All categories

4 years ago

Which is the molar mass of BF3? 10.81 g/mol 29.81 g/mol 48.81 g/mol 67.81 g/mol

Chemistry

2 answers:

kondor19780726 [428]4 years ago

5 0

The molar mass of BF3 is 67.81 g/mol

<em><u> Explanation</u></em>

Molar mass is the mass of all atoms in a molecule in gram per mole.
molar mass of a molecule is calculated by adding atomic mass of constituent atom

use the periodic table to determine the atomic mass of each element in the molecule.

that is;

atomic mass of B = 10.81 g/mol

atomic mass of F = 19 g/mol

since there 3 atoms of F in BF3 the atomic massof F in BF3= 3 x19 = 57 g/mol

total molar mass of BF3 = 10.81 g/mol + 57 g/mol = 67.81 g/mol

LUCKY_DIMON [66]4 years ago

3 0

Answer:

The molar mass of BF3 is 67.81 g/mol

Explanation:

Molar mass is the mass of all atoms in a molecule in gram per mole. Use the periodic table to determine the atomic mass of each element in the molecule.

You might be interested in

For the following reactions, write a balanced equation using half-reactions and calculate the voltage to be expected.

Iteru [2.4K]

a) $2Na(s) +2H_2O(I)$ → $2Na^+(aq) + OH^-(aq)+ H_2(g)$

b) $2Ag (s) +2H^(aq)$ → $2 Ag^+ (aq) +H_2(g)$

<h3>What are half-reactions?</h3>

The half-reaction method is a way to balance redox reactions. It involves breaking the overall equation down into an oxidation part and a reduction part.

$2Na(s) +2H_2O(I)$ → $2Na^+(aq) + OH^-(aq)+ H_2(g)$

$E^0 cell = E^0 (reduction) - E^0 (oxidation)$

= $E^0(\frac{H_2O}{H_2}, OH^-) -E^0(Na^+/Na)$

= -0.83 - (-2.71) =1.88V

$2Ag (s) +2H^(aq)$ → $2 Ag^+ (aq) +H_2(g)$

$E^0cell$ = $E^0(H^+/H_2) -E^0(Ag^+/Ag)$

$E^0cell$ =-0. - (0.8) =-0.8V

Learn more about the half-reactions here:

https://brainly.in/question/18053421

#SPJ1

8 0

2 years ago

A sample of 325 mg of neon occupies 2 dm^3 at 20.0 c. use the perfect gas law to determine the pressure of the gas.

Musya8 [376]

Answer:

0.1935atm is the pressure of the gas.

Explanation:

In the problem you have the mass of Neon (You can obtain moles using molar mass), you have volume, and temperature. You can use general ideal gas law to solve pressure:

PV = nRT

P = nRT / V

<em>Where P is pressure in atm, n are moles, R is gas constant (0.082atmL/molK), T is absolute temperature (20.0°C + 273.15 = 293.15K), and V is volume in L = Volume in dm³</em>

<em />

<em>Moles gas:</em>

Molar mass Ne = 20.1797g/mol

0.325g * (1mol / 20.1797g) = 0.0161 moles

Replacing:

P = nRT / V

P = 0.0161 moles * 0.082atmL/molK * 293.15K / 2L

P = 0.1935atm is the pressure of the gas

7 0

3 years ago

How many grams of oxygen will react with 2.0 grams of iron II sulfide?

Elenna [48]

Answer:

How many grams Iron(II) Sulfide in 1 mol? The answer is 87.91. We assume you are converting between grams Iron(II) Sulfide and mole. You can view more details on each measurement unit: molecular weight of Iron(II) Sulfide or mol The molecular formula for Iron(II) Sulfide is FeS. The SI base unit for amount of substance is the mole.

Explanation:

3 0

3 years ago

What does gravity cause causes

frez [133]

What? do you mean what does gravity cause?

8 0

3 years ago

Read 2 more answers

At what temperature would a 1.30 m NaCl solution freeze, given that the van't Hoff factor for NaCl is 1.9? Kf for water is 1.86

Setler [38]

Answer:

-4.59°C

Explanation:

Let's see the formula for freezing point depression.

ΔT = Kf . m . i

ΔT = Freezing T° of pure solvent - Freezing T° of solution

Kf = Freezing constant. For water if 1.86°C/m

m = molality (moles of solute in 1kg of solvent)

i = Van't Hoff factor.

0°C - Freezing T° of solution = 1.86°C /m . 1.30m . 1.9

Freezing T° of solution = - (1.86°C /m . 1.30m . 1.9)

Freezing T° of solution = - (1.86°C/m . 1.30m . 1.9) → -4.59°C

NaCl → Na⁺ + Cl⁻

4 0

3 years ago