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

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Chemistry

Ryleigh Collier

7 November, 02:45

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

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Patricia Hardy · 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.