Answer:
2.0 atm is the difference between the ideal pressure and the real pressure.
Explanation:
If 1.00 mole of argon is placed in a 0.500-L container at 27.0 °C
Moles of argon = n = 1.00 mol
Volume of the container,V = 0.500 L
Ideal pressure of the gas = P
Temperature of the gas,T = 27 °C = 300.15 K[/tex]
Using ideal gas equation:
Vander wall's of equation of gases:
The real pressure of the gas= 
For argon:
b=0.03219 L/mol.
Difference :
2.0 atm is the difference between the ideal pressure and the real pressure.
Answer: 0.0725ppm
Explanation:
133.4g of MgBr2 dissolves in 1.84L of water.
Therefore Xg of MgBr2 will dissolve in 1L of water. i.e
Xg of MgBr2 = 133.4/1.84 = 72.5g
The concentration of MgBr2 is 72.5g/L = 0.0725mg/L
Recall,
1mg/L = 1ppm
Therefore, 0.0725mg/L = 0.0725ppm
The current condition in the troposhere is (C) The Atmosphere
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.
