1.50 g of aluminium reacted with 35.0 cm3 of 1.00 mol dm–3 solution of copper(II) chloride, and 1.98 g of solid product was collected by filtration. Calculate the percentage yield for this reaction.

89.2%

Explanation:

The reaction of Al with CuCl₂ is:

2Al(s) + 3CuCl₂(aq) → 2AlCl₃(aq) + 3Cu(aq)

Assuming the reaction occurs until limiting reactant is over, we must find limiting reactant:

Moles Al -Molar mass: 26.98g/mol-

1.50g Al * (1mol / 26.98g) = 0.0556 moles

Moles CuCl₂:

35cm³ = 0.035L * (1.00mol / L) = 0.035 moles

For a complete reaction of Al there are necessaries:

0.0556 moles Al * (3 moles CuCl₂ / 2 moles Al) = 0.0834 moles of CuCl₂

As there are just 0.035 moles of CuCl₂, CuCl₂ is limiting reactant.

The solid produced is Cu, the theoretical mass of Cu is:

0.035 moles CuCl₂ * (3 moles Cu / 3 moles CuCl₂) = 0.035 moles Cu

0.035 moles Cu * (63.546g / mol) = 2.22g Cu

As actual yield was 1.98g, percentage yield is:

1.98g Cu / 2.22g Cu * 100 =

both adhesion and cohesion are attractions.

they are different in that adhesion is the force of attraction between the molecules of two different substances, whereas cohesion is the force of attraction between molecules of the same substance.

possible examples include capillary action, in which the adhesion between water and glass causes the water to rise in a narrow tube against the force of gravity.

because of hydrogen bonding, water is extremely cohesive.

this causes molecules on the surface of water to be drawn inward, which is why drops of water form beads on smooth surfaces.

hope this .