17kg of aluminium was produced from 51kg of aluminium oxide (al2o3) by electrolysis. what was the percentage yield?

Consider this reaction : 2Al2O3 → 4Al + 3O2

The number of moles of Al2O3 can be determined from its mass →

Number of moles of AL2O3 = mass/molar mass

                                               =51/(27x2+16x3)

                                               = 0.5 mol

Now, calculate aluminium's number of moles from the mole ratio →

Mole ratio  4(Al) : 2(Al2O3)

Number of moles of Al = (4/2) x0.5mol = 1 mol

Mass of Al = number of moles x molar mass

                                   = 1x27

                                   = 27kg (theoretical yield)

Given, actual yield = 17kg

Therefore, percentage yield = (actual yield / theoretical yield ) x 100

                             = (17/27)x100

                               = 62.96%

yes, water is wet, just as it makes other things wet, it is wet itself, kinda like ice, when ice is in water, the ice makes water cold, and ice is cold, therefore with that example, water is wet

it's all four options.