__ ch3ch2cooh(l) + __ o2(g)  __ co2(g) + __ h2o(l) how many moles of o2 are required to oxidize 1 mole of ch3ch2cooh according to the reaction represented above?

The given chemical equation represents the combustion reaction of propanoic acid:

On balancing we get,

The above balanced chemical equation tells us that, 2 mol require 7 mol for complete combustion to produce and

Given moles of = 1 mol

Calculating moles of required for combustion:

Therefore, 3.5 mol Oxygen is required for complete combustion of 1 mol propanoic acid.

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

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