Answer:
NH
3
acts as a Bronsted-Lower acid by giving its lone pair electrons.
Only in reaction 1 and 2 it acts as Bronsted-Lowry acid.
Explanation:
hope it's help you
The empirical formula will be CHCl
<h3>What is the empirical formula?</h3>
The simplest whole number ratio of atoms in a compound is the empirical formula of a chemical compound in chemistry. Sulfur monoxide's empirical formula, SO, and disulfur dioxide's empirical formula, S2O2, are two straightforward examples of this idea. As a result, both the sulfur and oxygen compounds sulfur monoxide and disulfur dioxide have the same empirical formula. They do not, however, have the same molecular formula, which specifies how many atoms are present in each molecule of a chemical compound.
For saran
C= 24.8% ,
H= 2.0% ,
Cl = 73.1%
= 24.8/ 12 = 2.0
= 2.0/1=2.0
= 73.1/ 35 = 2.0
Now, dividing each mole by the smallest moles (hydrogen's moles), one obtains:
C= 2.0 / 2.0 = 1
H= 2.0/2.0 = 1
Cl = 2.0/ 2.0 = 1
The empirical formula will be CHCl
Learn more about empirical formula here:-
brainly.com/question/14044066
#SPJ4
Take what you are given so 0.457g divide this by the molar mass (calculate this by taking the atomic weight of Na and Cl and add them together 23+35).
So 0.457gNaCl divide by (58g NaCl) = .0078 mol Nacl
<em><u>Larger molecules take longer to move up the chromatography paper or TLC plate, whereas smaller molecules are more mobile. Likewise, the polarity of the molecules can affect how far the spots travel, depending on the type of solvent used.</u></em>
![\large\sf\red{♡♡}](https://tex.z-dn.net/?f=%5Clarge%5Csf%5Cred%7B%E2%99%A1%E2%99%A1%7D)
Answer:
1.195 g of Arsenic.
Explanation:
Equation of the reaction:
Ga(l) + As(s) → GaAs(s).
Calculating the limiting reagent by:
Number of moles of:
Gallium:
Molar mass of Gallium = 69.7 g/mol.
Mass = 4 g
Number of moles = mass/molar mass
= 4/69.7
= 0.0574 mol.
Arsenic:
Molar mass of Arsenic = 75 g/mol.
Mass = 5.5 g
Number of moles = mass/molar mass
= 5.5/75
= 0.0733 mol
Therefore, using stoichiometry since 1 mole of Gallium reacted with 1 mole of Arsenic. The limiting reagent is Gallium.
Excess reagent is Arsenic.
Number of moles excess = 0.0733 - 0.0574
= 0.0159 moles
Mass of the excess Arsenic left =
Molar Mass * number of moles
= 0.0159 * 75
= 1.195 g of Arsenic.