For the reaction, X + Y → A + B, ΔGo is –1324 kJ. Which one of the following statements is NOT valid concerning the reaction?
a. The reaction is spontaneous as written.
b. Three of these statements are valid.
c. The reaction will proceed rapidly from left to right.
d. The reaction is thermodynamically favorable.
e. The products are more stable than the reactants.

c. The reaction will proceed rapidly from left to right.

Explanation:

The variation of the free Gibbs energy doesn't tell anything about the speed of reaction.

On the other hand, when ΔGo is negative: the reaction is spontaneous, thermodynamically favourable, and the products are more stable than the reactants

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)