How many atoms of carbon are in 79.7 moles of carbon?

Answer:

4NH3+6NO+5N2+6H20

Explanation:

Answer:

moles= w/mm

moles=150/30

moles=5

Answer:

A B D

Explanation:

Answer:  A: Being the power source of stars

                B: Forming heavier elements from light elements

                D: Being used in thermonuclear weapons

Explanation: (Edmentum)

Answer: 0.637M

10.2M

1.36M

0.0982M

Explanation: the answer is 1.36M

The molarity of the CsOH solution is 0.636 M.

Molarity is the concentration of any substance in a place.

The reaction is

HBr + CsOH —> CsBr + H₂O

The formula of molarity

[tex]M = \dfrac{n}{V}[/tex]

[tex]\dfrac{0.25 \times 38.2 }{15} = 0.6366[/tex]

Thus, the molarity of the CsOH solution is 0.636 M.

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Answer:

pH = 10.95

Explanation:

To solve this question we must, as first, find pKb of dimethylamine. Then, using H-H equation we can solve the pH of the buffer:

pKb dimethylamine:

Based on the equilibrium:

(CH3)2NH(aq) + H2O(l) ⇄ (CH3)2NH2⁺(aq) + OH-(aq)

Kb is defined as:

Kb = [OH-] [(CH3)2NH2⁺] / [(CH3)2NH]

Both (CH3)2NH2⁺(aq) + OH- comes from the same equilibrium, that means:

[OH-] = [(CH3)2NH2⁺]

And: [(CH3)2NH] = 0.457M

[OH-] can be obtained from pH as follows:

14 -pH = pOH

14-12.2 = 1.8 =pOH

10^-pOH = [OH-] = 0.01585M

Replacing:

Kb = [0.01585M] [(0.01585M] / [0.457M]

Kb = 5.50x10⁻⁴

pKb = -logkb = 3.26

pH of the buffer:

Using H-H equation for bases:

pOH = pKb + log [conjugate acid] / [weak base]

pOH = 3.26 + log [0.280M] / [0.457M]

pOH = 3.05

pH = 14 - pOH

Since orbital period depends on how far you are from the sun, planets closer to the sun have a orbital period less than one earth year.

These planets are Mercury and Venus

Answer:

[tex]\rho=12g/cm^3[/tex]

Explanation:

From the question we are told that:

Length[tex]l=379.0pm=>379*10^{-10}cm[/tex]

Atomic mass of X [tex]M= 195.0 amu=>gmol^{-1}[/tex]

Where

[tex]Avogadro\ constant = 6.023 * 10^{23} mol-1[/tex]

Let

The Number of units in BCC unit cell [tex]n= 2[/tex]

Generally the equation for Density is mathematically given by

[tex]\rho= \frac{M x n}{l^3*Avogadro constant}[/tex]

[tex]\rho=\frac{197 x 2}{(379*10^{-10})^3*6.023 x 10^{23}}[/tex]

[tex]\rho=12g/cm^3[/tex]

Therefore he density of Xin g/cc

[tex]\rho=12g/cm^3[/tex]

Answer:

Percentage of Ba = 52.5%

Explanation:

We'll begin by calculating the molar mass of Ba(NO3)₂. This can be obtained as follow:

Molar mass of Ba(NO3)₂ = 137 + 2[14 +(16×3)]

= 137 + 2[14 + 48]

= 137 + 2[62]

= 137 + 124

= 261 g/mol

Next, we shall determine the mass of Ba in Ba(NO3)₂. This can be obtained as follow:

Mass of Ba in Ba(NO3)₂ = 137 g/mol

Finally, we shall determine the percentage of Ba in Ba(NO3)₂. This can be obtained as follow:

Percentage of Ba = mass of Ba / mass of Ba(NO3)₂ × 100

Percentage of Ba = 137 / 261 × 100

Percentage of Ba = 13700 / 261

Percentage of Ba = 52.5%

Thus, the percentage of Ba in Ba(NO3)₂ is 52.5%

Answer:

ummm u ok?

Explanation:

Answer:

a.

