Answer:
Fe₂O₃
Explanation:
To solve this question we must find the moles of Iron in 1.68g. With the difference of the masses we can find the moles of oxygen. The formula will be obtained with the ratio of both amount of moles:
<em>Moles Fe:</em>
1.68g * (1mol / 56g) =0.03moles
<em>Moles O:</em>
2.40g-1.68g = 0.72g * (1mol/16g) = 0.045moles
The ratio O/Fe is:
0.045moles / 0.03moles = 1.5 moles. this ratio is obtained if the formula is:
<h3>Fe₂O₃</h3>
The atomic mass of element is the weighted average atomic mass of the element with respect to the abundance of the isotopes of that element
atomic mass is the sum of the products of the mass of isotopes by their percentage abundance
atomic mass = 15.000 amu x 5.000 % + 16.000 amu x 95.000 %
= 0.7500 + 15.200
atomic mass of element is therefore 15.950
Explanation:
(a) The given reaction equation is as follows.
(acidic)
So, here the reduction and oxidation-half reactions will be as follows.
Oxidation-half reaction: 
Reduction-half-reaction: 
As total charge present on reactant side is -1 and total charge present on product side is +3. And, since it is present in aqueous medium. Hence, we will balance the charge for this reaction equation as follows.
(acidic)
(b) The given reaction equation is as follows.
(basic)
So, here the reduction and oxidation-half reactions will be as follows.
Reduction-half reaction: 
Oxidation-half reaction: 
Hence, to balance the number of electrons in this equation we multiply it by 4 as follows.

Therefore, balancing the whole reaction equation in the basic medium as follows.
Answer:
25 ml of stock
Explanation:
Molarity x Volume of Concentrated Stock = Molarity x Volume of Diluted Stock
=> Mc x Vc = Md x Vd => (0.5M)(x) = (0.25M)(50 ml)
=> x = Vc = (0.25M x 50 ml) / (0.50M) = 25 ml of stock