Question

when 2 moles c and 1.5 moles O2 reacted, no residue remained. find the composition of product.

Answer 1

Answer:

Carbon  has  more  moles than oxygen which  has 0.5 moles less.When  we have fewer moles of oxygen  gas reacting with carbon, it  means oxygen will be   used completely  before all of  carbon reacts .

Therefore oxgyen is  behaves   as  a limiting agent  in reaction below:

2 moles of  carborn  +1.5 moles of oxygen =  ? moles of  caborn  (iv) oxide

writing a  balanced chemical  equation

C(s)   +   O₂(g) ⇒CO₂(g)

The  above  chemical  equation  is  balanced.It shows a  mole  ratio of 1:1

Since  carborn ( iv )oxide is  the product that is produced by a mole ratio of 1: 1 for  the  reactants,  the composition of  the product will equal to  1.5 moles of  oxygen  gas

Answer 2

The composition of the product will be 1.5 moles.

Given,

Number of moles of Carbon (C) = 2 moles

Number of moles of Oxygen $(O_{2} )$ = 1.5 moles

To Find,

The composition of the product formed

Solution,

Moles of Carbon is more than the moles of Oxygen by

$= (2-1.5) = 0.5 moles$

Since the number of moles of Carbon is higher than that of the Oxygen, we can infer that there will be no oxygen residue left and before the exhaustion of carbon, oxygen will get exhausted.

Therefore, in the given equation, oxygen is identified as the limiting agent.

The chemical equation is:

O$C(s) + O_{2} (g)$ ⇒ $CO_{2} (g)$

The molar ratio will be 1:1.

Since, the product that is formed, Carbon dioxide is also under the molar ratio of 1:1,

we can conclude that the product formed will have the composition of 1.5 moles of Oxygen.

Hence, the composition of the product formed will be 1.5 moles of Carbon dioxide.

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