Explanation:

electromagnetism

Answer:

36.16 amu

Explanation:

From the question given above, the following data were obtained:

1st Isotope:

Mass of 1st isotope = 35.01 amu

Abundance of 1st isotope = 35%

2nd isotope:

Mass of 2nd isotope = 36.01 amu

Abundance of 2nd isotope = 15%

3rd isotope:

Mass of 3rd isotope = 37.02 amu

Abundance of 3rd isotope = 50%

Atomic mass of element A =?

The atomic mass of element A can be obtained as follow:

Atomic mass = [(mass of 1st × Abundance)/100] + [(mass of 2nd × Abundance)/100] + [(mass of 3rd × Abundance)/100]

= [(35.01 × 35)/100] + [(36.01 × 15)/100] + [(37.02 × 50)/100]

= 12.25 + 5.40 + 18.51

= 36.16 amu

Thus, the atomic mass of element A is 36.16 amu

Answer:

226.9 J·kg⁻¹·°C⁻¹

Explanation:

The specific heat of a substance can be defined as the amount is heat that has to be added in order for a given mass of the substance to increase its temperature:

In this case:

We input the data:

And calculate c:

Answer:

1. 3.83 L

2. 0.368 mole

Explanation:

1. Determination of the volume

Pressure (P) = 3.21 atm

Temperature (T) = 202 K

Number of mole (n) = 0.741 mole

Gas constant (R) = 0.0821 L.atm/molK

Volume (V) =?

The volume can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

3.21 × V = 0.741 × 0.0821 × 202

3.21 × V = 12.3497283

Divide both side by 3.21

V = 12.2888922 / 3.21

V = 3.83 L

Thus, the volume of the gas is 3.83 L

2. Determination of the number of mole.

Pressure (P) = 2.50 atm

Temperature (T) = 215 K

Volume (V) = 2.60 L

Gas constant (R) = 0.0821 L.atm/molK

Number of mole (n) =?

The number of mole can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

2.50 × 2.60 = n × 0.0821 × 215

6.5 = n × 17.6515

Divide both side by 17.6515

n = 6.5 / 17.6515

n = 0.368 mole

Thus, the number of mole of the gas is 0.368 mole.

Answer:

Option B: p H equals 2.00 , because the molar concentration of H with a positive 1 charge equals 1.0 times 10 to the negative 2 power molar .

pH = 2 because [H⁺] = 1×10¯² M

Explanation:

To know which option is correct, we shall determine the pH of the 0.010 M HClO₄ solution. This can be obtained as follow:

We'll begin by calculating the concentration of the hydrogen ion [H⁺] in the solution. This is illustrated below:

HClO₄ is a strong acid and will dessociates as follow:

HClO₄ (aq) —> H⁺ (aq) + ClO₄¯ (aq)

From the balanced equation above,

1 mole of HClO₄ produced 1 mole H⁺.

Therefore, 0.010 M HClO₄ will also produce 0.010 M H⁺.

Finally we shall determine the pH of the solution. This can be obtained as follow:

Concentration of the hydrogen ion [H⁺] = 0.010 = 1×10¯² M

pH =?

pH = –Log [H⁺]

pH = –Log 1×10¯²

pH = 2

Thus,

The pH = 2

because,

[H⁺] = 1×10¯² M

Thus, option B gives the correct answer to the question.

Based on the definition of pH, pH of 0.010 M solution of HClO4 equals 2.00, because the molar concentration of H with a positive 1 charge equals 1.0 times 10 to the negative 2 power molar.

The pH of a solution is the negative logarithm of the hydrogen ion concentration of a solution.

pH of a solution is a measure of the acidity of the solution.

where

For the 0.010 M solution of HClO4, [H+} = 0.01 M

pH = -log(0.01)

pH = 2.00

Therefore,  pH of 0.010 M solution of HClO4 equals 2.00, because the molar concentration of H with a positive 1 charge equals 1.0 times 10 to the negative 2 power molar.

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The concept molar mass is used here to determine the compound which has the greatest mass for its one mole. The correct option is C.

The molar mass also defined as the molecular weight of a compound is generally the sum of the atomic masses of each atoms present in the given compound. Its unit is g mol⁻¹.

