<u>Answer:</u>
<em>The energy to turn the ice into water:</em>
- The energy that is required to change the state of ice into a liquid is obtained in the form of heat energy from the ambient temperature of the warm room.
- Once this heat energy is absorbed, the individual molecules of ice gain kinetic energy and start vibrating faster.
- Yet, the temperature of the ice remains constant until the ice reaches its melting point because this energy is first utilised to break all the bonds of the lattice structure of the ice.
- After all the bonds are broken and all of the ice has changed into water, if more heat is provided again, then the temperature of the water will increase.
Answer:
Under high temperatures and low pressure, gases behave the most ideal.
Explanation:
Low pressure reduces the effect of the finite size of real particles by increasing the volume around each particle, and a high temperature gives enough kinetic energy to the particles to better overcome the attractions that exist between real particles. (Prevents sticking.)
In summary, real gases behave more like ideal gases when they are far away from a phase boundary, (condensation or freezing).
<span>Gather your materials. Gather the sand, salt and iron filing mixture; a magnet; a paper towel; a cup of warm water; an empty cup; and a piece of filter paper.Use the magnet to remove the iron. ...Use warm water to dissolve the salt. ...<span>Remove the sand from the salt water.</span></span>
The molecular formula shows the number of atoms present. The molecular formula of the gas is most likely ClO2.
In terms of gas density and molar mass, the ideal gas equation can be written in the form; PM = dRT
Where;
P = pressure of the gas
M = molar mass of the gas
d = density of the gas
R = molar gas constant
T = temperature of the gas
Making the molar mass of the gas the subject of the formula;
M = dRT/P
d = 2.875 g/L
R = 0.082 atmLmol-1K-1
T = 11°C + 273 = 284 K
P = 750.0 mm Hg or 0.99 atm
Substituting values;
M = 2.875 g/L × 0.082 atmLmol-1K-1 × 284 K/ 0.99 atm
M = 67.6 g/mol
The gas is most likely ClO2.
Learn more: brainly.com/question/11969651
Answer:
The mass of N a H C O 3 present is 2.431 g
Explanation:
The sample contains 57.2 % N a H C O 3 by mass.
To find the mass of N a H C O 3 in the sample, we need to find what the equivalent of 57.2 %.
Mass of N a H C O 3 = Percentage Composition * Mass of sample
Mass of N a H C O 3 = 57.2 / 100 * 4.25
Mass of N a H C O 3 = 2.431 g
The mass of N a H C O 3 present is 2.431 g
