Can someone please tell me which ones are true! There\'s a lot of different answ
ID: 858435 • Letter: C
Question
Can someone please tell me which ones are true! There's a lot of different answers I'm getting Modesto Junior College - CHEM 143-Fall14-PANDEY: HW 16 ms/mod/ibis/view.php?id=1407587 Caloulator Calculator Periodic Table 1 of 16 Incorrect Mapd Chemical reactions occur when molecules or atoms collide, the bonds between atoms are broken, and new bonds are formed. Breaking the bonds of the reactants requires energy; bond formation releases energy Which of the following statements regarding energy changes during a reaction are true? Decreasing the temperature decreases the kinetic energy of the reactants, and the reaction goes When the activation energy is high, the reaction rate is fast. Increasing the amount of reactants creases the number o co sions, and the reaction goes more faster The activation e nerg (Ea) is the energy difference between the energy of the products and the energy of the reactants. Reactants must collide, with proper orientation with energy greater than or equal to the activation energy for a reaction to occur If the energy of the products is lower than the energy of the reactants, the reaction is endothermic. r The energy of a collision between atoms or molecules must be greater than or equal to thie activation energy (E.) for bonds tobe broken. O Prenous Give Up & View Solution ) Check Answer ) Next a ExitExplanation / Answer
As the temprature decreases, the kinetic energy of the reactants decreases. This decreases the number of effective collisions Hence, the reaction becomes slow. Thus this statement is true.
Whn the activation energy is high, the fraction of molecules possesing energy equal to or greater than the activation energy is low. Hence, the reaction rate is slow. Thus, the statement is false.
When the concentration of the reactants is increased, the number of collisions increases. Hence, the reaction becomes faster.
The activation energy is the difference between the energy of the transition state and the energy of the reactants. hence, the statement is false.
When reactants have proper orientation and energy greater than or equal to the activation energy, they make effective collisions and the reaction occurs. Hence, the statement is true.
When the energy of the products is lower than the energy of the reactants, the reaction is exothermic. Hence, the statement is false.
When the energy of collision is greter than or equal to the activation energy for the bonds to be broken, the collision will be effective. Hence the statement is true.