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)

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 =

For  0.011 mole of Al(s) consumed no. of moles of Pb(s) produced :

Thus 0.0165 moles of Pb(s) that should have been formed From the 0.011 mole of Al(s) consumed .

3 moles of Pb(s) formed for each 2 moles of Al(s) consumed

0.0165 moles of Pb(s)should have been formed when 0.011 moles of Al(s) consumed

Step-by-step explanation:

We are given that the equation for the reaction between Al(s) and Pb+2(aq) is

given below:

2 moles of Al(s) consumed then number of Pb(s) formed=3 moles

1 mole of Al(s) consumed then number of Pb(s) formed= moles

0.011 moles of Al(s) consumed then number of moles of Pb(s) formed=

3 moles of Pb(s) formed when 2 mole of Al(s) consumed

0.0165 moles of Pb(s) should have been formed when 0.011 moles of Al(s) consumed

it is true

step-by-step explanation:

all the combinations add up i used   calculator