Chemistry, 10.07.2019 21:00 chem1014

How to calculate the mass of iron in .275 grams of iron iii sulfate?

Answers: 2

Show answers

Answers

Answer from: Satoetoe24

Molar mass of iron(III)sulfate that is Fe₂(SO₄)₃ =399.88 g mol⁻¹

Mass given of iron(III)sulfate that is Fe₂(SO₄)₃= 0.275 g

Number of moles of iron(III)sulfate that is Fe₂(SO₄)₃= $\frac{0.275}{399.88}$

=0.00068 mol

there are two moles of Fe in 1 mole of Fe₂(SO₄)₃

So, in 0.00068 mol of Fe₂(SO₄)₃=2 ×0.00068 mol of Fe

= 0.00136 mol of Fe

molar mass of Fe=55.8 g mol⁻¹

So the mass of iron in 0.00136 mol of Fe= 55.8 g mol⁻¹ × 0.00136 mol

=0.075 g

Answer from: GaryCarmine

Mass of iron = 0.275 grams

The chemical formula of iron (III) sulfate = $Fe_{2}(SO_{4})_{3}$

First, calculate the number of moles of $Fe_{2}(SO_{4})_{3}$

Number of moles of iron (III) sulfate = $\frac{given mass in g}{molar mass}$

Molar mass of iron (III) sulfate = 399.88 g/mol

Number of moles of iron (III) sulfate = $\frac{0.275 g}{399.88 g/mol}$

= $6.87\times 10^{-4} mol$

In one mole of iron (III) sulfate there are two moles of iron according to the chemical formula.

So, in $6.87\times 10^{-4} mol$ of iron (III) sulfate there are = $2\times 6.87 \times 10^{-4} mol$ of iron.

Number of moles of iron = $13.74\times 10^{-4} mol$

Molar mass of iron = 55.8 g/mol

Mass of iron = $number of moles \times molar mass$

= $13.74\times 10^{-4} mol \times 55.8 g/mol$

= $766.692 \times 10^{-4} g$

= $7.66 \times 10^{-2} g$

Hence, mass of iron = $7.66 \times 10^{-2} g$

Answer from: Quest

Okay this will take 1 hour okay dont forget me.

Answer from: Quest

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and conduct electricity easily while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.

Another question on Chemistry

Chemistry, 22.06.2019 01:30

Arollercoaster car at the top of a hill has potential energy kinetic energy chemical energy light energy

Answers: 1

Answer

Chemistry, 22.06.2019 14:00

Calculate the energy required to ionize a hydrogen atom to an excited state where the electron is initially in the n = 5 energy level. report your answer in kilojoules

Answers: 1

Answer

Chemistry, 22.06.2019 20:10

The lattice enthalpy (formation of ionic solid from ions in the gas phase) for agcl(s) is -916 kj/mol and the hydration enthalpy (dissolution of gaseous ions into water) is -850 kj/mol. how much heat (in joules) is involved in forming 1l of saturated agcl solution (1.8 × 10-4 g / 100 ml water) by dissolving agcl(s)? assume solution volume does not change much upon dissolution. the equations are given below. ag+(g) + cl−(g) æ agcl(s)

Answers: 3

Answer

Chemistry, 22.06.2019 21:20

If a simple machine aduces the strength of a force, what must be increased? the speed of the input force the work the simple machine performs the size of the simple machine the distance over which the force is applied