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

Question

sergeinik [125]

3 years ago

5

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

Chemistry

1 answer:

Marysya12 [62] · Answer 1 · 2021-12-02T00:07:37+03:00

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.