Answer:
The following are the four unusual characteristics of water due to hydrogen bonding:
1. Water exhibits high specific heat as the presence of hydrogen bonds enhances the concentration of energy needed for the molecules to accelerate the speed, thus, elevating the specific heat.
2. Water has both high melting and high boiling points as hydrogen bonds enhance the energy, which is needed at the time of phase change, thus, increasing both the melting and the boiling points.
3. The hydrogen bonds present in the water gives rise to robust intermolecular attractions, therefore, enhancing the surface tension.
4. The hydrogen bonds present in the water makes the water to exhibit high heat of vaporization, that is, of about 41 KJ/mol.
Answer: D
Explanation:
Forces can be divided into those that act by direct contact—such as when you push on a door to open it—and those that act at a distance, where there is no apparent physical contact between the objects. Magnetism, and electrical charge, and gravitation are examples of forces that act at a distance.
<span>Neutral objects attract each other. [London dispersion forces]
Oppositely charged objects attract each other.
</span><span>Neutral objects and charged objects attract each other.</span>
Answer:
12 valence electrons
Explanation:
Number of valence electrons: 2 carbons (2 x 4 valence electrons= 8e-) and 4 hydrogens (4 x 1 valence electron = 4 e-) added up gives us 12 valence electrons to work with: Counting the bonds we have made shows that we have used up 10 of the 12 valence electrons leaving us with 2 to complete the octets.
Answer:
0.013 mole
Explanation:
Step 1:
Data obtained from the question. This includes:
Volume (V) = 250 mL
Pressure (P) = 1.3 atm
Temperature (T) = 33°C
Number of mole of (n) =?
Step 2:
Conversion to appropriate units.
The volume and the temperature given in the question must be converted to their appropriate unit in order to obtain the answer to the question in the right unit.
For volume:
We must, convert mL to L
1000 mL = 1 L
Therefore, 250 mL = 250/1000 = 0.25 L
For temperature:
We, must convert °C to K.
K = °C + 273
K = 33°C + 273
K = 306K
Step 3:
Determination of the number of mole of CO2.
Applying the ideal gas equation:
PV = nRT
The number of mole of CO2 can be obtained as follow:
V = 0.25 L
P = 1.3 atm
T = 306K
R (gas constant) = 0.082atm.L/Kmol
Number of mole of (n) =?
PV = nRT
1.3 x 0.25 = n x 0.082 x 306
Divide both side by 0.082 x 306
n = (1.3 x 0.25) /(0.082 x 306)
n = 0.013 mole