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Question: How many moles of \[{O_2}\] are required to produce \[92.0grams\] of \[N{O_2}\]? \[2N{O_{(g)}} + {...

How many moles of O2{O_2} are required to produce 92.0grams92.0grams of NO2N{O_2}?
2NO(g)+O2(g)→2NO2(g)2N{O_{(g)}} + {O_{2(g)}} \to 2N{O_{2(g)}}

Explanation

Solution

At the point when atoms pick up or lose electrons to yield particles or join with different atoms to shape molecules, their symbols are adjusted or consolidated to create chemical equations that properly speak about these species. Stretching out this imagery to speak to both the personalities and the general amounts of substances going through a chemical (or physical) change includes composing and balancing a chemical equation.

Complete step-by-step answer:
The substances going through reaction are called reactants, and their formulas are put on the left half of the equation. The substances created by the reaction are called products, and their formulas are set on the correct sight of the equation. Additional signs (+) separate individual reactant and product formulas, and an arrow (→) separate the reactant and product (left and right) sides of the equation.

The overall quantities of reactant and product species are spoken to by coefficients (numbers put promptly to one side of every formula). A coefficient of one is commonly discarded and the coefficient basically represents the number of moles of that substance before which it is placed.

So, from the given equation we can conclude that to form two moles ofNO2N{O_2}, one mole of oxygen will be required.
The amount of NO2N{O_2} formed is 92.0grams92.0grams.
Molar mass of N{O_2}$$$$ = (14 + 16 \times 2)g = 46g
So, number of moles of NO2N{O_2} formed =9246=2moles = \dfrac{{92}}{{46}} = 2moles
And as we know that one mole of oxygen will be required to produce two moles of NO2N{O_2}.

So, the mole of oxygen required here is one mole.

Note: Despite the fact that chemical substances are separated and new compounds are shaped during a chemical reaction, molecules in the reactants don't vanish, nor do new atoms seem to frame the products. In chemical reactions, particles are rarely made or destroyed. The very atoms that were available in the reactants are available in the products—they are just rearranged into various arrangements. In a total chemical equation, the different sides of the equation should be available on the reactant and the product sides of the equation.