If 3.0 grams of H2 were produced from the following reaction, how many grams of Al reacted?
2AI + 6HCI --->2AIC3 + 3H2

Note the following:
molar mass of Al = 27 g/mol
molar mass of H = 1.0 g/mol
molar mass of Cl = 35.5 g/mol

27g of Al

Explanation:

2AI + 6HCI —> 2AIC3 + 3H2

molar mass of Al = 27 g/mol

Mass conc of Al from the balanced equation = 2 x 27 = 54g

Molar Mass of H2 = 2x1 = 2g/mol

Mass conc of H2 from the balanced equation = 3 x 2 = 6g

From the equation,

54g of Al produced 6g of H2.

Therefore, Xg of Al will produce 3g of H2 i.e

Xg of Al = (54x3)/6 = 27g

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.

level 4 to level 2 : ))