Identify the limiting and excess reactants when 1.00 g of zinc reacts with 150 mL of 0.250M Pb (NO3) 2. How many grams of lead are formed in this single replacement reaction

Question

Carter Bridges

Chemistry

21 November, 10:35

Identify the limiting and excess reactants when 1.00 g of zinc reacts with 150 mL of 0.250M Pb (NO3) 2. How many grams of lead are formed in this single replacement reaction

+4

Answers (1)

Know the Answer?

Corey Pham · Answer 1

The reaction equation is:

Zn + Pb (NO₃) ₂ → Pb + Zn (NO₃) ₂

The moles of lead are calculated using:

moles = concentration x volume

moles = 0.25 x 0.15

moles = 0.0375

The moles of zinc are: 1 / 65 = 0.015

We see from the equation that equimolar quantities of zinc and lead should be present. Therefore, lead is in excess and zinc is the limiting reactant.