Look at this reaction:
3NO(g) ⇆ N2O(g) + NO2(g)
Keq = 1.8×10^(18) (at 298 K),
△H° = -155 kJ/mol.
Which of the following statements about this reaction is not correct?

a) ΔS < 0 because there is more order in the products than in the reactants.
b) This is an endothermic reaction.
c) The products are heavily favored at room temperature.
d) At a higher temperature, products would be less favored than at room temperature.

The correct option is;

b) This is an endothermic reaction

Explanation:

To answer the question, we analyze each of the options as follows;

a) ΔS < 0 because there is more order in the products than in the reactants.

The above statement is correct as there are fewer molecules in the product than in the reactants

b) This is an endothermic reaction.

The heat of the reaction is △H° = -155 kJ/mol which is negative, suggestive of an exothermic reaction, therefore the above equation is not correct

c) The products are heavily favored at room temperature.

Based on the high value of keq at 298 K the above statement is correct

d) At a higher temperature, products would be less favored than at room temperature.

The above statement is true as the amount of heat produced will be returned bck to the system tending to reverse the reaction.

they both have a y in them

question: ray weighs 100 kilograms, his wrestling partner, bobby, weighs 50 kilograms. if ray moves at 4 m s , how fast will bobby have to run at him to apply an equal amount of kinetic energy?

answer: 8 m/s he needs to run twice as fast to keep up so he has some work to do

explanation:   if the mass has units of kilograms and the velocity of meters per second, the kinetic energy has units of kilograms-meters squared per second squared.

question answered by

(jacemorris04)