Solid aluminum (Al) and chlorine (C1,) gas react to form solid aluminum chloride (A1CI2). Suppose you have 7.0 mol of Al and 1.0 mol of Cl, in a reactor. Suppose as much as possible of the Al reacts. How much will be left? Round your answer to the nearest 0.1 mol.

6.3 moles

Explanation:

From the balanced equation of reaction:

2 moles of aluminium reacts with 3 moles of chlorine gas to form 2 moles of AlCl3.

Therefore, 1 mole of chlorine will require: 2 x 1/3 = 0.67 mole of aluminium.

Hence, 0.67 mole of aluminium will be needed for 1 mole of chlorine. If 7 moles of aluminium is present, then:

   7 - 0.67 = 6.33 moles of aluminium will be left.

To the nearest 0.1, it means 6.3 moles of aluminium will be left.

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

indium, and thallium have three electrons i think