Lead (II) nitrate as Pb(NO3)2 and potassium iodide as KI combine to form the products shown. 2 KNO3 + PbI2 How many moles of each reactant are involved in the reaction?   2 moles of lead (II) nitrate and 1 mole of potassium iodide 1 mole of lead (II) nitrate and 2 moles of potassium iodide 1 mole of lead (II) nitrate and 1 mole of potassium iodide 2 moles of lead (II) nitrate and 2 moles of potassium iodide

Al2O3 + 2Fe -------> Fe2O3 + 2Al   How many moles of Iron (III) oxide is produced from if 8.2 moles of Iron is used to react with aluminium oxide.

For the following chemical reactions, how do I identify the number of moles of the compound in the third column that would be produced from the number of moles of compound in the second column assuming that all of the other reactants in the equation in the first column are in excess.                   Reaction   Moles initially     Moles produced N2 + 3H2 → 2 NH3 0.027 moles N2 a.______moles NH3 5 C + 2 SO2 →CS2 + 4 CO 3.80 moles C b._______moles CO 5 C + 2 SO2 →CS2 + 4 CO 6.7 moles C c._______moles CS2

In the reaction 2NH3 + CO2 - -- > CO(NH2)2 + H2O, 8 moles of NH3 react with 8 moles of CO2, the obtained amount of CO(NH2)2 in moles will be: O 10 8. O 4 O 2