Indium has 49 protons
mass number (# of neutrons and # of protons combined) is 115
115 - 49 = 66
66 neutrons
Answer:
3HC2H3O2(aq) + Al(OH)3(aq) --> AI(C2H3O2)3(aq) + 3H2O(l)
Explanation:
HC2H3O2 is the chemical formula for Ethanoic acid which can be written as CH3COOH.
Hence, the balanced equation is stated as 3CH3COOH(aq) + Al(OH)3(aq) --> AI(CH3COO)3(aq) + 3H2O(l)
Acid + base → Salt + Water.
The equation is a neutralization reaction in which the acid, aqeous CH3COOH reacts completely with an appropriate amount of base, aqueous Al(OH)3 to produce salt, aqueous AI(CH3COO)3(aq)
and water, liquid H2O only.
During this reaction, the hydrogen ion, H+, from the Ethanoic acid is neutralized by the hydroxide ion, OH-, from the Aluminum hydroxide to form the water molecule, H2O and aluminium ethanoate.
Thus, it is called a neutralization reaction.
Answer:
0.17 moles
Explanation:
In the elements of the periodic table, the atomic mass = molar mass. <u>Ex:</u> Atomic mass of Carbon is 12.01 amu which means molar mass of Carbon is also 12.01g/mol.
In order to find the # of moles in a 12 g sample of NiC-12, we will need to multiply the number of each atom by its molar mass and then add the masses of both Nickel and C-12 found in the periodic table:
- Molar Mass of Ni (Nickel): 58.69 g/mol
- Molar Mass of C (Carbon): 12.01 g/mol
Since there's just one atom of both Carbon and Nickel, we just add up the masses to find the molar mass of the whole compound of NiC-12.
- 58.69 g/mol of Nickel + 12.01 g/mol of Carbon = 70.7 g/mol of NiC-12
There's 12g of NiC-12, which is less than the molar mass of NiC-12, so the number of moles should be less than 1. In order to find the # of moles in NiC-12, we need to do some dimensional analysis:
- 12g NiC-12 (1 mol of NiC-12/70.7g NiC-12) = 0.17 mol of NiC-12
- The grams cancel, leaving us with moles of NiC-12, so the answer is 0.17 moles of NiC-12 in a 12 g sample.
<em>P.S. C-12 or C12 just means that the Carbon atom has an atomic mass of 12amu and a molar mass of 12g/mol, or just regular carbon.</em>
