Question

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

Answer 1

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:

$CuSO_4 + Fe \rightarrow FeSO_4 + Cu$

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: brainly.com/question/19099163