# Boron Trifluoride Molar Mass - BRAINGITH (2023)

molar mass of boron trifluoride​

Table od Content

## 1. molar mass of boron trifluoride​

molar mass = 67.81 g

Explanation:

The chemical formula of boron trifluoride is B F₃

molar mass = (10.8110 g × 1) + (18.9984 g × 3)

molar mass = 67.81 g

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## 2. ammonia is polar molecule while boron trifluoride is a nonpolar molecule

The Statement is TRUE

Boron trifluoride is a non-polar molecule, whereas ammonia is a polar molecule.

## 3. ammonia is polar molecule while boron trifluoride is a nonpolar molecule explain the difference

Explanation:

Sori hindi ko masend kase may rude words daw

## 4. Make a rap about Molar mass and Calculating Molar mass​

The molar mass is the mass of a given chemical element or chemical compound. divided by the amount of substance

Molar mass is the mass in grams of 1 mole of the substance, you can find it by summing the standard atomic masses of its component atoms.

Hope this helps!

## 5. 1. What is the average atomic mass of Ca? What is the molar mass of Ca?2. The atomic mass of Br is 79.90 amu. What is its molar mass?3. The molecular mass of water, H2O, is 18.02 amu. What is the molar mass of water, H2O?4. The formula mass of NaCl is 58.44 amu. What is the molar mass of NaCl?

$${\huge{\boxed{{{Question}}}}}$$

1. What is the average atomic mass of Ca? What is the molar mass of Ca?

2. The atomic mass of Br is 79.90 amu. What is its molar mass?

3. The molecular mass of water, H2O, is 18.02 amu. What is the molar mass of water, H2O?

4. The formula mass of NaCl is 58.44 amu. What is the molar mass of NaCl?

$${\huge{\boxed{{{Answer}}}}}$$

1. What is the average atomic mass of Ca?

What is the molar mass of Ca?

Calcium

CalciumAtomic mass

40.078 u

2. The atomic mass of Br is 79.90 amu. What is its molar mass?

Calculate the atomic mass of gallium. 3. Bromine has two naturally occurring isotopes (Br-79 and Br-81) and an atomic mass of 79.904 amu.

3. The molecular mass of water, H2O, is 18.02 amu. What is the molar mass of water, H2O?

Water

Water Molar mass

18.01528 g/mol

4. The formula mass of NaCl is 58.44 amu. What is the molar mass of NaCl?

Sodium chloride

Sodium chloride Molar mass

58.44 g/mol

$${\huge{\boxed{{{Explanation}}}}}$$

How do you find the molar mass of CA?

Solution:

Solution:Formula =Ca(NO3)2.

Molar mass Ca=40.08g/mol.

Molar mass N=14.01g/mol.

Molar mass O=16.00g/mol.

How do I find molar mass?

The molar mass is the mass of a given chemical element or chemical compound (g) divided by the amount of substance (mol). The molar mass of a compound can be calculated by adding the standard atomic masses (in g/mol) of the constituent atoms.

However, molar mass can also be calculated by multiplying the atomic mass in amu by the molar mass constant (1 g/mol). To calculate the molar mass of a compound with multiple atoms, sum all the atomic mass of the constituent atoms.

Water:

Formula: H₂O

Density: 997 kg/m³

Molar mass: 18.01528 g/mol

Boiling point: 100 °C

Melting point: 0 °C

IUPAC ID: Oxidane, Water

What is the mass of a mole of NaCl called?

The molar mass of sodium chloride is 58.44 g/mol.

One mol of NaCl (6.02 x1023 formulas) has a mass of 58.44 g.

____________________________________

How do you find the molar mass of CA?

https://chem.libretexts.org

How do I find molar mass?

https://courses.lumenlearning.com

Water:

https://www.britannica.com/science

What is the mass of a mole of NaCl called?

https://uh.edu/~chem1p/c3/C3F99.pdf

$${\huge{\boxed{{{-Roseann}}}}}$$

Note: This is not mine, I have credits to the owner.

Judge it if it's not correct ❤️

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## 6. What is the mass number of boron-10?​

Boron-10 atom is a stable isotope of boron with relative atomic mass 10.0129370, 19.9 atom percent natural abundance and nuclear spin 3+.

10.0129370

Boron-10 atom is a stable isotope of boron with relative atomic mass 10.0129370, 19.9 atom percent natural abundance and nuclear spin 3+.

Explanation:

## 7. Naturally occurring boron has two stable isotopes. It contains 20% boron-10 and 80% boron-11, themasses of which are 79 and 81 amu, respectively. What is the atomic mass of boron?​

Strategy:

Each isotope contributes to the average atomic mass based on its relative abundance. Multiplying the mass of an isotope by its fractional abundance (not percent) will give the contribution to the average atomic mass of that particular isotope.

Solution:

First, the percents are converted to fractions: 20 percent to 20/100 or 0.20 and 80 percent to 80/100 or 0.80. We find the contribution to the average atomic mass for each isotope, then add the contributions together to obtain the average atomic mass.

