Filtration because of the chemicals needed to spread them
<h3> Part A</h3>
The molar mass of silver = 107.87 g/mol ( <em>from periodic table)</em>
<h3>
part B</h3>
The moles of silver is 0.2946 moles
<u><em>calculation</em></u>
moles =mass÷ molar mass
= 31.78 g ÷ 107.87 =0.2946 moles
<h3>part c</h3>
The number of atoms of silver that are in this sample is 1.773 x 10²³ atoms
<u><em>calculation</em></u>
According to Avogadro's law 1 mole = 6.02 x 10²³ atoms
0.2946 moles= ? atoms
by cross multiplication
= [ (0.2946 moles x 6.02 x 10²³ ) / 1 mole] = 1.773 x 10²³ atoms
calorimeter<span> is a device used to measure the amount of heat involved in a chemical or physical process. For example, when an exothermic reaction occurs in solution in a calorimeter, the heat produced by the reaction is absorbed by the solution, which increases its temperature. When an endothermic reaction occurs, the heat required is absorbed from the thermal energy of the solution, which decreases its temperature (</span>[link]<span>). The temperature change, along with the specific heat and mass of the solution, can then be used to calculate the amount of heat involved in either case.</span>
The percent ionic character is a quantity that measure how ionic the bond is. To scale, a perfect ionic bond would have 100% ionic character, while a perfect covalent bond would have 0% ionic character. What makes a bond ionic? An ionic bond is the bonding of a cation and anion together that complete their individual state by reacting their extra valence electrons. The stronger the ionic bond, the greater the electronegativity of the atoms are. Electronegativity is the ability of the atom to attract electrons toward itself. So, the formula for percent ionic character is:
percent ionic character =
where
x^Be is the electronegativity of Beryllium equal to 1.57
x^F is the electronegativity of Fluorine equal to 3.98
percent ionic character =
percent ionic character = 45.26%
The boiling point is defined as the temperature...
The boiling point is defined as the temperature at which the vapor pressure of the liquid is equal to the ambient pressure, and bubbles of vapor form directly in the liquid. The normal boiling point is specified when the ambient pressure is 1 atm
Of course, if we reduce the ambient pressure, the boiling point will substantially be reduced, and this is the example of the principle of vacuum distillation, where an otherwise in volatile liquid is distilled under high vacuum.