The mass of 1 mole of any substance is also called the molar mass. Evidently molar mass is equal to the atomic mass or the molecular mass denoted in grams depending upon whether the substance contains atoms or molecules.

Here (SiHA) is known as the most important bioceramic which is used in the field of bioactive bone implants. The compound CO is carbon monoxide, CH₃OH is methanol and C₂H₆ is ethane.

The molar mass of the given compounds are obtained by adding their atomic masses :

CO = (12.011 g/mol+ 15.999 g/mol) = 28.01 g/mol

CH₃OH = (12.011 g/mol + 3 × 1.007 g/mol + 15.999 g/mol + 1.007 g/mol) = 32.04 g/mol

C₂H₆ = (2 × 12.011 g/mol + 6 ×  1.007 g/mol) = 30.07 g/mol

Here among the given compounds CH₃OH has the greatest mass for one mole of the compound.

Thus the correct option is C - CH₃OH.

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Answer:

79.1g of weak base must be combined with 56.0g of conjugate acid

Explanation:

that is 1.00 M in the weak base?

The weak base is C5H5N with a pKa of 5.17 (Ka=6.7×10-6)and a desire pH of 5.63

The equilibrium of the weak base is with the bromide salt of the conjugate acid is:

C5H5N(aq) + H2O(l) + Br- ⇄ C5H5NHBr(aq) + OH-(aq)

Where Kb = Kw / Ka = 1x10⁻¹⁴ / 6.7x10⁻⁶

Kb = 1.49x10⁻⁹ is defined as:

Kb = 1.49x10⁻⁹ = [C5H5NHBr] [OH-] / [C5H5N]

Where [OH-] = 10^-(14- pH) = 10^-(14- 5.63) = 4.255x10⁻⁹M

[C5H5N] = 1.00M

Replacing:

1.49x10⁻⁹ = [C5H5NHBr] [OH-] / [C5H5N]

1.49x10⁻⁹ = [C5H5NHBr] [4.255x10⁻⁹M] / [1.00M]

[C5H5NHBr] = 0.35M

In 1L the moles of C5H5NHBr are 0.35 moles

Mass C5H5NHBr: 160.0118g/mol

0.35 moles * (160.0118g / mol) =

56.0g of C5H5NHBr are necessaries

The mass of C5H5N is -79.1g/mol-:

1.00moles * (79.1g/mol) =

Answer: Limitations to population growth are either density-dependant or density-independent. Density-dependent factors include disease, competition, and predation. Density-dependant factors can have either a positive or a negative correlation to population size.

Explanation:

Answer:

Can you translate it on English so we can understand

Answer:

C. Base.

Explanation:

Hello there!

In this case, according to the given information, it turns out convenient for us to realize that the concept acid and base we should use here is based off the Bronsted-Lowry one, which says that an acid is a hydrogen donor. In such a way, since water accepts one H ion as it goes to H3O⁺, we infer it is C. Base and the H2S the acid.

Also, we can tell HS⁻ is the conjugate base and H3O⁺ the conjugate acid.

Regards!

Answer:

magnetism of water

Explanation:

Not sure

Answer:

27.98g/mol

Explanation:

Using ideal gas law equation;

PV = nRT

Where;

P = pressure (atm)

V = volume (L)

T = temperature (K)

n = number of moles (mol)

R = gas law constant (0.0821 Latm/molK)

According to the information given:

V = 2.5L

P = 1.4 atm

T = 282K

n = ?

Using PV = nRT

n = PV/RT

n = 1.4 × 2.5/0.0821 × 282

n = 3.5/23.1522

n = 0.151mol

Using the formula to calculate molar mass of the elemental gas:

mole = mass/molar mass

Molar mass = mass/mole

Molar mass = 4.23g ÷ 0.151mol

Molar mass = 27.98g/mol

Answer:

The answers are in the explanation.

