When 4.0 mol h2o react with 4.0 mol al in the reaction below, 2.7 mol of al are used up in the reaction. how many moles of al are left over unreacted?

2 al + 3 h2o → al2o3 + 3h2 (c? )

2.7 mol al left over

2.0 mol al left over

1.3 mol al left over

0.7 mol al left over

Answer : The moles of Al left over unreacted are, 1.3 mole

Explanation : Given,

The total moles of Al are taken in this reaction = 4.0 mole

The moles of Al used in this reaction = 2.7 mole

Now we have to calculate the moles of Al are left over unreacted.

The moles of Al are left over unreacted = The total moles are taken in this reaction - The moles of Al used in this reaction

The moles of Al are left over unreacted = 4.0 mole - 2.7 mole = 1.3 mole

Therefore, the moles of Al left over unreacted are, 1.3 mole

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.