All categories

3 years ago

5F248+ 2NH3(8) ► NF418 + 6HF

Chemistry

1 answer:

mylen [45]3 years ago

6 0

Answer:

14.2L at STP

Explanation:

Based on the problem, 2 moles of NH3 produce 6 moles of HF. To solve this question we have to convert the mass of NH3 to moles. With the chemical equation find the moles of HF and using PV = nRT find the liters of HF:

Moles NH3 -Molar mass: 17.031g/mol-

3.6g NH3 * (1mol / 17.031g) = 0.211 moles NH3

Moles HF:

0.211 moles NH3 * (6mol HF / 2mol NH3) = 0.634 moles HF

Volume HF

PV = nRT; V = nRT/P

Where V is volume in liters, n are moles of the gas = 0.634 moles, R is gas constant = 0.082atmL/molK, T is absolute temperature = 273.15K at STP and P is pressure = 1atm at STP.

Replacing:

V = 0.634moles*0.082atmL/molK*273.15K / 1atm

V = 14.2L at STP

You might be interested in

Janice looked out the window. Her yard still had snow on it. Snow on the yard across the street had melted. Why did Janice’s yar

atroni [7]

Janice’s yard was probably not exposed to as much sun and heat as the yard across the street

4 0

4 years ago

Read 2 more answers

Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two rea

Oksi-84 [34.3K]

Answer:

Explanation:

To find the theoretical yield of the equation. First identify the limiting reactant in a chemical equation.

Step 1: write out the equation and balance it.

Al+ 3mno2=3mn+ 2Alo3.

The limiting reactant is mn02 because it is not found in excess.

Step 2: convert the % to gram . All contain 67.2% mole and mno2 will be 100-67.2= 32.8

All=67.2÷100×290(total gram of the reactants)=194.88g

Mno2=32.8÷100×290g=94.12g.

Step 3:calculate the molar mass of mno2 and that of mn. The atomic mass of mn is 54.9380 and that of oxygen is 16.

Mno2=54.938+ (16)2=86.98g/mol.

Mn=54.938.

Step 4:

From your balanced equation , calculate mn.

94.12g mno2× (1mol mno2÷86.98(molarmass) of mno2×3 mol of mn/4molAl×54.938g of mn÷1mol of mn.

94.12g×1÷86.98g×3÷4×54.938÷1

=44.58g

6 0

3 years ago

When 6.040 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.95 grams of CO2 and 7.759 grams of H

algol [13]

Answer: The empirical formula is $CH_2$ and molecular formula is $C_4H_8$

Explanation:

We are given:

Mass of $CO_2$ = 18.95 g

Mass of $H_2O$ = 7.759 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 18.59 g of carbon dioxide, = $\frac{12}{44}\times 18.59=5.07g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 7.759 g of water, = $\frac{2}{18}\times 7.759=0.862g$ of hydrogen will be contained.

Mass of C = 5.07 g

Mass of H = 0.862 g

Step 1 : convert given masses into moles.

Moles of C = $\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{5.07g}{12g/mole}=0.422moles$

Moles of H= $\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.862g}{1g/mole}=0.862moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = $\frac{0.422}{0.422}=1$

For H = $\frac{0.862}{0.422}=2$

The ratio of C : H = 1: 2

Hence the empirical formula is $CH_2$ .

The empirical weight of $CH_2$ = 1(12)+2(1)= 14 g.

The molecular weight = 56.1 g/mole

Now we have to calculate the molecular formula.

$n=\frac{\text{Molecular weight }}{\text{Equivalent weight}}=\frac{56.1}{14}=4$

The molecular formula will be= $4\times CH_2=C_4H_8$

6 0

3 years ago

Which one of the following molecules is polar? Showallworkindetails. A) BH3 B) CCl4 C) SO2 D) CO2 E) PF5

Darya [45]

Answer:

C) SO₂

Explanation:

The figure below shows — clockwise from the upper left — BH₃, CCl₄, SO₂. CO₂, and PCl₅.

You must draw the Lewis structures of the molecules and then use VSEPR theory to figure out their molecular shape.

A) BH₃

BH₃ has a trigonal planar geometry.

It is nonpolar because of symmetry.

The bond dipole of the vertical B-H bond balances the equal and opposite resultant of the two downward-pointing B-H bonds.

BH₃ is nonpolar.

B) CCl₄

CCl₄ has a tetrahedral geometry.

The resultant of the two C-Cl bond dipoles on the right balances the equal and opposite resultant of the two C-Cl bond dipoles on the right.

CCl₄ is nonpolar.

C) SO₂

The Lewis structure shows that the central S atom has two S=O double bonds and a lone pair.

The electron pair geometry is trigonal planar and the molecular geometry is bent.

There is a net resultant of the S=O bond dipoles.

SO₂ is polar.

D) CO₂

CO₂ has a linear geometry with two C=O bonds pointing in opposite directions.

The bond dipoles cancel, so

CO₂ is nonpolar.

E) PCl₅

PCl₅ has a trigonal bipyramidal geometry.

The axial P-Cl bond dipoles cancel, as do the equatorial trigonal planar ones.

PCl₅ is nonpolar.

4 0

4 years ago

What is the correct answer

yanalaym [24]

A and D will increase the rate of solution of a salt in a water

3 0

3 years ago