Question

What is not a mole ratio of ${\text{6C}}{{\text{O}}_{\text{2}}}{\text{ + 6}}{{\text{H}}_{\text{2}}}{\text{O }} \to {\text{ }}{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ + 6}}{{\text{O}}_{\text{2}}}$?
(A) $\dfrac{{{\text{6 mole C}}{{\text{O}}_{\text{2}}}}}{{{\text{6 moles }}{{\text{H}}_{\text{2}}}{\text{O}}}}$
(B) $\dfrac{{{\text{6 moles }}{{\text{H}}_{\text{2}}}{\text{O}}}}{{{\text{6 moles }}{{\text{O}}_{\text{2}}}}}$
(C) $\dfrac{{{\text{6 moles C}}{{\text{O}}_{\text{2}}}}}{{{\text{1 mole }}{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}}}$
(D) $\dfrac{{{\text{6 mole }}{{\text{H}}_{\text{2}}}{\text{O}}}}{{{\text{mole }}{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}}}$
(E) $\dfrac{{{\text{6 mole C}}{{\text{O}}_{\text{2}}}}}{{{\text{6 mole }}{{\text{O}}_{\text{2}}}}}$

Answer 1

We first write a well-balanced equation of the reaction. Those coefficients of the reactants are the moles themselves that are reacting in it, the ratio of mole any of the reactants with another reactant or product or of product with product is called mole ratio.

Complete step by step answer:
First need of any chemical reaction is to be well balanced. So balancing the equation correctly will give the information of the reacting amounts. The co-efficient that are meant to balance an equation are the moles of the reactant reacting to form the moles of product. We get the information about the quantity of the reactants and the product according to the law of definite proportion. The chemical equation given in the question above is well balanced.
It says that ${\text{6}}$ moles of ${\text{C}}{{\text{O}}_{\text{2}}}$ reacts with ${\text{6}}$ moles of ${{\text{H}}_{\text{2}}}{\text{O}}$ to produce ${\text{1}}$ mole of ${{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}$ and ${\text{6}}$moles of ${{\text{O}}_{\text{2}}}$. So now we will make the ratio of the reactants and products
Ratio of ${\text{C}}{{\text{O}}_{\text{2}}}{\text{ : }}{{\text{H}}_{\text{2}}}{\text{O = 6 : 6}}$
Ratio of ${{\text{H}}_{\text{2}}}{\text{O : }}{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ = 6 : 1}}$
Ratio of ${\text{C}}{{\text{O}}_{\text{2}}}{\text{ : }}{{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ = 6 : 1}}$
Ratio of ${\text{C}}{{\text{O}}_{\text{2}}}{\text{ : }}{{\text{O}}_{\text{2}}}{\text{ = 6 : 6}}$
Ratio of ${{\text{H}}_{\text{2}}}{\text{O : }}{{\text{O}}_{\text{2}}}{\text{ = 6 : 6}}$
Ratio of ${{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}{{\text{O}}_{\text{6}}}{\text{ : }}{{\text{O}}_{\text{2}}}{\text{ = 1 : 6}}$

So, the correct answer is Option D .

Note: when we know the moles of the reaction, we can do the reaction when any weight of the reactant is given and predict the amount of other reactant needed and the amount of product produced.
The ratio of moles gives most of the information about the amount of product form in mass because of ${\text{moles = }}\dfrac{{{\text{given weight}}}}{{{\text{molecular weight}}}}$.
By this formula we can easily find the molar mass of an unknown product or the weight of the product form in the reaction.