According to the equation, 2Al(s) + 6H2O(l) + 2KOH(aq) to make 2K[Al(OH)4](aq) + 3H2(g). How many grams of hydrogen gas would be formed in the reaction of 1.15 grams of Al and excess KOH?

0.06457g of H₂

Explanation:

2Al(s) + 6H₂O(l) + 2KOH(aq) → 2K[Al(OH)₄](aq) + 3H₂(g)

Based on the equation 2 moles of Al produce 3 moles of hydrogen.

First, we need to convert mass of Al to moles and then with the chemical equation find moles and mass of hydrogen:

Moles Al (Molar mass: 26.982g/mol):

1.15g Al * (1mol / 26.982g) = 0.04262 moles Al

Moles H₂:

0.04262 moles Al * (3 moles H₂ / 2 mol Al) = 0.06393 moles H₂

Mass hydrogen (Molar mass: 1.01g/mol):

0.06393 moles H₂ * (1.01g/mol) =

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 .

the increase of protons   hope this