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Lubov Fominskaja [6]
3 years ago
7

A sample is decomposed in the laboratory and found that it contains 52.2% carbon (C), 13.0% hydrogen (H), and 34.8% oxygen (O).

What is the empirical formula of this compound?
Chemistry
1 answer:
Andrej [43]3 years ago
7 0
The empirical formula would be C2H6O
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What is the predominant intermolecular force in the liquid state of each of these compounds: ammonia (NH3), methane (CH4), and n
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Answer:

The  predominant intermolecular force in the liquid state of each of these compounds:

ammonia (NH3)

methane (CH4)

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1.Hydrogen bonding: It is a weak electrostatic force of attraction that exists between the hydrogen atom and a highly electronegative atom like N,O,F.

2.Dipole-dipole interactions: They exist between the oppositely charged dipoles in a polar covalent molecule.

3. London dispersion forces exist between all the atoms and molecules.

NH3 ammonia consists of intermolecular H-bonding.

Methane has London dispersion forces.

Because both carbon and hydrogen has almost similar electronegativity values.

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3 0
3 years ago
calculate the number of moles of gas that occupy a 3.45L container at a pressure of 1.48 atm and a temperature of 45.6 Celsius ​
Otrada [13]

Answer:

There are 0,2 moles of gas that ocuppy the container.

Explanation:

We apply the formula of the ideal gases, we clear n (number of moles); we use the ideal gas constant R = 0.082 l atm / K mol. Firs we convert the unit of temperature in Celsius into Kelvin:

0°C= 273 K ------> 45,6 °C= 273 + 45, 6= 318, 6 K

PV= nRT ---> n= PV/RT

n= 1,48 atm x 3,45 L /0.082 l atm / K mol x 318,6 K

n= 0,195443479 mol

8 0
3 years ago
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