Answer:
For each 2 moles of Al(s) that are used, 3 moles of Pb(s) are formed.
0.0165 moles of Pb(s) that should have been formed From the 0.011 mole of Al(s) consumed
Step-by-step explanation:
Given :
The equation for the reaction between Al(s) and Pb+2(aq) is:
2Al(s) + 3Pb+2(aq) 2Al+2(aq) + 3Pb(s)
To find: 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)
Solution:
Now to calculate the how many moles of Pb(s) are formed for each 2 moles of Al(s) that are used
Consider the given equation.
So, we can see that for each 2 moles of Al(s) that are used, 3 moles of Pb(s) are formed.
Now , for 2 moles of Al(s) no. of moles of Pb(s) produced = 3
For 1 moles of Al(s) no. of moles of Pb(s) produced = \(\frac{3}{2}\)
For 0.011 mole of Al(s) consumed no. of moles of Pb(s) produced :
\(\frac{3}{2} \times 0.011\)
\(0.0165\)
Thus 0.0165 moles of Pb(s) that should have been formed From the 0.011 mole of Al(s) consumed .
