Gas is a substance that will not phase change.
And vapor is a substance above it's boiling point temperature.
Answer:
209.3 Joules require to raise the temperature from 10 °C to 15 °C.
Explanation:
Specific heat capacity:
It is the amount of heat required to raise the temperature of one gram of substance by one degree.
Formula:
Q = m × c × ΔT
Given data:
mass of water = 10 g
initial temperature T1= 10 °C
final temperature T2= 15 °C
temperature change =ΔT= T2-T1 = 15°C - 10°C = 5 °C
Energy or joules added to increase the temperature Q = ?
Solution:
We know that specific heat of water is 4.186 J/g .°C
Q = m × c × ΔT
Q = 10 g × 4.186 J/g .°C × 5 °C
Q = 209.3 J
Answer:
<h2>Na^+ Cl^- > NaCl</h2>
Answer:
H2 < CH3Cl < HF
Explanation:
The intermolecular forces are the forces that bond the molecules together in a substance. There are three types of these forces:
- Dipole induced -dipole induced, or London dispersion -> Is the weakest and is presented in nonpolar molecules, in which a dipole is induced and so the molecules are joined together;
- Dipole-dipole -> Is stronger than the London dispersion and occurs in a polar molecule. In this case, the dipole already exists (partial positive and negative charges), so the poles are attracted;
- Hydrogen bond -> It's the strongest and is formed when the hydrogen is bonded with a higher electronegativity element (F, O, and N).
So, the molecule of H2 is linear and formed by the same element, so, is nonpolar, and has London dispersion forces. The molecule of CH3Cl has 3 nonpolar bonds (C-H), and one polar bond (C-Cl), so it's polar and has dipole-dipole forces. And the HF molecule has hydrogen bonds.
*A polar bond is a bond formed by elements with different electronegativities.
