f,C_3H_4}=3(-393.5kJ/mol)+2(-241.8kJ/mol)-(-1940.9kJ/mol)\\\\\Delta H_{f,C_3H_4}=276.8kJ/mol[/tex]

Best regards!

Answer:

0.0876L of 0.478M Na₃PO₄ are needed

Explanation:

The reaction of calcium chloride, CaCl₂, with sodium phosphate, Na₃PO₄ is:

3CaCl₂ + 2Na₃PO₄ → Ca₃(PO₄)₂ + 6NaCl

Where 3 moles of calcium chloride react with 2 moles of sodium phosphate to produce 1 mole of calcium phosphate.

To solve this question we need to find moles of CaCl₂ added. Using the reaction we can find the moles of Na₃PO₄ that are needed to react completely and the volume using its concentration:

Moles CaCl₂:

0.225L * (0.279mol / L) = 0.0628moles of CaCl₂

Moles Na₃PO₄:

0.0628moles of CaCl₂ * (2mol Na₃PO₄ / 3 mol CaCl₂) =

0.0419moles of Na₃PO₄

Volume 0.478M Na₃PO₄:

0.0419moles of Na₃PO₄ * (1L / 0.478mol) =

Answer: Na, S, Cl

Explanation:

Atomic size decreases as one moves from left to right on the periodic table with elements in the same period. This is as a result of the electrons increasing in the outer circle and thus being drawn to the protons in the nucleus which will lead to the outer shell area decreasing.

Sodium (Na) comes before Sulfur (S) which comes before Chlorine (S) so this is the decreasing order as they are all in the same period.

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Answer:

Ideal Gas

The ideal gas is extremely small and the mass is almost zero and no volume Ideal gas is also considered as a point mass.

Real Gas

The molecules of real gas occupy space though they are small particles and also have volume.

anation:

The differences between an ideal gas and a real gas are that the ideal gas follows the gas laws perfectly under all conditions. Whereas a real gas deviates from ideal gas behaviors.

The ideal gas law, also known as the general gas equation, is a fundamental principle in thermodynamics and relates the pressure, volume, temperature, and number of moles of an ideal gas.

An ideal gas is a theoretical gas that follows the gas laws perfectly under all conditions of temperature and pressure. It is assumed to have no volume, no intermolecular forces, and elastic collisions between its particles. An ideal gas also obeys the ideal gas law.

On the other hand, a real gas is a gas that does not follow the gas laws perfectly under all conditions of temperature and pressure. Real gases have volume and intermolecular forces that affect their behavior. These forces cause deviations from ideal gas behavior, especially at high pressures and low temperatures.

In summary, while an ideal gas is a theoretical gas that follows the gas laws perfectly under all conditions, a real gas is a gas that deviates from ideal gas behavior due to its volume, intermolecular forces, and non-elastic collisions between its particles.

Learn more about ideal gas law here:

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Answer:

Kindly check the attached picture for the diagram of the chemical compound.

Explanation:

So, the following parameters were given from the question above;

=> A triplet at 0.9 ppm and a quartet at 1.4 ppm, a singlet at 1.35 ppm. Now, the unknown compound has a molecular formula of C7H16O.

For a triplet at 0.9ppm, there are nine (9) atoms of hydrogen, for the quartet at 1.4ppm there are six(6) atoms of hydrogen and for the singlet at 1.35 ppm, the number of hydrogen atoms is one(1). Hence, the total number of hydrogen atoms = 16.

Therefore, number of bondings = [(2 × number of carbon atoms) + 2 - number of hydrogen atoms present on the compound)/2 .

Thus number of bonds =[( 2× 7) + 2 - 16] ÷ 2 = 0.

Hence, there is no double bond or ring in the compound.

Mostly and for what I would say is A

The gases can undergo compression when subjected to lower temperatures and pressure. The water bottle becomes dented as the collision slowed down and got closer to each other. Thus, option C is correct.

Freezing has been the physical process that is involved in changing the states of matter from liquid to solids. This results in a decrease in the entropy of the water which decreases the heat and randomness of the particles.

As the temperature decreases the collision and the kinetic energy of the particles decreases. This results in the loss of entropy and makes the molecules or the particles show a higher force of attraction leading to close packing. The space becomes dense and tightly packed.

As the particle becomes closely packed it dents the water bottle at low temperature as now it has its own shape (solids) unlike the liquids. The lower temperature converts the liquids into solids.

Therefore, as the water freezes the bottle experiences a dent as ice is formed from liquids by freezing.

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Answer:

all of the above

Explanation:

now I will bless you with this-