Question

calculate how many moles of NO₂ form when each quantity of reactant completely reacts.

2N₂O₅(g)--->4NO₂(g)+O₂(g)

a.   2.5 mol N₂O₅                    b.     6.8 mol  N₂O₅     

c.   15.2 g N₂O₅                      d.     2.87  kg  N₂O₅                                                                                       

Answer 1

Concepts and reason

Balanced chemical equation:

• Balanced chemical equation for a reaction is an equation which obeys the law of conservation of mass. From the balanced chemical equation, reaction to a product ratio can be calculated.

Law of conservation of mass:

• This law indicates that in the chemical reaction, mass is neither created nor destroyed.

Fundamentals

Balanced chemical equation:

This equation indicates that “a” moles of R (reactant) reacts with B and forms b moles of P (product).

Mole concept: The number of moles of the substance is the simple ratio of the mass to the molar mass of that substance.

Molar mass= Mass of a 1 molar substance is known as molar mass of a compound.

(a)

The given balanced chemical equation is shown below.

From the equation, it is clear that 2moles of are decomposed to 4moles of and 1mole of oxygen.

If,

2.5moles of is used in the reaction and by assuming the complete consumption of in the reaction, the number of moles of produced is expressed below:

(b)

Given balanced chemical equation is shown below.

From the equation, 2moles of are decomposed to 4moles of and 1mole of oxygen.

If,

6.8moles of is used in the reaction and by assuming the complete consumption of in the reaction, the number of moles of produced is expressed below:

(c)

Given balanced chemical equation is shown below.

From the equation. 2moles of are decomposed to 4moles of and 1mole of oxygen.

If,

15.2 grams of is used in the reaction and by assuming the complete consumption of in the reaction, the number of moles of used is expressed below:

(d)

The given balanced chemical equation is shown below.

From the equation, it is clear that 2moles of are decomposed to 4moles of and 1mole of oxygen.

If,

2.87kg of is used in the reaction and by assuming the complete consumption of in the reaction, the number of moles of is expressed below.

Ans: Part a

The number of moles of produced is 5.

Part b

The number of moles of produced is 13.6.

Part c

The number of moles of produced is 0.282.

Part d

The number of moles of produced is 53.16.