All categories

4 years ago

Identify the structure as having hydrogen bonding, dipole-dipole moments or London dispersion forces (LDF).

1 answer:

8 0

A.) H2O - HYDROGEN BONDING ; Covalent Bond ; Polar

B.) NH3 - LDF ; Covalent Bond ; Non-polar

C.) CH4 - HYDROGEN BONDING ; Covalent Bond ; Polar
<span>
D.) CO2 - LDF ; Covalent Bond ; Non-polar

</span>

You might be interested in

Which of the following gases in Earth's atmosphere would you expect to find as molecules and which as individual atoms? Explain

azamat

Answer: argon

Explanation:

7 0

3 years ago

The solid rocket boosters for the space shuttle employ a mixture of aluminum and ammonium perchlorate (molar mass = 117 g/mol) a

Mnenie [13.5K]

Answer : The volume of gas at STP produced are 45.0 L

Explanation :

First we have to calculate the moles of ammonium perchlorate.

$\text{Moles of }NH_4ClO_4=\frac{\text{Mass of }NH_4ClO_4}{\text{Molar mass of }NH_4ClO_4}$

Molar mass of $NH_4ClO_4$ = 117 g/mole

$\text{Moles of }NH_4ClO_4=\frac{235g}{117g/mole}=2.01mole$

Now we have to calculate the moles of $NO$ gas produced during the reaction.

The balanced chemical reaction is,

$3Al(s)+3NH_4ClO_4(s)\rightarrow Al_2O_3(s)+AlCl_3(s)+3NO(g)+6H_2O(g)$

From the reaction we conclude that,

As, 3 moles of $NH_4ClO_4$ produces 3 moles of NO gas

So, 2.01 moles of $NH_4ClO_4$ produces 2.01 moles of NO gas

Now we have to calculate the volume of gas at STP.

At STP, 1 mole of substance occupy 22.4 L volume of gas.

As, 1 mole of NO gas occupy 22.4 L volume of gas.

So, 2.01 mole of NO gas occupy 2.01 × 22.4 L = 45.0 L volume of gas.

Therefore, the volume of gas at STP produced are 45.0 L

6 0

4 years ago

Definition <br> Nuclear Fusion

denis-greek [22]

Answer:

a nuclear reaction in which atomic nuclei of low atomic number fuse to form a heavier nucleus with the release of energy.

Explanation:

4 0

3 years ago

there are 3.0 x 10^22 molecules of sucrose in a sample. how many grams of sucrose is this? The molar mass of C12H22O11 is about

gladu [14]

The amount of sucrose in the sample would be 17 grams

<h3>Number of molecules of substances</h3>

There are 6.022 x $10^{23}$ molecules in 1 mole of every substance.

3.0 x $10^2^2$ molecules will, therefore, be:

1 x 3.0 x $10^2^2$ /6.022 x $10^{23}$ = 0.0498 moles

Mass of 0.0498 moles sucrose = 0.0498 x 342 = 17 grams

More on the number of molecules of substances can be found here: brainly.com/question/19481036

#SPJ1

5 0

2 years ago

Calculate pressure (at STP) in 10.0 L vessel after reaction of 1.0 L hydrochloric acid (concentration 35 % and density 1.28 g/cu

SCORPION-xisa [38]

Answer:

The pressure in the vessel is 13,3 atm.

Explanation:

2 HCl (aq)+ CaCO₃ (s) → CaCl₂(aq)+ H₂O(l)+ CO₂(g)

The increase in the pressure of the vessel after the reaction is by formation of a gas (CO₂). So we have to find the produced moles of this gas and apply the gas ideal law to find the pressure.

We have to find the limit reactant, to do so, we have to calculate the moles of each reactant in the reaction, the one that have the less moles will be the limit reactant:

HCl:

1,0L × (35/100) × (1000 cm³/1L) × (1,28 g/ 1cm³) × (1mol HCl/ 36,46 g) ÷ 2mol

<em>(Concentration) (L to cm³) (cm³ to g) (g to mol) (moles of reaction)</em>

moles of HCl= 6,14 mol

CaCo₃:

1,0 kg × (96/100) × (1000 g/1kg) × (1 mol/100,09g)

<em>(Limestone) (CaCo₃ in limestone) (kg to g) (g to mol) </em>

moles of CaCo₃= 9,59 mol

So, reactant limit is HCl

This reaction have a yield of 97%. So, the CO₂ moles are:

6,14 mol × 97÷ = 5,96 mol CO₂

The ideal gas formula to obtain pressure is:

P = nRT/V

Where: n = 5,96mol; R= 0,082 atm×L/mol×K; T = 273,15 (until STP conditions) and V= 10,0 L

Replacing this values in the equation the pressure is

P = 13,3 atm

I hope it helps!

7 0

3 years ago