Question

lead (ii) nitrate as $pb(no_{3})_{2}$ and potassium iodide as $ki$ combine to form the products shown.
$2kno3 + pbi_{2}$
how many moles of each reactant are involved in the reaction?
(1 point)
1 mole of lead (ii) nitrate and 1 mole of potassium iodide
2 moles of lead (ii) nitrate and 1 mole of potassium iodide
2 moles of lead (ii) nitrate and 2 moles of potassium iodide
1 mole of lead (ii) nitrate and 2 moles of potassium iodide

Explanation:

Step1: Write the balanced chemical equation

The reaction between lead (II) nitrate \(Pb(NO_3)_2\) and potassium iodide \(KI\) is a double - displacement reaction. The balanced chemical equation is \(Pb(NO_3)_2 + 2KI=2KNO_3 + PbI_2\)

Step2: Identify the moles of reactants

From the balanced chemical equation \(Pb(NO_3)_2 + 2KI = 2KNO_3+PbI_2\), we can see that the coefficient of \(Pb(NO_3)_2\) is \(1\) and the coefficient of \(KI\) is \(2\). In a chemical equation, the coefficients represent the number of moles of each reactant and product.

Answer:

1 mole of lead (II) nitrate and 2 moles of potassium iodide