I believe the answer is A the 1st one
Is true. Nitrogen gas behaves more like an ideal gas as the
temperature increases. Under normal conditions such as normal pressure and temperature
conditions , most real gases behave qualitatively as an ideal gas. Many
gases such as air , nitrogen , oxygen ,hydrogen , noble gases , and some heavy
gases such as carbon dioxide can be treated as ideal gases within a reasonable tolerance. Generally,
the removal of ideal gas conditions tends to be lower at higher temperatures and lower density (that is at lower pressure ), since the work made by the intermolecular
forces is less important compared to the kinetic energy<span> of the particles, and the size of the molecules is less important
compared to the empty space between them. </span><span>The ideal gas model
tends to fail at lower temperatures or at high pressures, when intermolecular
forces and intermolecular size are important.</span>
Answer:
The answer is C. The high solvation energy for LI+
Explanation:
LiF has lower solubility because of the high solvation energy of Li+ ion. This is due to the smaller size and very big charge compared to Cs+ ion which has a bigger size and solvent molecules easily surround it.
Solvation energy is simply the amount energy that is required to make a solute dissolve in a solvent.
The balanced equation for the above reaction is;
CH₄ + 2O₂ ---> CO₂ + 2H₂O
Stoichiometry of CH₄ to O₂ is 1:2
The number of methane moles present - 1.44 g/ 16 g/mol = 0.090 mol
Number of oxygen moles present - 9.5 g/ 32 g/mol = 0.30 mol
If methane is the limiting reagent,
0.090 moles of methane react with 0.090x 2 = 0.180 mol
only 0.180 mol of O₂ is required but 0.30 mol of O₂ has been provided therefore O₂ is in excess and CH₄ is the limiting reactant.
Number of moles of water that can be produced - 0.180 mol
Therefore mass of water produced - 0.180 x 18 g/mol = 3.24 g
Therefore mass of 3.24 g of water can be produced
