The metal content of iron in ores can be determined by a redox procedure in which the sample is first oxidized with br2 to convert all the iron to fe3+ and then titrated with sn2+ to reduce the fe3+ to fe2+.

the balanced equation is: 2fe3+(aq) + sn2+(aq) -> 2fe2+(aq) + sn4+(aq)

what is the mass percentage fe in a 0.1875g sample if 13.28 ml of 0.1015 m sn2+ solution is needed to titrate the fe3+?

80.27%

Explanation:

Let's consider the following balanced equation.

2 Fe³⁺(aq) + Sn²⁺(aq) ⇒ 2Fe²⁺(aq) + Sn⁴⁺(aq)

First, we have to calculate the moles of Sn²⁺ that react.

We also know the following relations:

Then, for 1.348 × 10⁻3 moles of Sn²⁺:

If there are 0.1505 g of Fe in a 0.1875 g sample, the mass percentage of Fe is:

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

a electronegativity decreases beacuse the size of nucleus is bigger.