(0.20)(10 amu) + (0.80)(11 amu) = 10.8 amu

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## 9. claculate the molar mass of water.the molar mass of oxygen=16.00 x 1=16/molethe molar mass of hydrogen=1.01 x 2=2.0g/mole

MOLAR MASS

Calculate the molar mass of water.

The chemical formula of water is H₂O

Molar Mass of Oxygen = 16 g/mol

16 • 1 = 16 g

Molar Mass of Hydrogen = 1.01 g/mol

1.01 • 2 = 2.0 g

Molar Mass of H₂O = molar mass O + molar mass H₂

Molar Mass of H₂O = 16 g + 2.0 g

Molar Mass of H₂O = 18 g/mol

$$\:$$

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B po ang sagoyt

sana nakatulong

## 11. claculate the molar mass of water.the molar mass of oxygen=16.00 x 1=16/molethe molar mass of hydrogen=1.01 x 2=2.0g/mole

MOLAR MASS

Calculate the molar mass of water.

The chemical formula of water is H₂O

Molar Mass of Oxygen = 16 g/mol

16 • 1 = 16 g

Molar Mass of Hydrogen = 1.01 g/mol

1.01 • 2 = 2.0 g

Molar Mass of H₂O = molar mass O + molar mass H₂

Molar Mass of H₂O = 16 g + 2.0 g

Molar Mass of H₂O = 18 g/mol

$$\:$$

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## 12. mass of water and molar mass​

mass of water: 18.01528 g/mol

Density: 997 kg/m³

Boiling point: 100 °C

Formula: H2O

Melting point: 0 °C

Molar mass: 18.01528 g/mol

IUPAC ID: Oxidane, Water

## 13. You have 207 mL of chlorine trifluoride (ClF3) gas at 0.919 atm and 45°C. What is the mass (in grams) of the sample?Molar mass: Cl = 35.45 g/mol ; F = 19 g/mol

3.41g

The mass

C

l

F

3

in the sample is 3.41 g.

Explanation:

To solve this problem, we need to use the ideal gas law:

P

V

=

n

R

T

P

is pressure in atmospheres,

V

is volume in liters,

n

is moles,

R

is the universal gas constant, and

T

is the temperature in Kelvins.

First, we will need to convert each of the units.

894

l

÷

1000

=

0.894

l

L

772

l

m

m

H

g

1

×

1

l

a

t

m

760

l

m

m

H

g

=

1.02

atm

28

+

273

=

301

l

K

Now, plug the above values into the equation and solve for moles.

(

1.02

)

(

0.894

)

=

(

n

)

(

0.08206

)

(

301

)

n

=

(

1.02

)

(

0.894

)

(

0.08206

)

(

301

)

=

0.0369

l

m

o

l

l

C

l

F

3

Finally convert moles of

C

l

F

3

to grams:

0.0369

l

m

o

l

l

C

l

F

3

1

×

92.448

l

g

l

C

l

F

3

1

l

m

o

l

l

C

l

F

3

=

3.41

l

g

l

C

l

F

3

## 14. what is a molar mass? How is the molar mass of a substance calculated ​

The molar mass of a substance is the mass in grams of 1 mole of the substance. As shown in this video, we can obtain a substance's molar mass by summing the molar masses of its component atoms. We can then use the calculated molar mass to convert between mass and number of moles of the substance.

Explanation:

## 16. ammonia is polar molecule while boron trifluoride is a nonpolar molecule explain the difference in polarity of this compound​

boron trifluoride has no hydrogen bonding, while nonpolar molecule doesboron trifluoride is a triangular planar, while nonpolar molecule is pyramidalboron trifluoride is a Lewis base, while nonpolar molecule is a Lewis acid.boron trifluoride the( B-F bond) polar than nonpolar molecule ( N-H bond).Boron is electronegative than nitrogen.

.

## 17. You have 207 mL of chlorine trifluoride (ClF3) gas at 0.919 atm and 45°C. What is the mass (in grams) of the sample?Molar mass: Cl = 35.45 g/mol ; F = 19 g/mol

The mass of the sample of $$ClF_{3}$$ gas is 0.674 g.

Explanation:

In this problem, we assume it is an ideal gas. With that, we use the Ideal Gas Law expressed as PV = nRT. Take note that the units must be consistent to a reference, usually the universal gas constant, R. It's up to you what value to use, but it would be favorable to use R = 0.0821 L atm/mol K considering the units of the volume, the pressure, and the molar mass are within the SI Units.

Given: V = 207 mL; P = 0.919 atm; T = 45 deg C;

MM, Cl = 35.45 g/mol; MM, F = 19 g/mol

To achieve consistency, we do the necessary conversions:

V = 207 mL $$(\frac{1 L}{1000mL})$$ = 0.207 L

T = 45 + 273 = 318 K

MM, $$ClF_{3}$$ = 35.45 g/mol + (3)(19 g/mol) = 92.45 g/mol

We can modify the equation above by expressing the number of moles, n, in terms of the relationship between MM and mass, where n = m/MM

PV = $$\frac{m}{MM} RT$$

$$m=\frac{PVMM}{RT} \\m=\frac{(0.919 atm)(0.207L)(92.45g/mol)}{(0.0821 \frac{Latm}{mol K)}(318K) } \\m=0.674 g$$

## 18. What is the molarity of a solution of 10% by mass cadmium sulfate, cdso4 (molar mass?

208.46 g/mol) by mass? The density of the solution is 1.10 g/mL.

