Question

I'm stuck....please help

The equation for the reaction between Al(s) and Pb+2(aq) is:

2Al(s) + 3Pb+2(aq) 2Al+2(aq) + 3Pb(s)

Therefore, for each 2 moles of Al(s) that are used, how many moles of Pb(s) are formed?

From the 0.011 mole of Al(s) consumed, calculate the number of moles of Pb(s) that should have been formed: mole(s)

Answer 1

The balanced equation shows you that for 2 moles of Al you get 3 moles of Pb

Answer 2

Therefore, for each 2 moles of Al(s) that are used, how many moles of Pb(s) are formed? is it 3 and 0.017 Pb(s) have been formed.

Answer 3

\[\frac{2}{3}=\frac{.011}{x}\]

Answer 4

x=.0165

Answer 5

I got the same answer but the second one is not an answer i can choose from.... 149, 59, 0.017 and 0.0073