solution volume to mass

Question

0.110L of 0.260M Pb(NO3)2 reacts with excess K2CrO4. How may grams are produced.

Answer 1

First, write the balanced equation:

Pb(NO3)2 + K2CrO4 ==> 2KNO3 + PbCrO4(s)

 

Since KcCrO4 is in excess, the amount of product will depend only on moles of Pb(NO3)2 present

moles Pb(NO3)2 = 0.110 L x 0.260 moles/L = 0.0260 moles

 

moles PbCrO4 produced = 0.0260 moles since mole ratio in balanced equation is 1:1

mass PbCrO4 produced = 0.0260 moles x 323 g/mole = 9.24 grams

 

moles KNO3 produced = 0.0260 moles Pb(NO3)2 x 2 moles KNO3/1 mole Pb(NO3)2 = 0.052 moles

mass KNO3 produced = 0.052 moles x 101 g/mole = 5.25 grams