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Determine the ratio of moles of iron actually used to moles of new product actually formed. Does this molar ratio agree with the ratio from the balanced chemical equation?​


equation 1.50g Cu 1 mole cu ÷ 63.5g Cu Fe ÷1 Cu 55.8gFe ÷ 1 mole = 1.32g Fe

Determine the ratio of moles of iron actually used to moles of new product actually formed Does this molar ratio agree with the ratio from the balanced chemical class=

Respuesta :

mickymike92

The mole ratio of iron to copper is 1 : 1, thus, 1.31 g of iron is required to produce 1.5 g of copper.

What is the equation of the reaction between iron and copper(ii) sulfate?

The reaction between iron and copper(ii) sulfate is a redox displacement reactions in which copper is displaced from its salt by iron.

The equation of the reaction is given below:

[tex]CuSO_4 + Fe \rightarrow FeSO_4 + Cu[/tex]

The mole ratio of both reactants and product is 1 : 1

  • moles = mass/molar mass

molar mass of copper sulfate = 160 g

molar mass of Cu = 64

molar mass of iron = 56 g

  • mole ratio of iron to copper = 1 : 1

moles of Cu in 1.5 g = 1.5/64 = 0.00234

mass of iron required = 0.00234 × 56 = 1.31 g of iron

Therefore, from the mole ratio of iron to copper, 1.31 g of iron is required to produce 1.5 g of copper.

Learn more about mole ratio at: https://brainly.com/question/19099163

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