Explanation:

## 19. . Which of the following statement is NOT true about molar mass? A. Molar mass can be determined without considering the molar masses of the individual elements. B. The molar mass of a substance is the sum of the atomic mass of all atoms indicated in the formula of a substance. C. The number of grams in the molar mass of an element is not the same as the atomic number. D. When calculating molar mass of a chemical compound, it states how many grams are in one mole of a substances​

Which of the following statement is NOT true about molar mass? A. Molar mass can be determined without considering the molar masses of the individual elements. B. The molar mass of a substance is the sum of the atomic mass of all atoms indicated in the formula of a substance. C. The number of grams in the molar mass of an element is not the same as the atomic number. D. When calculating molar mass of a chemical compound, it states how many grams are in one mole of a substances

## 20. Boron (B,Z=5) has to naturally occurring isotopes. find the percent abundances of boron-10. and boron-11 given these data: aromatic mass of B=10.81 amu, isotopic mass of boron-10=10.0129 amu, and isotopic mass of boron-11=11.0093 amu. (Hint:The sum of the fractional abundances is 1. if x=abundance of boron-10, then 1-x=abundance of boron-11.​

trip ko lang thx sa point

## 21. 1.mass of carbon + mass of carbon=2.mass of boron+mass of boron=​

1. 24.022

mass of carbon-12.011

2.21.6

mass of boron-10.8

## 22. Compute for the molar mass of CuSAnswer:Compute for the molar mass of Lanthanum Answer:Compute for the molar mass of Ytterbium Answer:​

Explanation:

compute the money cuins

10.811u ± 0.007u

yan po

## 24. Molar mass (g/mol) what is the molar mass of calcium​

40.078 u

Atomic number: 20

Symbol: Ca

## 25. SERIOUS ANSWER PO PLEASE!Boron has two isotopes, Boron-10 and Boron-11, whose percentage abundances are 19.8% and 80.2% respectively. The atomic masses of Boron-10 and Boron-11 are 10.0129 amu and 11.0093 amu respectively. Write the symbols for the two isotopes of boron and determine the relative atomic mass.

where:

atomic mass = average atomic mass of the element

f.a. = fractional abundance of the isotope.

To get f.a., we simply need to divide the given percent abundance by 100.

We’re given the following values:

Average Atomic Mass = 10.811 amu

Boron-10: Mass = 10.012938 amu

Boron-11: Mass = 11.009305 amu

The atomic masses of Boron-10 and Boron-11 are 10.012938 and 11.009305 amu, respectively. The average atomic mass of boron is 10.811 amu. Calculate the natural abundances of these two isotopes

Explanation:

sana maka tulong pls mark me as a brainliea

## 26. A sample of a compound containing boron (B) and hydrogen (H) contains 6.444 g of B and 1.803g of H. The molar mass of the compound is about 30 g. What is its molecular formula?

The molecular formula of the compound is BH3.

Explanation:

In order to solve for the molecular formula, we need to know the molar mass of the compound and the masses of the elements in the compound. We can then use the mole ratio to calculate the number of molecules in the compound.

The molar mass of the compound is about 30 g. The masses of the elements in the compound are 6.444 g of B and 1.803 g of H. The mole ratio is therefore B:H = 6.444:1.803 = 3.6. This means that there are 3.6 molecules of B in every molecule of BH3.

## 27. 5. How can we determine the number of moles of a givensubstance?a. Add the mass of the c. Multiply the mass of thesubstance by its atomic substance by its atomicmass and molar massmass and molar massb. Subtract the mass of the d. Divide the mass of thesubstance by its atomic substance by its atomicmass and molar massmass and molar mass​

D

Explanation:

sana po makatulong

paki follow narin po salamat po

## 28. 4. To obtain the molar mass of a compound, its formula is expressas:a. molar mass = number of atoms + atomic mass of elements.b. molar mass = number of atoms x atomic mass of elements.c. molar mass = number of atoms / atomic mass of elements,d. molar mass = number of atoms - atomic mass of elements.​

B. molar mass = number of atoms x atomic mass of elements

Explanation:

## 29. explain why boron trifluoride is a stronger lewis acid than trimethyl borate​

yes po

Explanation:

uhm sa tingin daw po ni papa satanas

## 30. mass number of boron-11?​

________________________________

$$\huge\sf\red{{Answer:}}$$

11.009306

Boron-11 isthe stable isotope of boron with relative atomic mass 11.009306, 80.1 atom percent natural abundance and nuclear spin 3/2. Boron-10, an isotope of boron, is used as a neutron absorber in BORON NEUTRON CAPTURE THERAPY.

________________________________

correct me if i'm wrong

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