In the following reaction, what is the relationship between the rate at which the nitrous oxide is used up, the rate at which the oxygen is used, and the rate at which the nitrogen dioxide is produced? 2n2o(g)+ 3o2(g) → 4no2(g)

Answer :

The relationship between the rate at which the nitrous oxide is used :

The relationship between the rate at which the oxygen is used :

The relationship between the rate at which the nitrogen dioxide is used :

Explanation :

The general rate of reaction is,

Rate of reaction : It is defined as the change in the concentration of any one of the reactants or products per unit time.

The expression for rate of reaction will be :

From this we conclude that,

In the rate of reaction, A and B are the reactants and C and D are the products.

a, b, c and d are the stoichiometric coefficient of A, B, C and D respectively.

The negative sign along with the reactant terms is used simply to show that the concentration of the reactant is decreasing and positive sign along with the product terms is used simply to show that the concentration of the product is increasing.

Now we have to determine the expression for rate of reaction.

The balanced chemical equations is:

The relationship between the rate at which the nitrous oxide is used :

The relationship between the rate at which the oxygen is used :

The relationship between the rate at which the nitrogen dioxide is used:

n has four pairs of electrons in the valence shell, electrons repel one another ,n has 7 protons in its nucleus, and since n has 7 protons, it must fill the second shell, giving it 4 pairs of electrons. the electrons form 3 bonds and 1 lone pair of electrons. each pair of electrons repels the other pairs, so they are equally far apart.

so all of the above

the correct answer is answer a. a mixture

no other options make sense

hope this

have a great day : )

  - sprinkles