Question

How many moles of MNo3 are produced when 4.30 kg of oxygen gas completely reacts according to the balanced chemical reaction: 2Mn(s) 3O₂(g) → 2Mno₃(s)

a. 0.25 mol
b. 0.50 mol
c. 1.00 mol
d. 2.00 mol

Answer 1

The calculation based on the provided chemical equation results in 89.5833 moles of MnO3 produced from 4.30 kg of oxygen, which does not match any of the provided options.

Step-by-step explanation:

To determine the number of moles of MnO3 produced from 4.30 kg of oxygen, we must first correct the provided chemical equation as it appears to have a typo. The likely correct form of the equation (based on stoichiometric logic and common compounds) would be:

2Mn(s) + 3O2(g) → 2MnO3(s) First, we convert the mass of oxygen to moles: 4.30 kg O2 × (1000 g / 1 kg) × (1 mol O2 / 32.00 g O2) = 134.375 mol O2

Then we use the stoichiometric relationship from the balanced equation: 3 mol O2 produce 2 mol MnO3

So, (134.375 mol O2) × (2 mol MnO3 / 3 mol O2) = 89.5833 mol MnO3

The answer does not match any of the provided options, indicating either the question or the choices may be incorrect.