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Question: In equation \( 2NO+{{O}_{2}}\to 2N{{O}^{2}} \) for each \( \left( 1.0 \right) \) mole of \( NO \) : ...

In equation 2NO+O2→2NO22NO+{{O}_{2}}\to 2N{{O}^{2}} for each (1.0)\left( 1.0 \right) mole of NONO : How many moles of O2{{O}_{2}} are consumed and of NO2N{{O}_{2}} produced? How many litres of each state condition)? How many grams of each?

Explanation

Solution

Hint : The mole is represented by the symbol mol. It is generally used as a unit of measurement for the amount of substance in the SI units where SI represents the International system of units. NO2(g)N{{O}_{2\left( g \right)}} is known by the name nitrogen dioxide.

Complete Step By Step Answer:
Molar mass of a chemical compound is defined as the mass of the sample chemical compound divided by the amount of the sample substance. The molar mass is generally measured in grams per mole represented as g/molg/mol .
The molar mass is also defined as the ratio of the mass of the substance to the number of particles present in it and it can be calculated by adding the standard atomic mass of the constituent atoms present in it. Molar mass also tells us the mass of one mole of substance. The balance chemical reaction is given by; NO(g)+12O2(g)→NO2(g)N{{O}_{(g)}}+\frac{1}{2}{{O}_{2(g)}}\to N{{O}_{2(g)}}
Now the stoichiometry indicates, that for each mole, each 30⋅g 30\cdot g~ of NO(g),N{{O}_{\left( g \right)}}, a half-mole quantity, 16g16g , of dioxygen gas reacts, to give a 46⋅g 46\cdot g~ mass of NO2(g).N{{O}_{2\left( g \right)}}.
And because the products and reactants are gaseous we could also say that each 2L2L of NO(g),N{{O}_{\left( g \right)}}, reacts with 1L1L dioxygen to gives a 2L2L volume of NO2(g).N{{O}_{2\left( g \right)}}. (because under the same conditions of temperature and pressure, volume is proportional to the molar quantity, i.e. V∝nV\propto n , which is old Avogadro's law.)
All of this relates to the given stoichiometry of the given reaction, which is stoichiometrically balanced with respect to mass and charge: 2NO+O2→2NO22NO+{{O}_{2}}\to 2N{{O}^{2}}
i.e. as written there are (2×30g)+32g=92g \left( 2\times 30g \right)+32g=92g~ of reactant, and necessarily 92g 92g~ of product.

Note :
Note that NO2(g).N{{O}_{2\left( g \right)}}. is used as an intermediate in the manufacturing of nitric acid as a nitrating agent in manufacturing of chemical explosives, as a sterilizing agent and as bleaching agent. It is somewhat toxic in nature and causes lung diseases.