How would each of the following change the rate of the reaction shown here? 2NO(

Question

How would each of the following change the rate of the reaction shown here? 2NO(g) + 2H2(g) -* N2(g) 2H20(g) A. -adding more NO This will cause no change to the rate of the reaction. B. Adding more reactant results in more reactant collisions, this increases the rate of the reaction. The temperature is lowered --,Some of the H2 is removed during the reaction C. The leads to an increases in the number of collisions among the reactants. The reaction rate will therefore decrease adding a catalyst Decreasing the energy also decreases the effective collisions of the for products to form. This wl decrease the rate of the reaction E. More reactant will collide resulting in an increase in the activation energy. This will decrease the rate of the reaction. This owers the activation energy for the reaction riin a decrease in the reaction rate. G.Less reactant will collide. Less collision will increase the rate of the reaction H. This will lower the energy of activation but now the reactants has more energy as they collide. These two factors will offset each other and there will be no change in the reaction rate. Decreasing the concentration of a reactant will decrease the number of collisions resulting in a decrease of the reaction rate J Increasing the number of reactant molecules will require more energy for the reaction to occur. The rate of reaction will therefore decreased. K. Decreasing the number of reactant molecules also decreases the energy necessary for the reaction to occur This results in an increase of the rate of the reaction. L. The rate of reaction will More reactant collide resulting in an increase in the activation energy. therefore increase M.This lowers the activation energy for the reaction resulting in an increase in the reaction rate Question 14 Given the following reaction at equilibriunm CaCO3 (s)--CaO (s) + CO2 (g) What would happen to the system if the total pressure were decrease by increasing the reaction vessel volume a. The direction of the equilibrium would shift to the left. b. The amount of CaCO3 would increase c. Less CO2(g) will form.

Explanation / Answer

question 13

Adding more NO: B

Temperature is lowered: D

Some of the H2 is removed during the reaction: I

Adding a catalyst: M

Question 14

d) The amount of CaO would increase.

If the equilibrium of a system is disturbed, the system will try to nullify the effect. (Le Chateleir's Principle)

In the effort to increase the pressure, the equilibrium shifts towards forward direction, producing more CO2 and CaO

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