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juin [17]
3 years ago
8

Explain hydrogen bonding.

Chemistry
1 answer:
denis23 [38]3 years ago
3 0

Answer:

Hydrogen bonding, interaction involving a hydrogen atom located between a pair of other atoms having a high affinity for electrons; such a bond is weaker than an ionic bond or covalent bond but stronger than van der Waals forces. Hydrogen bonds can exist between atoms in different molecules or in parts of the same molecule.

Explanation:

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A 10.00 g sample of a compound containing only carbon, hydrogen, and oxygen forms 23.98 g CO2 and 4.91 g H2O upon complete combu
yanalaym [24]
We can determine the empirical formula by first converting each of the grams to moles. remember to do this, first, we need the molar mass of the molecules which can be calculated by adding the mass of the atoms from the periodic table. 

molar mass of CO2= 44.0 g/mol
molar mass of H2O= 18.02 g/mol

now, lets determine the grams of each atom

Carbon: 23.98 g x (12.011 g / 44.01 g) = 6.54 g C

Hydrogen: 4.91 g x (2.0158 g / 18.02 g) = 0.55 g H

Oxygen: 10.0 - (6.54 + 0.55) = 2.91 g O

Now let's convert each mass to moles.

C: 6.54 g / 12.01 g / mol = 0.54 mol
H: 0.55 g / 1.01 g/mol = 0.54 mol
O: 2.91 g / 16.00 g/mol = 0.18 mol

now that we have the moles of each atom, we need to divide them by the smallest value to find the ration. If you do not get the whole number, you need to multiply until to get a whole number.

C:  0.54 mol / 0.18 mol = 3
H:  0.54 mol / 0.18 mol = 3
O: 0.18 mol / 0.18 mol = 1

empirical formula--> C₃H₃O



4 0
4 years ago
What is the total number of atoms in this formula?<br> NaHCO3
Pavel [41]
6 - one sodium atom, 1 hydrogen atom, 1 carbon atom, and 3 oxygen atoms.


7 0
4 years ago
A sample of a gas is occupying a 1500 ml container at a pressure of 3.4 atm and a temperature of 25 oc. if the temperature is in
Salsk061 [2.6K]

The new pressure will be 7.65 atm

<h3>General gas law</h3>

The problem is solved using the general gas equation:

P1V1/T1 = P2V2/T2

In this case, P1 = 3.4 atm, V1 = 1500 mL, T1 = 25 ^O C, V2 = 2000 mL, and T2 = 75  ^O C

What we are looking for is P2.

Thus, P2 = P1V1T2/T1V2

          = 3.4 x 1500 x 75/25 x 2000 = 382500/50000 = 7.65 atm

More on general gas laws can be found here: brainly.com/question/2542293

#SPJ1

7 0
2 years ago
How many grams of NaCl are required to make 150.0mL of a 5.000 m solution
Yanka [14]

The  number of  grams of NaCl  required  to make 150.0 ml of a 5.000m solution  is  43.875  grams


<u><em>calculation</em></u>

Step 1:  calculate  moles of NaCl

moles=  molarity x  volume in liters

volume in liters =  150.0  ml/1000= 0.15  l

moles is=  5.000mol/l  x0.15  l  =0.75  moles


Step2 :  find  mass

mass=  moles  x molar  mass

molar mass  of NaCl= 23 +35.5 = 58.5  g/mol

mass= 0.75  moles x58.5 g/mol = 43.875 grams

6 0
4 years ago
What kind of thermal energy transfer is illustrated in the diagram?
xxTIMURxx [149]

Answer:

I think radiaction

Explanation:

5 0
3 years ago
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