Explanation:

The energy required to convert 10g of ice at -10°C to water vapor at 120°C is obtained per stages as follows:

Increasing temperature of ice from -10°C - 0°C:

Q = S*ΔT*m

Q is energy, S specific heat of ice = 2.06J/g°C, ΔT is change in temperature = 0°C - -10°C = 10°C and m is mass of ice = 10g

Q = 2.06J/g°C*10°C*10g

Q = 206J

Change from solid to liquid:

The heat of fusion of water is 333.55J/g. That means 1g of ice requires 333.55J to be converted in liquid. 10g requires:

Q = 333.55J/g*10g

Q = 3335.5J

Increasing temperature of liquid water from 0°C - 100°C:

Q = S*ΔT*m

Q is energy, S specific heat of ice = 4.18J/g°C, ΔT is change in temperature = 100°C - 0°C = 100°C and m is mass of water = 10g

Q = 4.18J/g°C*100°C*10g

Q = 4180J

Change from liquid to gas:

The heat of vaporization of water is 2260J/g. That means 1g of liquid water requires 2260J to be converted in gas. 10g requires:

Q = 2260J/g*10g

Q = 22600J

Increasing temperature of gas water from 100°C - 120°C:

Q = S*ΔT*m

Q is energy, S specific heat of gaseous water = 1.87J/g°C, ΔT is change in temperature = 20°C and m is mass of water = 10g

Q = 1.87J/g°C*20°C*10g

Q = 374J

Total Energy:

206J + 3335.5 J + 4180J + 22600J + 374J =

30695.5J =

30.7kJ

Answer:

Molarity = 0.06 mol/L

Molality = 0.063

Explanation:

Complete question

A student dissolves 1.5g of styrene C8H8 in 225.mL of a solvent with a density of 1.02/gmL . The student notices that the volume of the solvent does not change when the styrene dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits

Solution

We must to know:

Molarity is equal to no. of moles divided by volume of solution

No. of moles = Mass/Molecular Mass

No. of moles of C8H8 = 1.5/104 = 0.0144

Molarity = 0.0144/225 = 0.06 mol/L

Molality = no. of moles / mass of solvent  

Substituting the given values, we get -  

Density = mass / V  

Mass = density  x V

1.02 * 225  

= 229.5 g  

Molality = 0.0144 / 229.5  

0.063

Answer:

I am really sorry but i really don't no

Answer:

our equation specifies that

32

⋅

g

of dioxygen and

4

⋅

g

of dihydrogen give

36

⋅

g

of water upon reaction, so..........

Explanation:

2

H

2

(

g

)

+

O

2

(

g

)

→

2

H

2

O

(

g

)

We started with

5.0

⋅

g

32.00

⋅

g

⋅

m

o

l

−

1

=

0.156

⋅

m

o

l

dioxygen

.

Given excess dihydrogen, this molar quantity thus gives

2

×

0.156

⋅

m

o

l

water.

And thus,

2

×

0.156

⋅

m

o

l

×

18.01

⋅

g

⋅

m

o

l

−

1

≅

6

⋅

g

water are evolved. Is this reaction exothermic or endothermic?

Answer:

The gases in a hair spray can are at a temperature of 26.0 °C and a pressure of 25.0 lbs/in2.

If the pressure becomes [tex]90.0lbs/in^{2}[/tex], what is the temperature of the gases?

Explanation:

According to Gay lussac's law:

the pressure of a gas is directly proportional to its absolute temperature.

[tex]P\alpha T[/tex]

[tex]\frac{P{1} }{T{1} }=\frac{P{2} }{T{2} }[/tex]

Given,

[tex]P1=25.0lbs/in^{2} \\P2=90.0lbs/in^{2} \\T1=26^{o} C=(26+273)K=299K\\T2=?[/tex]

Substitute these values in the above formula:

[tex]\frac{P{1} }{T{1} }=\frac{P{2} }{T{2} }\\\\\frac{25lbs/in^{2} }{299K} }=\frac{90.0lbs/in^{2} }{T{2} }\\\\\\On simplification \\T2=1076.4K\\T2=(1076.4-273)^{o} C=803.4^{o} C[/tex]

Answer:

The gases will be raised to a temperature of 803.4[tex]^{o} C[/tex].

Answer:

Metal oxide + acid —> salt + water

Explanation: