Answer:
water is denser
Explanation:
if you were to fill 2 55 gallon barrels of each product the water would weigh more because water is more dense
Answer:
table sugar: water
motor oil: gasoline
rubber from tire marks: gasoline
adhesive residue from a packing tape: gasoline
Explanation:
Like dissolves like so a polar compound will dissolve in a polar solvent and a non polar compound will dissolve in a non-polar solvent. The intermolecular forces of attraction are responsible for the dissolution of substances in different solvents.
For example, polar solute exhibit hydrogen bonding and dipole interaction with polar solvents (water). Non-polar solute exhibit London dispersion forces with non-polar solvents(gasoline).
Answer: a contest in which you are eliminated if you fail to spell a word correctly.
Answer: 2.93 L
Explanation:
AI-generated answer
To find the volume occupied by 0.108 mol of helium gas at a pressure of 0.909 atm and a temperature of 306 K, we can use the ideal gas law equation:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Rearranging the equation to solve for V:
V = (nRT) / P
Plugging in the given values:
n = 0.108 mol
R = 0.0821 L·atm/(mol·K) (the ideal gas constant)
T = 306 K
P = 0.909 atm
V = (0.108 mol * 0.0821 L·atm/(mol·K) * 306 K) / 0.909 atm
Calculating this expression, we find that the volume occupied by 0.108 mol of helium gas at a pressure of 0.909 atm and a temperature of 306 K is approximately 2.93 L.
Now, let's consider the second part of the question: Would the volume be different if the gas was argon (under the same conditions)?
The volume would be the same for argon gas.
According to the ideal gas law, at the same temperature, pressure, and number of moles, the volume occupied by a gas is the same regardless of the gas's identity. Therefore, if we replaced helium gas with argon gas while keeping the same conditions of pressure, temperature, and number of moles, the volume occupied by argon gas would be the same, approximately 2.93 L.
Intermolecular bonds become weaker
Freezing
Intermolecular bonds become stronger
Evaporation
Temperature increases
Vibration of molecules slows down
Molecules vibrate faster
Which of the above changes would be accompanied by an increase of the kinetic energy of particles in a liquid?
A, B, C, and H
A, C, D, and G
B, E, F, and H
B, C, F, and G
With an increase in the kinetic energy of the solid molecule the intermolecular bonds become weaker, temperature increases, melting and molecules vibrating faster are changes.
Kinetic energy is the form of the energy that is present in an entity in motion. When the kinetic energy is increased then the temperature of the particles increases and leads to evaporation.
The increased kinetic energy weakens the intermolecular bonds of the liquid particles and the molecules of the particles start vibrating fast.
Therefore, option b. intermolecular bonds become weak, option e. evaporation, option f. temperature increases and option h. molecules vibrate faster are the changes.
Learn more about kinetic energy here:
Final answer:
The changes that increase the kinetic energy of liquid particles are B, E, F, and H which correspond to evaporation, temperature increases, and molecules vibrating faster.
Explanation:
The changes that would be accompanied by an increase of the kinetic energy of particles in a liquid are evaporation, temperature increases, and molecules vibrate faster. During evaporation, molecules gain sufficient energy to overcome intermolecular forces and enter the gaseous phase. When the temperature increases, the average kinetic energy of the molecules increases, causing them to vibrate faster. Consequently, the correct answer is B, E, F, and H.
The changes that would be accompanied by an increase of the kinetic energy of particles in a liquid are B, E, F, and G.
When temperature increases, the average kinetic energy of the particles in a liquid also increases. This is represented by changes B and F. Evaporation (change E) also leads to an increase in the kinetic energy of the particles as they gain enough energy to escape into the vapor phase. Lastly, intermolecular bonds becoming weaker (change G) allows for more movement of the particles, increasing their kinetic energy.