Heating 2.40 g of the oxide of metal x (molar mass of x = 55.9 g/mol) in carbon monoxide (co) yields the pure metal and carbon dioxide. the mass of the metal product is 1.68 g. from the data given, show that the simplest formula of the oxide is x2o3 and write a balanced equation for the reaction.

The molecular formula of the oxide of metal be . The balanced equation for the reaction is given by:

Explanation:

Let the molecular formula of the oxide of metal be

Mass of metal product = 1.68 g

Moles of metal X =

1 mol of metal oxide produces 2 moles of metal X.

Then 0.03005 moles of metal X will be produced by:

of metal oxide

Mass of 0.01502 mol of metal oxide = 2.40 g (given)

y = 2.999 ≈ 3

The molecular formula of the oxide of metal be . The balanced equation for the reaction is given by:

ljjjljlj kjlk,ljym jlyu; jm; l mumytj

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.